We prepare a solution by mixing 0.10 L of 0.12 M sodium chloride with 0.23 L of a 0.18 M

Calculate the molarity of each solution. a. 3.25 mol of LiCl in 2.78 L solution b. 28.33 g C6H12O6 in 1.28 L of solution c. 32.4 mg NaCl in 122.4 mL of solution

Calculate the molarity of each solution. a. 0.38 mol of LiNO3 in 6.14 L of solution b. 72.8 g C2H6O in 2.34 L of solution c. 12.87 mg KI in 112.4 mL of solution

What is the molarity of NO3 - in each solution? a. 0.150 M KNO3 b. 0.150 M Ca(NO3)2 c. 0.150 M Al(NO3)3

What is the molarity of Cl- in each solution? a. 0.200 M NaCl b. 0.150 M SrCl2 c. 0.100 M AlCl3

Problem 57E How many moles of KCl are contained in each solution? a. 0.556 L of a 2.3 M KCl solution b. 1.8 L of a 0.85 M KCl solution c. 114 mL of a 1.85 M KCl solution

What volume of 0.200 M ethanol solution contains each amount in moles of ethanol? a. 0.45 mol ethanol b. 1.22 mol ethanol c. 1.2 x 10-2 mol ethanol

A laboratory procedure calls for making 400.0 mL of a 1.1 M NaNO3 solution. What mass of NaNO3 (in g) is needed?

A chemist wants to make 5.5 L of a 0.300 M CaCl2 solution. What mass of CaCl2 (in g) should the chemist use?

Problem 61E If 123 mL of a 1.1 M glucose solution is diluted to 500.0 mL, what is the molarity of the diluted solution?

If 3.5 L of a 4.8 M SrCl2 solution is diluted to 45 L, what is the molarity of the diluted solution?

To what volume should you dilute 50.0 mL of a 12 M stock HNO3 solution to obtain a 0.100 M HNO3 solution?

To what volume should you dilute 25 mL of a 10.0 M H2SO4 solution to obtain a 0.150 M H2SO4 solution?

Consider the reaction: What volume of 0.150 M Li2S solution is required to completely react with 125 mL of 0.150 M Co(NO3)2?

What is the minimum amount of 6.0 M H2SO4 necessary to produce 25.0 g of H2 (g) according to the reaction between aluminum and sulfuric acid?

What is the molarity of ZnCl2 that forms when 25.0 g of zinc completely reacts with CuCl2 according to the following reaction? Assume a final volume of 275 mL.

A 25.0 mL sample of a 1.20 M potassium chloride solution is mixed with 15.0 mL of a 0.900 M barium nitrate solution and this precipitation reaction occurs: The solid BaCl2 is collected, dried, and found to have a mass of 2.45 g. Determine the limiting reactant, the theoretical yield, and the percent yield.

A 55.0 mL sample of a 0.102 M potassium sulfate solution is mixed with 35.0 mL of a 0.114 M lead(II) acetate solution and this precipitation reaction occurs: The solid PbSO4 is collected, dried, and found to have a mass of 1.01 g. Determine the limiting reactant, the theoretical yield, and the percent yield.

For each compound (all water soluble), would you expect the resulting aqueous solution to conduct electrical current? a. CsCl b. CH3OH c. Ca(NO2)2 d. C6H12O6

Classify each compound as a strong electrolyte or nonelectrolyte. a. MgBr2 b. C12H22O11 c. Na2CO3 d. KOH

Determine whether each compound is soluble or insoluble. If the compound is soluble, list the ions present in solution. a. AgNO3 b. Pb(C2H3O2)2 c. KNO3 d. (NH4)2S

Determine whether each compound is soluble or insoluble. For the soluble compounds, list the ions present in solution. a. AgI b. Cu3(PO4)2 c. CoCO3 d. K3PO4

Complete and balance each equation. If no reaction occurs, write “NO REACTION.” a. LiI(aq) + BaS(aq) ? b. KCl(aq) + CaS(aq) ? c. CrBr2(aq) + Na2CO3(aq) ? d. NaOH(aq) + FeCl3(aq) ?

Complete and balance each equation. If no reaction occurs, write “NO REACTION.” a. NaNO3(aq) + KCl(aq) ? b. NaCl(aq) + Hg2(C2H3O2)2(aq) ? c. (NH4)2SO4(aq) + SrCl2(aq) ? d. NH4Cl(aq) + AgNO3(aq) ?

Problem 77E Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write “NO REACTION.” a. potassium carbonate and lead(II) nitrate b. lithium sulfate and lead(II) acetate c. copper(II) nitrate and magnesium sulfide d. strontium nitrate and potassium iodide

Problem 78E Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write “NO REACTION.” a. sodium chloride and lead(II) acetate b. potassium sulfate and strontium iodide c. cesium chloride and calcium sulfide d. chromium(III) nitrate and sodium phosphate

Write balanced complete ionic and net ionic equations for each reaction.

Write balanced complete ionic and net ionic equations for each reaction.

Mercury(I) ions (Hg22+) can be removed from solution by precipitation with Cl-. Suppose that a solution contains aqueous Hg2(NO3)2. Write complete ionic and net ionic equations to show the reaction of aqueous Hg2(NO3)2 with aqueous sodium chloride to form solid Hg2Cl2 and aqueous sodium nitrate.

Problem 82E Lead(II) ions can be removed from solution by precipitation with sulfate ions. Suppose that a solution contains lead(II) nitrate. Write complete ionic and net ionic equations to show the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate.

Problem 83E Write balanced molecular and net ionic equations for the reaction between hydrobromic acid and potassium hydroxide.

Problem 84E Write balanced molecular and net ionic equations for the reaction between nitric acid and calcium hydroxide.

Complete and balance each gas-evolution equation.

Problem 91AE: Uranium hexafluoride, UF6, is processed to produce fuel for nuclear reactors and nuclear weapons. UF6 is made from the reaction of elemental uranium with CIF3, which also produces CI2 as a by-product. (a) Write the balanced molecular equation for the conversion of U and CIF3 into UF6 and CI2. (b) Is this a metathesis reaction? (c) Is this a redox reaction?

The accompanying photo shows the reaction between a solution of \(\mathrm{Cd}\left(\mathrm{NO}_{3}\right)_{2}\) and one of \(\mathrm{Na}_2\mathrm{S}\). (a) What is the identity of the precipitate? (b) What ions remain in solution? (c) Write the net ionic equation for the reaction, (d) Is this a redox reaction?

Problem 93: Suppose you have a solution that might contain any or all of the following cations: Ni2+, Ag+ Sr2+, and Mn2+. Addition of HCI solution causes a precipitate to form. After filtering off the precipitate, H2S04 solution is added to the resulting solution and another precipitate forms. This is filtered off, and a solution of NaOH is added to the resulting solution. No precipitate is observed. Which ions are present in each of the precipitates? Which of the four ions listed above must be absent from the original solution?

Problem 94: You choose to investigate some of the solubility guidelines for two ions not listed in Table the chromate ion (CrO4 2-) and the oxalate ion (C2O42 -). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts:

Problem 95: Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the aqueous HCI in the stomach and each of the following substances used in various antacids: (a) AI(OH)3(s), (b) Mg(OH)2(s), (c) MgCO3(s), (d) NaAI(CO3)(OH)2(s), (e) CaCO3(s).

Problem 96AE The commercial production of nitric acid involves the following chemical reactions: (a) Which of these reactions are redox reactions?(b) In each redox reaction identify the element undergoing oxidation and the element undergoing reduction, (c) How many grams of ammonia must you start with to make 1000.0 L of a 0.150 M aqueous solution of nitric acid? Assume all the reactions give 100% yield.

Problem 97AE: Consider the following reagents: zinc, copper, mercury (density 13.6 g/mL), silver nitrate solution, nitric acid solution, (a) Given a 500-mL Erlenmeyer flask and a balloon, can you combine two or more of the foregoing reagents to initiate a chemical reaction that will inflate the balloon? Write a balanced chemical equation to represent this process. What is the identity of the substance that inflates the balloon? (b) What is the theoretical yield of the substance that fills the balloon? (c) Can you combine two or more of the foregoing reagents to initiate a chemical reaction that will produce metallic silver? Write a balanced chemical equation to represent this process. What ions are left behind in solution? (d) What is the theoretical yield of silver?

Problem 98: Lanthanum metal forms cations with a charge of 3+. Consider the following observations about the chemistry of lanthanum: When lanthanum metal is exposed to air, a white solid (compound A) is formed that contains lanthanum and one other element. When lanthanum metal is added to water, gas bubbles are observed and a different white solid (compound B) is formed. Both A and B dissolve in hydrochloric acid to give a clear solution. When either of these solutions is evaporated, a soluble white solid (compound C) remains. If compound C is dissolved in water and sulfuric acid is added, a white precipitate (compound D) forms, (a) Propose identities for the substances A, B, C, and D. (b) Write net ionic equations for all the reactions described. (c) Based on the preceding observations, what can be said about the position of lanthanum in the activity series (Table)? Table Activity Series of Metals in Aqueous Solution

Problem 99 A 35.0-mL sample of 1.00 M KBr and a 60.0-mL sample of 0.600 M KBr are mixed. The solution is then heated to evaporate water until the total volume is 50.0 ml. How many grams of silver nitrate are required to precipitate out silver bromide in the final solution?

Problem 100AE: Using modern analytical techniques, it is possible to detect sodium ions in concentrations as low as 50 pg/mL. What is this detection limit expressed in (a) molarity of Na+, (b) the number of Na+ ions per cubic centimeter of solution, (c) the mass of sodium per 1000 L of solution?

Problem 101: Hard water contains Ca2+, Mg2+, and Fe2+, which interfere with the action of soap and leave an insoluble coating on the insides of containers and pipes when heated. Water softeners replace these ions with Na+. Keep in mind that charge balance must be maintained, (a) If 1500 L of hard water contains 0.020 M Ca2+ and 0.0040 M Mg2+, how many moles of Na+ is needed to replace these ions? (b) If the sodium is added to the water softener in the form of NaCI, how many grams of sodium chloride are needed?

Problem 102: Tartaric acid, H2C4H406, has two acidic hydrogens. The acid is often present in wines and precipitates from solution as the wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 24.65 ml of 0.2500 MNaOH solution to titrate both acidic protons in 50.00 ml of the tartaric acid solution. Write a balanced net ionic equation for the neutralization reaction, and calculate the molarity of the tartaric acid solution.

Problem 103AE: (a) A strontium hydroxide solution is prepared by dissolving 12.50 g of Sr(OH)2 in water to make 50.00 ml of solution. What is the molarity of this solution? (b) Next the strontium hydroxide solution prepared in part (a) is used to titrate a nitric acid solution of unknown concentration. Write a balanced chemical equation to represent the reaction between strontium hydroxide and nitric acid solutions, (c) If 23.9 ml of the strontium hydroxide solution was needed to neutralize a 37.5 ml aliquot of the nitric acid solution, what is the concentration (molarity) of the acid?

A solid sample of \(Zn(OH)_2\) is added to 0.350 L of 0.500 M aqueous HBr. The solution that remains is still acidic. It is then titrated with 0.500 MNaOH solution, and it takes 88.5 ml of the NaOH solution to reach the equivalence point. What mass of \(Zn(OH)_2\) was added to the HBr solution?

Problem 105IE Suppose you have 5.00 g of powdered magnesium metal, 1.00 L of 2.00 M potassium nitrate solution, and 1.00 L of 2.00 M silver nitrate solution, (a) Which one of the solutions will react with the magnesium powder? (b) What is the net ionic equation that describes this reaction? (c)What volume of solution is needed to completely react with the magnesium? (d) What is the molarity of the Mg2+ ions in the resulting solution?

Problem106: (a) By titration, 15.0 ml of 0.1008 M sodium hydroxide is needed to neutralize a 0.2053-g sample of a weak acid. What is the molar mass of the acid if it is monoprotic? (b) An elemental analysis of the acid indicates that it is composed of 5.89% H, 70.6% C, and 23.5% O by mass. What is its molecular formula? ?

Problem 107: A 3.455-g sample of a mixture was analyzed for barium ion by adding a small excess of sulfuric acid to an aqueous solution of the sample. The resultant reaction produced a precipitate of barium sulfate, which was collected by filtration, washed, dried, and weighed. If 0.2815 g of barium sulfate was obtained, what was the mass percentage of barium in the sample?

Problem 108: A fertilizer railroad car carrying 34,300 gallons of commercial aqueous ammonia (30% ammonia by mass) tips over and spills. The density of the aqueous ammonia solution is 0.88 g/cm3. What mass of citric acid, C(OH)(COOH)(CH2COOH)2, (which contains three acidic protons) is required to neutralize the spill? 1 gallon = 3.785 L.

Problem 109 IE: A sample of 7.75 g of Mg(OH)2 is added to 25.0 ml of 0.200 M HN03. (a) Write the chemical equation for the reaction that occurs, (b) Which is the limiting reactant in the reaction? (c) How many moles of Mg(OH)2, HN03, and Mg(N03)2 are present after the reaction is complete?

Problem 111 The average concentration of gold in seawater is 100 fM (femtomolar). Given that the price of gold is $1764.20 per troy ounce (1 troy ounce = 31.103 g), how many liters of seawater would you need to process to collect $5000 worth of gold, assuming your processing technique captures only 50% of the gold present in the samples?

Problem 112 The mass percentage of chloride ion in a 25.00-mL sample of seawater was determined by titrating the sample with silver nitrate, precipitating silver chloride. It took 42.58 ml of 0.2997 M silver nitrate solution to reach the equivalence point in the titration. What is the mass percentage of chloride ion in seawater if its density is 1.025 g/ml?

Problem 110 IE: Lead glass contains 18-40% by mass of PbO (instead of CaO in regular glass). Lead glass is still used industrially, but lead crystal' drinking goblets are no longer considered safe, as the lead may leach out and cause toxic responses in humans. A particular 286-g lead crystal goblet that holds 450 mL of liquid is 27% PbO by mass, and it leaches 3.4 micrograms of lead every time it is filled. How many grams of sodium sulfide would be required to decontaminate all the lead in the entire goblet?

Problem 113 The arsenic in a 1.22-g sample of a pesticide was converted to As043- by suitable chemical treatment. It was then titrated using Ag+ to form Ag3As04 as a precipitate, (a) What is the oxidation state of As in As043-? (b) Name Ag3As04 by analogy to the corresponding compound containing phosphorus in place of arsenic, (c) If it took 25.0 ml of 0.102 M Ag+ to reach the equivalence point in this titration, what is the mass percentage of arsenic in the pesticide?

Problem 114: The US. standard for arsenate in drinking water requires that public water supplies must contain no greater than 10 parts per billion (ppb) arsenic. If this arsenic is present as arsenate, AsO43-, what mass of sodium arsenate would be present in a 1.00-L sample of drinking water that just meets the standard? Parts per billion is defined on a mass basis as

Problem 115 Federal regulations set an upper limit of 50 parts per million (ppm) of NH3 in the air in a work environment that is, 50 molecules of NH3(g) for every million molecules in the air]. Air from a manufacturing operation was drawn through a solution containing 1.00 * 102 ml of 0.0105 M HCI. The NH3 reacts with HCI according to: After drawing air through the acid solution for 10.0 min at a rate of 10.0 L/min, the acid was titrated. The remaining acid needed 13.1 ml_ of 0.0588 MNaOH to reach the equivalence point, (a) How many grams of NH3 were drawn into the acid solution? (b) How many ppm of NH3 were in the air? (Air has a density of 1.20 g/L and an average molar mass of 29.0 g/mol under the conditions of the experiment.) (c) Is this manufacturer in compliance with regulations?

Consider the precipitation reaction: What volume of 0.175 M Na3PO4 solution is necessary to completely react with 95.4 mL of 0.102 M CuCl2?

Iron(III) sulfide reacts with carbon monoxide according to the equation: A reaction mixture initially contains 22.55 g Fe2O3 and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?

Elemental phosphorus reacts with chlorine gas according to the equation: A reaction mixture initially contains 45.69 g P4 and 131.3 g Cl2. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?

Lead ions can be precipitated from solution with KCl according to the reaction: When 28.5 g KCl is added to a solution containing 25.7 g Pb2+, a PbCl2 precipitate forms. The precipitate is filtered and dried and found to have a mass of 29.4 g. Determine the limiting reactant, theoretical yield of PbCl2, and percent yield for the reaction.

Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is When 10.1 g of Mg reacts with 10.5 g O2, 11.9 g MgO is collected. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

Urea (CH4N2O) is a common fertilizer that is synthesized by the reaction of ammonia (NH3) with carbon dioxide: In an industrial synthesis of urea, a chemist combines 136.4 kg of ammonia with 211.4 kg of carbon dioxide and obtains 168.4 kg of urea. Determine the limiting reactant, theoretical yield of urea, and percent yield for the reaction.

Many computer chips are manufactured from silicon, which occurs in nature as SiO2. When SiO2 is heated to melting, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 155.8 kg of SiO2 reacts with 78.3 kg of carbon to produce 66.1 kg of silicon. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

Complete and balance each acid–base equation. a. H2SO4(aq) + Ca(OH)2(aq) ? b. HClO4(aq) + KOH(aq) ? c. H2SO4(aq) + NaOH(aq) ?

Complete and balance each acid–base equation. a. HI(aq) + LiOH(aq) ? b. HC2H3O2(aq) + Ca(OH)2(aq) ? c. HCl(aq) + Ba(OH)2(aq) ?

A 25.00 mL sample of an unknown HClO4 solution requires titration with 22.62 mL of 0.2000 M NaOH to reach the equivalence point. What is the concentration of the unknown HClO4 solution? The neutralization reaction is

A 30.00 mL sample of an unknown H3PO4 solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.38 mL of NaOH solution is added. What is the concentration of the unknown H3PO4 solution? The neutralization reaction is

Complete and balance each gas-evolution equation.

Two aqueous solutions of KOH and MgCl2 are mixed. Which of the following diagrams best represents the mixture? For simplicity, water molecules are not shown. (Color codes are: K1 5 purple, OH2 5 red, Mg21 5 green, Cl2 5 orange.) (a) (b) (c) (d)

Characterize the following compounds as soluble or insoluble in water: (a) Ca3(PO4)2, (b) Mn(OH)2, (c) AgClO3, (d) K2S.

Characterize the following compounds as soluble or insoluble in water: (a) CaCO3, (b) ZnSO4, (c) Hg(NO3)2, (d) HgSO4, (e) NH4ClO4.

Write ionic and net ionic equations for the following reactions: (a) AgNO3(aq) 1 Na2SO4(aq) (b) BaCl2(aq) 1 ZnSO4(aq) (c) (NH4)2CO3(aq) 1 CaCl2(aq)

Write ionic and net ionic equations for the following reactions: (a) Na2S(aq) 1 ZnCl2(aq) (b) K3PO4(aq) 1 3Sr(NO3)2(aq) (c) Mg(NO3)2(aq) 1 2NaOH(aq)

Which of the following processes will likely result in a precipitation reaction? (a) Mixing a \(NaNO_3\) solution with a \(CuSO_4\) solution. (b) Mixing a \(BaCl_2\) solution with a \(K_2SO_4\) solution. Write a net ionic equation for the precipitation reaction.

With reference to Table 4.2, suggest one method by which you might separate (a) K1 from Ag1, (b) Ba21 from Pb21, (c) NH4 1 from Ca21, (d) Ba21 from Cu21. All cations are assumed to be in aqueous solution, and the common anion is the nitrate ion.

List the general properties of acids and bases

Give Arrhenius and Brnsteds definitions of an acid and a base. Why are Brnsteds definitions more useful in describing acid-base properties?

Give an example of a monoprotic acid, a diprotic acid, and a triprotic acid.

What are the characteristics of an acid-base neutralization reaction?

What factors qualify a compound as a salt? Specify which of the following compounds are salts: CH4, NaF, NaOH, CaO, BaSO4, HNO3, NH3, KBr?

Identify the following as a weak or strong acid or base: (a) NH3, (b) H3PO4, (c) LiOH, (d) HCOOH (formic acid), (e) H2SO4, (f) HF, (g) Ba(OH)2.

Identify each of the following species as a Brnsted acid, base, or both: (a) HI, (b) CH3COO2, (c) H2PO4 2, (d) HSO2 4.

Identify each of the following species as a Brnsted acid, base, or both: PO4 32, (b) ClO2 2, (c) NH4 1, (d) HCO3 2.

Balance the following equations and write the corresponding ionic and net ionic equations (if appropriate): (a) HBr(aq) 1 NH3(aq) (b) Ba(OH)2(aq) 1 H3PO4(aq) (c) HClO4(aq) 1 Mg(OH)2(s)

Balance the following equations and write the corresponding ionic and net ionic equations (if appropriate): (a) CH3COOH(aq) 1 KOH(aq) (b) H2CO3(aq) 1 NaOH(aq) (c) HNO3(aq) 1 Ba(OH)2(aq)

Give an example of a combination redox reaction, a decomposition redox reaction, and a displacement redox reaction.

All combustion reactions are redox reactions. True or false? Explain.

What is an oxidation number? How is it used to identify redox reactions? Explain why, except for ionic compounds, oxidation number does not have any physical significance

(a) Without referring to Figure 4.11, give the oxidation numbers of the alkali and alkaline earth metals in their compounds. (b) Give the highest oxidation numbers that the Groups 3A7A elements can have.

How is the activity series organized? How is it used in the study of redox reactions?

Use the following reaction to define redox reaction, half-reaction, oxidizing agent, reducing agent: 4Na(s) 1 O2(g) 2Na2O(s)

Is it possible to have a reaction in which oxidation occurs and reduction does not? Explain.

What is the requirement for an element to undergo disproportionation reactions? Name five common elements that are likely to take part in such reactions.

For the complete redox reactions given here, (i) break down each reaction into its half-reactions; (ii) identify the oxidizing agent; (iii) identify the reducing agent. (a) 2Sr 1 O2 2SrO (b) 2Li 1 H2 2LiH (c) 2Cs 1 Br2 2CsBr (d) 3Mg 1 N2 Mg3N2

For the complete redox reactions given here, write the half-reactions and identify the oxidizing and reducing agents. (a) 4Fe 1 3O2 2Fe2O3 (b) Cl2 1 2NaBr 2NaCl 1 Br2 (c) Si 1 2F2 SiF4 (d) H2 1 Cl2 2HCl

Arrange the following species in order of increasing oxidation number of the sulfur atom: (a) H2S, (b) S8, (c) H2SO4, (d) S22, (e) HS2, (f) SO2, (g) SO3.

Phosphorus forms many oxoacids. Indicate the oxidation number of phosphorus in each of the following acids: (a) HPO3, (b) H3PO2, (c) H3PO3, (d) H3PO4, (e) H4P2O7, (f) H5P3O10.

Give the oxidation number of the underlined atoms in the following molecules and ions: (a) ClF, (b) IF7, (c) CH4, (d) C2H2, (e) C2H4, (f) K2CrO4, (g) K2Cr2O7, (h) KMnO4, (i) NaHCO3, (j) Li2, (k) NaIO3, (l) KO2, (m) PF6 2, (n) KAuCl4.

Give the oxidation number for the following species: H2, Se8, P4, O, U, As4, B12.

Give oxidation numbers for the underlined atoms in the following molecules and ions: (a) Cs2O, (b) CaI2, (c) Al2O3, (d) H3AsO3, (e) TiO2, (f) MoO4 22, (g) PtCl4 22, (h) PtCl6 22, (i) SnF2, (j) ClF3, (k) SbF6 2.

Give the oxidation numbers of the underlined atoms in the following molecules and ions: (a) Mg3N2, (b) CsO2, (c) CaC2, (d) CO3 22, (e) C2O4 22, (f) ZnO2 22, (g) NaBH4, (h) WO4 2

Nitric acid is a strong oxidizing agent. State which of the following species is least likely to be produced when nitric acid reacts with a strong reducing agent such as zinc metal, and explain why: N2O, NO, NO2, N2O4, N2O5, NH4 1.

Which of the following metals can react with water? (a) Au, (b) Li, (c) Hg, (d) Ca, (e) Pt

On the basis of oxidation number considerations, one of the following oxides would not react with molecular oxygen: NO, N2O, SO2, SO3, P4O6. Which one is it? Why?

Predict the outcome of the reactions represented by the following equations by using the activity series, and balance the equations. (a) Cu(s) 1 HCl(aq) (b) I2(s) 1 NaBr(aq) (c) Mg(s) 1 CuSO4(aq) (d) Cl2(g) 1 KBr(aq)

Classify the following redox reactions: (a) 2H2O2 2H2O 1 O2 (b) Mg 1 2AgNO3 Mg(NO3)2 1 2Ag (c) NH4NO2 N2 1 2H2O (d) H2 1 Br2 2HBr

Classify the following redox reactions: (a) P4 1 10Cl2 4PCl5 (b) 2NO N2 1 O2 (c) Cl2 1 2KI 2KCl 1 I2 (d) 3HNO2 HNO3 1 H2O 1 2NO

Which of the following are redox processes? (a) CO2 CO22 3 (b) VO3 VO2 (c) SO3 SO22 4 (d) NO2 2 NO2 3 (e) Cr31 CrO22 4

Of the following, which is most likely to be the strongest oxidizing agent? O2, O1 2 , O2 2 , O22 2 .

Write the equation for calculating molarity. Why is molarity a convenient concentration unit in chemistry?

Describe the steps involved in preparing a solution of known molar concentration using a volumetric flask.

Calculate the mass of KI in grams required to prepare 5.00 3 102 mL of a 2.80 M solution

Describe how you would prepare 250 mL of a 0.707 M NaNO3 solution.

How many moles of MgCl2 are present in 60.0 mL of 0.100 M MgCl2 solution?

How many grams of KOH are present in 35.0 mL of a 5.50 M solution?

Calculate the molarity of each of the following solutions: (a) 29.0 g of ethanol (C2H5OH) in 545 mL of solution, (b) 15.4 g of sucrose (C12H22O11) in 74.0 mL of solution, (c) 9.00 g of sodium chloride (NaCl) in 86.4 mL of solution

Calculate the molarity of each of the following solutions: (a) 6.57 g of methanol (CH3OH) in 1.50 3 102 mL of solution, (b) 10.4 g of calcium chloride (CaCl2) in 2.20 3 102 mL of solution, (c) 7.82 g of naphthalene (C10H8) in 85.2 mL of benzene solution.

Calculate the volume in mL of a solution required to provide the following: (a) 2.14 g of sodium chloride from a 0.270 M solution, (b) 4.30 g of ethanol from a 1.50 M solution, (c) 0.85 g of acetic acid (CH3COOH) from a 0.30 M solution.

Determine how many grams of each of the following solutes would be needed to make 2.50 3 102 mL of a 0.100 M solution: (a) cesium iodide (CsI), (b) sulfuric acid (H2SO4), (c) sodium carbonate (Na2CO3), (d) potassium dichromate (K2Cr2O7), (e) potassium permanganate (KMnO4).

What volume of 0.416 M Mg(NO3)2 should be added to 255 mL of 0.102 M KNO3 to produce a solution with a concentration of 0.278 M NO2 3 ions? Assume volumes are additive.

Barium hydroxide, often used to titrate weak organic acids, is obtained as the octahydrate, Ba(OH)2 ? 8H2O. What mass of Ba(OH)2 ? 8H2O would be required to make 500.0 mL of a solution that is 0.1500 M in hydroxide ions?

Describe the basic steps involved in diluting a solution of known concentration.

Write the equation that enables us to calculate the concentration of a diluted solution. Give units for all the terms.

Describe how to prepare 1.00 L of 0.646 M HCl solution, starting with a 2.00 M HCl solution.

Water is added to 25.0 mL of a 0.866 M KNO3 solution until the volume of the solution is exactly 500 mL. What is the concentration of the final solution?

How would you prepare 60.0 mL of 0.200 M HNO3 from a stock solution of 4.00 M HNO3?

You have 505 mL of a 0.125 M HCl solution and you want to dilute it to exactly 0.100 M. How much water should you add? Assume volumes are additive.

A 35.2-mL, 1.66 M KMnO4 solution is mixed with 16.7 mL of 0.892 M KMnO4 solution. Calculate the concentration of the final solution.

A 46.2-mL, 0.568 M calcium nitrate [Ca(NO3)2] solution is mixed with 80.5 mL of 1.396 M calcium nitrate solution. Calculate the concentration of the final solution.

Describe the basic steps involved in gravimetric analysis. How does this procedure help us determine the identity of a compound or the purity of a compound if its formula is known?

Distilled water must be used in the gravimetric analysis of chlorides. Why?

If 30.0 mL of 0.150 M CaCl2 is added to 15.0 mL of 0.100 M AgNO3, what is the mass in grams of AgCl precipitate?

A sample of 0.6760 g of an unknown compound containing barium ions (Ba21) is dissolved in water and treated with an excess of Na2SO4. If the mass of the BaSO4 precipitate formed is 0.4105 g, what is the percent by mass of Ba in the original unknown compound?

How many grams of NaCl are required to precipitate most of the Ag1 ions from 2.50 3 102 mL of 0.0113 M AgNO3 solution? Write the net ionic equation for the reaction.

The concentration of sulfate in water can be determined by adding a solution of barium chloride to precipitate the sulfate ion. Write the net ionic equation for this reaction. Treating a 145-mL sample of water with excess BaCl2(aq) precipitated 0.330 g of BaSO4. Determine the concentration of sulfate in the original water sample.

Describe the basic steps involved in an acid-base titration. Why is this technique of great practical value?

How does an acid-base indicator work?

A student carried out two titrations using a NaOH solution of unknown concentration in the buret. In one titration she weighed out 0.2458 g of KHP (see p. 152) and transferred it to an Erlenmeyer flask. She then added 20.00 mL of distilled water to dissolve the acid. In the other titration she weighed out 0.2507 g of KHP but added 40.00 mL of distilled water to dissolve the acid. Assuming no experimental error, would she obtain the same result for the concentration of the NaOH solution?

Would the volume of a 0.10 M NaOH solution needed to titrate 25.0 mL of a 0.10 M HNO2 (a weak acid) solution be different from that needed to titrate 25.0 mL of a 0.10 M HCl (a strong acid) solution?

A quantity of 18.68 mL of a KOH solution is needed to neutralize 0.4218 g of KHP. What is the concentration (in molarity) of the KOH solution?

Calculate the concentration (in molarity) of a NaOH solution if 25.0 mL of the solution are needed to neutralize 17.4 mL of a 0.312 M HCl solution.

Calculate the volume in mL of a 1.420 M NaOH solution required to titrate the following solutions: (a) 25.00 mL of a 2.430 M HCl solution (b) 25.00 mL of a 4.500 M H2SO4 solution (c) 25.00 mL of a 1.500 M H3PO4 solution

What volume of a 0.500 M HCl solution is needed to neutralize each of the following: (a) 10.0 mL of a 0.300 M NaOH solution (b) 10.0 mL of a 0.200 M Ba(OH)2 solution

What are the similarities and differences between acid-base titrations and redox titrations?

Explain why potassium permanganate (KMnO4) and potassium dichromate (K2Cr2O7) can serve as internal indicators in redox titrations.

Iron(II) can be oxidized by an acidic K2Cr2O7 solution according to the net ionic equation: Cr2O22 7 1 6Fe21 1 14H1 2Cr31 1 6Fe31 1 7H2O If it takes 26.0 mL of 0.0250 M K2Cr2O7 to titrate 25.0 mL of a solution containing Fe21, what is the molar concentration of Fe21?

The SO2 present in air is mainly responsible for the acid rain phenomenon. Its concentration can be determined by titrating against a standard permanganate solution as follows: 5SO2 1 2MnO2 4 1 2H2O 5SO22 4 1 2Mn21 1 4H1 Calculate the number of grams of SO2 in a sample of air if 7.37 mL of 0.00800 M KMnO4 solution are required for the titration.

A sample of iron ore (containing only Fe21 ions) weighing 0.2792 g was dissolved in dilute acid solution, and all the Fe(II) was converted to Fe(III) ions. The solution required 23.30 mL of 0.0194 M K2Cr2O7 for titration. Calculate the percent by mass of iron in the ore. (Hint: See Problem 4.95 for the balanced equation.)

The concentration of a hydrogen peroxide solution can be conveniently determined by titration against a standardized potassium permanganate solution in an acidic medium according to the following equation: 2MnO2 4 1 5H2O2 1 6H1 5O2 1 2Mn21 1 8H2O If 36.44 mL of a 0.01652 M KMnO4 solution are required to oxidize 25.00 mL of a H2O2 solution, calculate the molarity of the H2O2 solution.

Oxalic acid (H2C2O4) is present in many plants and vegetables. If 24.0 mL of 0.0100 M KMnO4 solution is needed to titrate 1.00 g of a sample of H2C2O4 to the equivalence point, what is the percent by mass of H2C2O4 in the sample? The net ionic equation is 2MnO2 4 1 16H1 1 5C2O22 4 2Mn21 1 10CO2 1 8H2O

A 15.0-mL sample of an oxalic acid solution requires 25.2 mL of 0.149 M NaOH for neutralization. Calculate the volume of a 0.122 M KMnO4 solution needed to react with a second 15.0-mL sample of the oxalic acid solution. (Hint: Oxalic acid is a diprotic acid. See Problem 4.99 for redox equation.)

Iodate ion, IO3 2, oxidizes SO3 22 in acidic solution. The half-reaction for the oxidation is SO3 22 1 H2O SO4 22 1 2H1 1 2e2 A 100.0-mL sample of solution containing 1.390 g of KIO3 reacts with 32.5 mL of 0.500 M Na2SO3. What is the final oxidation state of the iodine after the reaction has occurred?

Calcium oxalate (CaC2O4), the main component of kidney stones, is insoluble in water. For this reason it can be used to determine the amount of Ca21 ions in fluids such as blood. The calcium oxalate isolated from blood is dissolved in acid and titrated against a standardized KMnO4 solution, as shown in Problem 4.99. In one test it is found that the calcium oxalate isolated from a 10.0-mL sample of blood requires 24.2 mL of 9.56 3 1024 M KMnO4 for titration. Calculate the number of milligrams of calcium per milliliter of blood.

Classify the following reactions according to the types discussed in the chapter: (a) Cl2 1 2OH2 Cl2 1 ClO2 1 H2O (b) Ca21 1 CO3 22 CaCO3 (c) NH3 1 H1 NH4 1 (d) 2CCl4 1 CrO4 22 2COCl2 1 CrO2Cl2 1 2Cl2 (e) Ca 1 F2 CaF2 (f) 2Li 1 H2 2LiH (g) Ba(NO3)2 1 Na2SO4 2NaNO3 1 BaSO4 (h) CuO 1 H2 Cu 1 H2O (i) Zn 1 2HCl ZnCl2 1 H2 (j) 2FeCl2 1 Cl2 2FeCl3 (k) LiOH 1 HNO3 LiNO3 1 H2O

Oxygen (O2) and carbon dioxide (CO2) are colorless and odorless gases. Suggest two chemical tests that would enable you to distinguish between these two gases.

Which of the following aqueous solutions would you expect to be the best conductor of electricity at 258C? Explain your answer. (a) 0.20 M NaCl (b) 0.60 M CH3COOH (c) 0.25 M HCl (d) 0.20 M Mg(NO3)2

A 5.00 3 102 -mL sample of 2.00 M HCl solution is treated with 4.47 g of magnesium. Calculate the concentration of the acid solution after all the metal has reacted. Assume that the volume remains unchanged.

Shown here are two aqueous solutions containing various ions. The volume of each solution is 200 mL. (a) Calculate the mass of the precipitate (in g) after the solutions are mixed. (b) What are the concentrations (in M) of the ions in the final solution? Treat each sphere as 0.100 mol. Assume the volumes are additive. SO4 22 Na1 Cl2 Ba21

Shown here are two aqueous solutions containing various ions. The volume of each solution is 200 mL. (a) Calculate the mass of the precipitate (in g) after the solutions are mixed. (b) What are the concentrations (in M) of the ions in the final solution? Treat each sphere as 0.100 mol. Assume the volumes are additive. OH2 K1 NO2 3 Al31

Calculate the volume of a 0.156 M CuSO4 solution that would react with 7.89 g of zinc

Sodium carbonate (Na2CO3) is available in very pure form and can be used to standardize acid solutions. What is the molarity of a HCl solution if 28.3 mL of the solution are required to react with 0.256 g of Na2CO3?

A 3.664-g sample of a monoprotic acid was dissolved in water. It took 20.27 mL of a 0.1578 M NaOH solution to neutralize the acid. Calculate the molar mass of the acid.

Acetic acid (CH3COOH) is an important ingredient of vinegar. A sample of 50.0 mL of a commercial vinegar is titrated against a 1.00 M NaOH solution. What is the concentration (in M) of acetic acid present in the vinegar if 5.75 mL of the base are needed for the titration?

A 15.00-mL solution of potassium nitrate (KNO3) was diluted to 125.0 mL, and 25.00 mL of this solution were then diluted to 1.000 3 103 mL. The concentration of the final solution is 0.00383 M. Calculate the concentration of the original solution

When 2.50 g of a zinc strip were placed in a AgNO3 solution, silver metal formed on the surface of the strip. After some time had passed, the strip was removed from the solution, dried, and weighed. If the mass of the strip was 3.37 g, calculate the mass of Ag and Zn metals present

Calculate the mass of the precipitate formed when 2.27 L of 0.0820 M Ba(OH)2 are mixed with 3.06 L of 0.0664 M Na2SO4.

Calculate the concentration of the acid (or base) remaining in solution when 10.7 mL of 0.211 M HNO3 are added to 16.3 mL of 0.258 M NaOH.

(a) Describe a preparation for magnesium hydroxide [Mg(OH)2] and predict its solubility. (b) Milk of magnesia contains mostly Mg(OH)2 and is effective in treating acid (mostly hydrochloric acid) indigestion. Calculate the volume of a 0.035 M HCl solution (a typical acid concentration in an upset stomach) needed to react with two spoonfuls (approximately 10 mL) of milk of magnesia [at 0.080 g Mg(OH)2/mL].

A 1.00-g sample of a metal X (that is known to form X21 ions) was added to 0.100 L of 0.500 M H2SO4. After all the metal had reacted, the remaining acid required 0.0334 L of 0.500 M NaOH solution for neutralization. Calculate the molar mass of the metal and identify the element

Carbon dioxide in air can be removed by an aqueous metal hydroxide solution such as LiOH and Ba(OH)2. (a) Write equations for the reactions. (Carbon dioxide reacts with water to form carbonic acid.) (b) Calculate the mass of CO2 that can be removed by 5.00 3 102 mL of a 0.800 M LiOH and a 0.800 M Ba(OH)2 solution. (c) Which solution would you choose for use in a space capsule and which for use in a submarine?

The molecular formula of malonic acid is C3H4O4. If a solution containing 0.762 g of the acid requires 12.44 mL of 1.174 M NaOH for neutralization, how many ionizable H atoms are present in the molecule?

A quantitative definition of solubility is the maximum number of grams of a solute that will dissolve in a given volume of water at a particular temperature. Describe an experiment that would enable you to determine the solubility of a soluble compound.

A 60.0-mL 0.513 M glucose (C6H12O6) solution is mixed with 120.0 mL of 2.33 M glucose solution. What is the concentration of the final solution? Assume the volumes are additive

An ionic compound X is only slightly soluble in water. What test would you employ to show that the compound does indeed dissolve in water to a certain extent?

A student is given an unknown that is either iron(II) sulfate or iron(III) sulfate. Suggest a chemical procedure for determining its identity. (Both iron compounds are water soluble.)

You are given a colorless liquid. Describe three chemical tests you would perform on the liquid to show that it is water.

Using the apparatus shown in Figure 4.1, a student found that a sulfuric acid solution caused the lightbulb to glow brightly. However, after the addition of a certain amount of a barium hydroxide [Ba(OH)2] solution, the light began to dim even though Ba(OH)2 is also a strong electrolyte. Explain.

The molar mass of a certain metal carbonate, MCO3, can be determined by adding an excess of HCl acid to react with all the carbonate and then back titrating the remaining acid with a NaOH solution. (a) Write an equation for these reactions. (b) In a certain experiment, 20.00 mL of 0.0800 M HCl were added to a 0.1022-g sample of MCO3. The excess HCl required 5.64 mL of 0.1000 M NaOH for neutralization. Calculate the molar mass of the carbonate and identify M

A 5.012-g sample of an iron chloride hydrate was dried in an oven. The mass of the anhydrous compound was 3.195 g. The compound was then dissolved in water and reacted with an excess of AgNO3. The AgCl precipitate formed weighed 7.225 g. What is the formula of the original compound?

You are given a soluble compound of unknown molecular formula. (a) Describe three tests that would show that the compound is an acid. (b) Once you have established that the compound is an acid, describe how you would determine its molar mass using a NaOH solution of known concentration. (Assume the acid is monoprotic.) (c) How would you find out whether the acid is weak or strong? You are provided with a sample of NaCl and an apparatus like that shown in Figure 4.1 for comparison.

You are given two colorless solutions, one containing NaCl and the other sucrose (C12H22O11). Suggest a chemical and a physical test that would allow you to distinguish between these two solutions.

The concentration of lead ions (Pb21) in a sample of polluted water that also contains nitrate ions (NO3 2) is determined by adding solid sodium sulfate (Na2SO4) to exactly 500 mL of the water. (a) Write the molecular and net ionic equations for the reaction. (b) Calculate the molar concentration of Pb21 if 0.00450 g of Na2SO4 was needed for the complete precipitation of Pb21 ions as PbSO4.

Hydrochloric acid is not an oxidizing agent in the sense that sulfuric acid and nitric acid are. Explain why the chloride ion is not a strong oxidizing agent like SO4 22 and NO3 2.

Explain how you would prepare potassium iodide (KI) by means of (a) an acid-base reaction and (b) a reaction between an acid and a carbonate compound

Sodium reacts with water to yield hydrogen gas. Why is this reaction not used in the laboratory preparation of hydrogen?

Describe how you would prepare the following compounds: (a) Mg(OH)2, (b) AgI, (c) Ba3(PO4)2.

Someone spilled concentrated sulfuric acid on the floor of a chemistry laboratory. To neutralize the acid, would it be preferable to pour concentrated sodium hydroxide solution or spray solid sodium bicarbonate over the acid? Explain your choice and the chemical basis for the action

Describe in each case how you would separate the cations or anions in an aqueous solution of: (a) NaNO3 and Ba(NO3)2, (b) Mg(NO3)2 and KNO3, (c) KBr and KNO3, (d) K3PO4 and KNO3, (e) Na2CO3 and NaNO3.

The following are common household compounds: table salt (NaCl), table sugar (sucrose), vinegar (contains acetic acid), baking soda (NaHCO3), washing soda (Na2CO3 ? 10H2O), boric acid (H3BO3, used in eyewash), epsom salt (MgSO4 ? 7H2O), sodium hydroxide (used in drain openers), ammonia, milk of magnesia [Mg(OH)2], and calcium carbonate. Based on what you have learned in this chapter, describe test(s) that would enable you to identify each of these compounds.

Sulfites (compounds containing the SO3 22 ions) are used as preservatives in dried fruit and vegetables and in wine making. In an experiment to test the presence of sulfite in fruit, a student first soaked several dried apricots in water overnight and then filtered the solution to remove all solid particles. She then treated the solution with hydrogen peroxide (H2O2) to oxidize the sulfite ions to sulfate ions. Finally, the sulfate ions were precipitated by treating the solution with a few drops of a barium chloride (BaCl2) solution. Write a balanced equation for each of the preceding steps.

A 0.8870-g sample of a mixture of NaCl and KCl is dissolved in water, and the solution is then treated with an excess of AgNO3 to yield 1.913 g of AgCl. Calculate the percent by mass of each compound in the mixture.

Based on oxidation number consideration, explain why carbon monoxide (CO) is flammable but carbon dioxide (CO2) is not

Which of the diagrams shown here corresponds to the reaction between AgOH(s) and HNO3(aq)? Write a balanced equation for the reaction. The green spheres represent the Ag1 ions and the red spheres represent the NO3 2 ions. (a) (b) (c)

Chlorine forms a number of oxides with the following oxidation numbers: 11, 13, 14, 16, and 17. Write a formula for each of these compounds

A useful application of oxalic acid is the removal of rust (Fe2O3) from, say, bathtub rings according to the reaction Fe2O3(s) 1 6H2C2O4(aq) 2Fe(C2O4)3 32 (aq) 1 3H2O 1 6H1 (aq) Calculate the number of grams of rust that can be removed by 5.00 3 102 mL of a 0.100 M solution of oxalic acid.

Acetylsalicylic acid (C9H8O4) is a monoprotic acid commonly known as aspirin. A typical aspirin tablet, however, contains only a small amount of the acid. In an experiment to determine its composition, an aspirin tablet was crushed and dissolved in water. It took 12.25 mL of 0.1466 M NaOH to neutralize the solution. Calculate the number of grains of aspirin in the tablet. (One grain 5 0.0648 g.)

A 0.9157-g mixture of CaBr2 and NaBr is dissolved in water, and AgNO3 is added to the solution to form AgBr precipitate. If the mass of the precipitate is 1.6930 g, what is the percent by mass of NaBr in the original mixture?

Hydrogen halides (HF, HCl, HBr, HI) are highly reactive compounds that have many industrial and laboratory uses. (a) In the laboratory, HF and HCl can be generated by reacting CaF2 and NaCl with concentrated sulfuric acid. Write appropriate equations for the reactions. (Hint: These are not redox reactions.) (b) Why is it that HBr and HI cannot be prepared similarly, that is, by reacting NaBr and NaI with concentrated sulfuric acid? (Hint: H2SO4 is a stronger oxidizing agent than both Br2 and I2.) (c) HBr can be prepared by reacting phosphorus tribromide (PBr3) with water. Write an equation for this reaction.

A 325-mL sample of solution contains 25.3 g of CaCl2. (a) Calculate the molar concentration of Cl2 in this solution. (b) How many grams of Cl2 are in 0.100 L of this solution?

Phosphoric acid (H3PO4) is an important industrial chemical used in fertilizers, in detergents, and in the food industry. It is produced by two different methods. In the electric furnace method, elemental phosphorus (P4) is burned in air to form P4O10, which is then reacted with water to give H3PO4. In the wet process, the mineral phosphate rock fluorapatite [Ca5(PO4)3F] is reacted with sulfuric acid to give H3PO4 (and HF and CaSO4). Write equations for these processes and classify each step as precipitation, acid-base, or redox reaction.

Ammonium nitrate (NH4NO3) is one of the most important nitrogen-containing fertilizers. Its purity can be analyzed by titrating a solution of NH4NO3 with a standard NaOH solution. In one experiment a 0.2041-g sample of industrially prepared NH4NO3 required 24.42 mL of 0.1023 M NaOH for neutralization. (a) Write a net ionic equation for the reaction. (b) What is the percent purity of the sample?

Is the following reaction a redox reaction? Explain. 3O2(g) 2O3(g)

What is the oxidation number of O in HFO?

Use molecular models like those in Figures 4.7 and 4.8 to represent the following acid-base reactions: (a) OH2 1 H3O1 2H2O (b) NH4 1 1 NH2 2 2NH3 Identify the Brnsted acid and base in each case

The alcohol content in a 10.0-g sample of blood from a driver required 4.23 mL of 0.07654 M K2Cr2O7 for titration. Should the police prosecute the individual for drunken driving? (Hint: See the Chemistry in Action essay on p. 144.)

On standing, a concentrated nitric acid gradually turns yellow in color. Explain. (Hint: Nitric acid slowly decomposes. Nitrogen dioxide is a colored gas.)

Describe the laboratory preparation for the following gases: (a) hydrogen, (b) oxygen, (c) carbon dioxide, and (d) nitrogen. Indicate the physical states of the reactants and products in each case. [Hint: Nitrogen can be obtained by heating ammonium nitrite (NH4NO2).]

Referring to Figure 4.18, explain why one must first dissolve the solid completely before making up the solution to the correct volume

Can the following decomposition reaction be characterized as an acid-base reaction? Explain. NH4Cl(s) NH3(g) 1 HCl(g)

Give a chemical explanation for each of the following: (a) When calcium metal is added to a sulfuric acid solution, hydrogen gas is generated. After a few minutes, the reaction slows down and eventually stops even though none of the reactants is used up. Explain. (b) In the activity series, aluminum is above hydrogen, yet the metal appears to be unreactive toward steam and hydrochloric acid. Why? (c) Sodium and potassium lie above copper in the activity series. Explain why Cu21 ions in a CuSO4 solution are not converted to metallic copper upon the addition of these metals. (d) A metal M reacts slowly with steam. There is no visible change when it is placed in a pale green iron(II) sulfate solution. Where should we place M in the activity series? (e) Before aluminum metal was obtained by electrolysis, it was produced by reducing its chloride (AlCl3) with an active metal. What metals would you use to produce aluminum in that way?

The recommended procedure for preparing a very dilute solution is not to weigh out a very small mass or measure a very small volume of a stock solution. Instead, it is done by a series of dilutions. A sample of 0.8214 g of KMnO4 was dissolved in water and made up to the volume in a 500-mL volumetric flask. A 2.000-mL sample of this solution was transferred to a 1000-mL volumetric flask and diluted to the mark with water. Next, 10.00 mL of the diluted solution were transferred to a 250- mL flask and diluted to the mark with water. (a) Calculate the concentration (in molarity) of the final solution. (b) Calculate the mass of KMnO4 needed to directly prepare the final solution.

The following cycle of copper experiment is performed in some general chemistry laboratories. The series of reactions starts with copper and ends with metallic copper. The steps are as follows: (1) A piece of copper wire of known mass is allowed to react with concentrated nitric acid [the products are copper(II) nitrate, nitrogen dioxide, and water]. (2) The copper(II) nitrate is treated with a sodium hydroxide solution to form copper(II) hydroxide precipitate. (3) On heating, copper(II) hydroxide decomposes to yield copper(II) oxide. (4) The copper(II) oxide is reacted with concentrated sulfuric acid to yield copper(II) sulfate. (5) Copper(II) sulfate is treated with an excess of zinc metal to form metallic copper. (6) The remaining zinc metal is removed by treatment with hydrochloric acid, and metallic copper is filtered, dried, and weighed. (a) Write a balanced equation for each step and classify the reactions. (b) Assuming that a student started with 65.6 g of copper, calculate the theoretical yield at each step. (c) Considering the nature of the steps, comment on why it is possible to recover most of the copper used at the start.

A quantity of 25.0 mL of a solution containing both Fe21 and Fe31 ions is titrated with 23.0 mL of 0.0200 M KMnO4 (in dilute sulfuric acid). As a result, all of the Fe21 ions are oxidized to Fe31 ions. Next, the solution is treated with Zn metal to convert all of the Fe31 ions to Fe21 ions. Finally, the solution containing only the Fe21 ions requires 40.0 mL of the same KMnO4 solution for oxidation to Fe31. Calculate the molar concentrations of Fe21 and Fe31 in the original solution. The net ionic equation is MnO4 2 1 5Fe21 1 8H1 Mn21 1 5Fe31 1 4H2O

Use the periodic table framework shown to show the names and positions of two metals that can (a) displace hydrogen from cold water, (b) displace hydrogen from steam, and (c) displace hydrogen from acid. Also show two metals that can react neither with water nor acid

Referring to the Chemistry in Action essay on page 156, answer the following questions: (a) Identify the precipitation, acid-base, and redox processes. (b) Instead of calcium oxide, why dont we simply add sodium hydroxide to seawater to precipitate magnesium hydroxide? (c) Sometimes a mineral called dolomite (a mixture of CaCO3 and MgCO3) is substituted for limestone to bring about the precipitation of magnesium hydroxide. What is the advantage of using dolomite?

A 22.02-mL solution containing 1.615 g Mg(NO3)2 is mixed with a 28.64-mL solution containing 1.073 g NaOH. Calculate the concentrations of the ions remaining in solution after the reaction is complete. Assume volumes are additive

Chemical tests of four metals A, B, C, and D show the following results. (a) Only B and C react with 0.5 M HCl to give H2 gas. (b) When B is added to a solution containing the ions of the other metals, metallic A, C, and D are formed. (c) A reacts with 6 M HNO3 but D does not. Arrange the metals in the increasing order as reducing agents. Suggest four metals that fit these descriptions

The antibiotic gramicidin A can transport Na1 ions into a certain cell at the rate of 5.0 3 107 Na1 ions s 21 . Calculate the time in seconds to transport enough Na1 ions to increase its concentration by 8.0 3 1023 M in a cell whose intracellular volume is 2.0 3 10210 mL.

Use Lagrange multipliers to give an alternate solution to the indicated exercise in Section 14.7. Exercise 49: Find the maximum volume of a rectangular box that is inscribed in a sphere of radius r

Many proteins contain metal ions for structural and/or redox functions. Which of the following metals fit into one or both categories: Ca, Cu, Fe, Mg, Mn, Ni, Zn?

The fastest way to introduce therapeutic agents into the bloodstream is by direct delivery into a vein (intravenous therapy, or IV therapy). A clinical researcher wishes to establish an initial concentration of 6 3 1024 mmol/L in the bloodstream of an adult male participating in a trial study of a new drug. The drug serum is prepared in the hospitals pharmacy at a concentration of 1.2 3 1023 mol/L. How much of the serum should be introduced intravenously in order to achieve the desired initial blood concentration of the drug?

Public water supplies are often fluoridated by the addition of compounds such as NaF, H2SiF6, and Na2SiF6. It is well established that fluoride helps prevent tooth decay; however, care must be taken not to exceed safe levels of fluoride, which can stain or etch tooth enamel (dental fluorosis). A safe and effective concentration of fluoride in drinking water is generally considered to be around 1 mg/L. How much fluoride would a person consume by drinking fluoridated water in 1 year? What would be the equivalent mass as sodium fluoride?

Potassium superoxide (KO2), a useful source of oxygen employed in breathing equipment, reacts with water to form potassium hydroxide, hydrogen peroxide, and oxygen. Furthermore, potassium superoxide also reacts with carbon dioxide to form potassium carbonate and oxygen. (a) Write equations for these two reactions and comment on the effectiveness of potassium superoxide in this application. (b) Focusing only on the reaction between KO2 and CO2, estimate the amount of KO2 needed to sustain a worker in a polluted environment for 30 min. See Problem 1.69 for useful information.

Muriatic acid, a commercial-grade hydrochloric acid used for cleaning masonry surfaces, is typically around 10 percent HCl by mass and has a density of 1.2 g/cm3 . A 0.5-in layer of boiler scale has accumulated on a 6.0-ft section of hot water pipe with an internal diameter of 2.0 in (see the Chemistry in Action essay on p. 126). What is the minimum volume of muriatic acid in gallons that would be needed to remove the boiler scale?

Because acid-base and precipitation reactions discussed in this chapter all involve ionic species, their progress can be monitored by measuring the electrical conductance of the solution. Match the following reactions with the diagrams shown here. The electrical conductance is shown in arbitrary units. (1) A 1.0 M KOH solution is added to 1.0 L of 1.0 M CH3COOH. (2) A 1.0 M NaOH solution is added to 1.0 L of 1.0 M HCl.

Problem 1E What is reaction stoichiometry? What is the significance of the coefficients in a balanced chemical equation?

Manganese(IV) oxide reacts with aluminum to form elemental manganese and aluminum oxide: What mass of Al is required to completely react with 25.0 g MnO2? a) 7.76 g Al b) 5.82 g Al c) 33.3 g Al d) 10.3 g Al

Sodium and chlorine react to form sodium chloride: What is the theoretical yield of sodium chloride for the reaction of 55.0 g Na with 67.2 g Cl2? a) 1.40 x 102 g NaCl b) 111 g NaCl c) 55.4 g NaCl d) 222 g NaCl

Problem 2E n a chemical reaction, what is the limiting reactant? The theoretical yield? The percent yield? What do we mean when we say a reactant is in excess?

Problem 3E We typically calculate the percent yield using the actual yield and theoretical yield in units of mass (g or kg). Would the percent yield be different if the actual yield and theoretical yield were in units of amount (moles)?

Sulfur and fluorine react to form sulfur hexaf uoride: If 50.0 g S is allowed to react as completely as possible with 105.0 g F2(g), what mass of the excess reactant is left? a) 20.5 g S c) 45.7 g F2 c) 15.0 g S d) 36.3 g F2

Problem 4E What is an aqueous solution? What is the difference between the solute and the solvent?

Problem 4SAQ A reaction has a theoretical yield of 45.8 g. When the reaction is carried out, 37.2 g of the product is obtained. What is the percent yield? a) 55.1% b) 44.8% c) 123% d) 81.2%

Problem 5E What is molarity? How is it useful?

What is the molarity of a solution containing 55.8 g of MgCl2 dissolved in 1.00 L of solution? a) 55.8 M b) 1.71 M c) 0.586 M d) 0.558 M

Problem 6E Explain how a strong electrolyte, a weak electrolyte, and a nonelectrolyte differ.

What mass (in grams) of Mg(NO3)2 is present in 145 mL of a 0.150 M solution of Mg(NO3)2? a) 3.23 g b) 0.022 g c) 1.88 g d) 143 g

Problem 7SAQ What volume of a 1.50 M HCI solution should you use to prepare 2.00 L of a 0.100 M HCI solution? a) 0.300 L b) 0.133 L c) 30.0 L d) 2.00 L

Problem 7E Explain the difference between a strong acid and a weak acid.

Problem 8E What does it mean for a compound to be soluble? Insoluble?

Potassium iodide reacts with lead(II) nitrate in the following precipitation reaction: What minimum volume of 0.200 M potassium iodide solution is required to completely precipitate all of the lead in 155.0 mL of a 0.112 M lead(II) nitrate solution? a) 348 mL b) 86.8 mL c) 174 mL d) 43.4 mL

Problem 9E What are the solubility rules? How are they useful?

Which solution will form a precipitate when mixed with a solution of aqueous \(\mathrm{Na}_{2} \mathrm{CO}_{3}\)? a) \(\mathrm{KNO}_{3}(a q)\) b) NaBr(aq) c) \(\mathrm{NH}_{4} \mathrm{Cl}(a q)\) d) \(\mathrm{CuCl}_{2}(a q)\)

Problem 10E What are the cations and anions whose compounds are usually soluble? What are the exceptions? What are the anions whose compounds are mostly insoluble? What are the exceptions?

Problem 11E What is a precipitation reaction? Give an example.

What is the net ionic equation for the reaction that occurs when aqueous solutions of KOH and SrCl2 are mixed? a) K+(aq) + Cl-(aq) ? KCl(s) b) Sr2+(aq) + 2 OH-(aq) ? Sr(OH)2(s) c) H+(aq) + OH-(aq) ? H2O(l) d) None of the above because no reaction occurs

What is the net ionic equation for the reaction that occurs when aqueous solutions of KOH and HNO3 are mixed?

Problem 12E How can you predict whether a precipitation reaction will occur upon mixing two aqueous solutions?

What is the net ionic equation for the reaction that occurs when aqueous solutions of KHCO3 and HBr are mixed?

Problem 13E Explain how a molecular equation, a complete ionic equation, and a net ionic equation differ.

What is the oxidation state of carbon in CO32-? a) +4 b) +3 c) -3 d) -2

Problem 14E What is the Arrhenius definition of an acid? A base?

Sodium reacts with water according to the reaction: Identify the oxidizing agent. a) Na(s) b) H2O(l) c) NaOH(aq) d) H2(aq)

Problem 15E What is an acid–base reaction? Give an example.

Identify the correct balanced equation for the combustion of propane (C3H8).

Problem 16E Explain the principles behind an acid–base titration. What is an indicator?

Problem 17E What is a gas-evolution reaction? Give an example.

Problem 18E What reactant types give rise to gas-evolution reactions?

Problem 19E What is an oxidation–reduction reaction? Give an example.

Problem 20E What are oxidation states?

Problem 21E How can oxidation states be used to identify redox reactions?

Problem 22E In a redox reaction, which reactant is the oxidizing agent? The reducing agent?

Problem 24E What is a combustion reaction? Why are they important? Give an example.

Consider the unbalanced equation for the combustion of hexane: Balance the equation and determine how many moles of O2 are required to react completely with 7.2 moles of C6H14.

Consider the unbalanced equation for the neutralization of acetic acid: \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Ba}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}(a q)\) Balance the equation and determine how many moles of \(\mathrm{Ba}(\mathrm{OH})_{2}\) are required to completely neutralize 0.461 mole of \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\).

Calculate how many moles of NO2 form when each quantity of reactant completely reacts. a. 2.5 mol N2O5 b. 6.8 mol N2O5 c. 15.2 g N2O5 d. 2.87 kg N2O5

Calculate how many moles of NH3 form when each quantity of reactant completely reacts. a. 2.6 mol N2H4 b. 3.55 mol N2H4 c. 65.3 g N2H4 d. 4.88 kg N2H4

Consider the balanced equation: Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that is made.

Consider the balanced equation Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that is made.

Hydrobromic acid dissolves solid iron according to the reaction: What mass of HBr (in g) do you need to dissolve a 3.2 g pure iron bar on a padlock? What mass of H2 would the complete reaction of the iron bar produce?

Sulfuric acid dissolves aluminum metal according to the reaction: Suppose you want to dissolve an aluminum block with a mass of 15.2 g. What minimum mass of H2SO4 (in g) do you need? What mass of H2 gas (in g) does the complete reaction of the aluminum block produce?

For each of the reactions, calculate the mass (in grams) of the product that forms when 3.67 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.

For each of the reactions, calculate the mass (in grams) of the product that forms when 15.39 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.

For each of the acid–base reactions, calculate the mass (in grams) of each acid necessary to completely react with and neutralize 4.85 g of the base. a. HCl(aq) + NaOH(aq) ? H2O(l) + NaCl(aq) b. 2 HNO3(aq) + Ca(OH)2(aq) ? 2 H2O(l) + Ca(NO3)2(aq) c. H2SO4(aq) + 2 KOH(aq) ? 2 H2O(l) + K2SO4(aq)

For each precipitation reaction, calculate how many grams of the first reactant are necessary to completely react with 55.8 g of the second reactant. a. 2 KI(aq) + Pb(NO3)2(aq) ? PbI2(s) + 2 KNO3(aq) b. Na2CO3(aq) + CuCl2(aq) ? CuCO3(s) + 2 NaCl(aq) c. K2SO4(aq) + Sr(NO3)2(aq) ? SrSO4(s) + 2 KNO3(aq)

For the following reaction, determine the limiting reactant for each of the initial amounts of reactants. a. 2 mol Na, 2 mol Br2 b. 1.8 mol Na, 1.4 mol Br2 c. 2.5 mol Na, 1 mol Br2 d. 12.6 mol ht0Na, 6.9 mol Br2

Find the limiting reactant for each initial amount of reactants. \(4\mathrm{\ Al}(s)+3\ \mathrm{O}_2(\mathrm{g})\rightarrow2\mathrm{\ Al}_2\mathrm{O}_3(\mathrm{s})\) a. \(1\mathrm{\ mol}\mathrm{\ Al},\ 1\mathrm{\ mol\ }\mathrm{O}_2\) b. \(4\mathrm{\ mol}\mathrm{\ Al},\ 1\mathrm{\ mol\ }\mathrm{O}_2\) c. \(16\mathrm{\ mol}\mathrm{\ Al},\ 13\mathrm{\ mol\ }\mathrm{O}_2\) d. \(7.4\mathrm{\ mol}\mathrm{\ Al},\ 6.5\mathrm{\ mol\ }\mathrm{O}_2\)

Consider the reaction: Each molecular diagram represents an initial mixture of the reactants. How many molecules of Cl2 would be formed from the reaction mixture that produces the greatest amount of products?

Consider the reaction: Each of the molecular diagrams represents an initial mixture of the reactants. How many CO2 molecules would be formed from the reaction mixture that produces the greatest amount of products?

Calculate the theoretical yield of the product (in moles) for each initial amount of reactants. a. 4 mol Ti, 4 mol Cl2 b. 7 mol Ti, 17 mol Cl2 c. 12.4 mol Ti, 18.8 mol Cl2

Calculate the theoretical yield of product (in moles) for each initial amount of reactants. a. 3 mol Mn, 3 mol O2 b. 4 mol Mn, 7 mol O2 c. 27.5 mol Mn, 43.8 mol O2

Zinc(II) sulfide reacts with oxygen according to the reaction: A reaction mixture initially contains 4.2 mol ZnS and 6.8 mol O2. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?

Iron(II) sulfide reacts with hydrochloric acid according to the reaction: A reaction mixture initially contains 0.223 mol FeS and 0.652 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?

For the reaction shown, calculate the theoretical yield of product (in grams) for each initial amount of reactants. a. 2.0 g Al, 2.0 g Cl2 b. 7.5 g Al, 24.8 g Cl2 c. 0.235 g Al, 1.15 g Cl2

For the reaction shown, calculate the theoretical yield of the product (in grams) for each initial amount of reactants. a. 5.0 g Ti, 5.0 g F2 b. 2.4 g Ti, 1.6 g F2 c. 0.233 g Ti, 0.288 g F2

Assign oxidation states to each atom in each element, ion, or compound. a. Ag b. Ag+ c. CaF2 d. H2S e. CO32- f. CrO42-

Assign oxidation states to each atom in each element, ion, or compound. a. Cl2 b. Fe3+ c. CuCl2 d. CH4 e. Cr2O72- f. HSO4 -

What is the oxidation state of Cr in each compound? a. CrO b. CrO3 c. Cr2O3

What is the oxidation state of Cl in each ion? a. ClO- b. ClO2- c. ClO3- d. ClO4-

Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent.

Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent.

Complete and balance each combustion reaction equation.

Complete and balance each combustion reaction equation:

The density of a 20.0% by mass ethylene glycol (C2H6O2) solution in water is 1.03 g/mL. Find the molarity of the solution.

Problem 101E People often use sodium bicarbonate as an antacid to neutralize excess hydrochloric acid in an upset stomach. What mass of hydrochloric acid (in grams) can 2.5 g of sodium bicarbonate neutralize? (Hint: Begin by writing a balanced equation for the reaction between aqueous sodium bicarbonate and aqueous hydrochloric acid.)

Problem 100E Find the percent by mass of sodium chloride in a 1.35 M NaCl solution. The density of the solution is 1.05 g/mL.

Problem 102E Toilet bowl cleaners often contain hydrochloric acid, which dissolves the calcium carbonate deposits that accumulate within a toilet bowl. What mass of calcium carbonate (in grams) can 3.8 g of HCl dissolve? (Hint: Begin by writing a balanced equation for the reaction between hydrochloric acid and calcium carbonate.)

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate the mass (in kg) of carbon dioxide that is added to the atmosphere per 1.0 kg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)

Many home barbeques are fueled with propane gas (C3H8). What mass of carbon dioxide (in kg) is produced upon the complete combustion of 18.9 L of propane (approximate contents of one 5-gallon tank)? Assume that the density of the liquid propane in the tank is 0.621 g/mL. (Hint: Begin by writing a balanced equation for the combustion reaction.)

Aspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form aspirin (C9H8O4) and acetic acid (C2H4O2). The balanced equation is In a laboratory synthesis, a student begins with 3.00 mL of acetic anhydride (density = 1.08 g/mL) and 1.25 g of salicylic acid. Once the reaction is complete, the student collects 1.22 g of aspirin. Determine the limiting reactant, theoretical yield of aspirin, and percent yield for the reaction.

The combustion of liquid ethanol (C2H5OH) produces carbon dioxide and water. After 4.62 mL of ethanol ( density = 0.789 g/mL ) is allowed to burn in the presence of 15.55 g of oxygen gas, 3.72 mL of water (density = 1.00 g/mL) is collected. Determine the limiting reactant, theoretical yield of H2O , and percent yield for the reaction. (Hint: Write a balanced equation for the combustion of ethanol.)

A loud classroom demonstration involves igniting a hydrogen filled balloon. The hydrogen within the balloon reacts explosively with oxygen in the air to form water. If the balloon is filled with a mixture of hydrogen and oxygen, the explosion is even louder than if the balloon is filled only with hydrogen— the intensity of the explosion depends on the relative amounts of oxygen and hydrogen within the balloon. Look at the molecular views representing different amounts of hydrogen and oxygen in four different balloons. Based on the balanced chemical equation, which balloon will make the loudest explosion?

A hydrochloric acid solution will neutralize a sodium hydroxide solution. Look at the molecular views showing one beaker of HCl and four beakers of NaOH. Which NaOH beaker will just neutralize the HCl beaker? Begin by writing a balanced chemical equation for the neutralization reaction.

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write “NO REACTION.” a. HCl(aq) + Hg2(NO3)2(aq) ? b. KHSO3(aq) + HNO3(aq) ? c. aqueous ammonium chloride and aqueous lead(II) nitrate d. aqueous ammonium chloride and aqueous calcium hydroxide

Hard water often contains dissolved Ca2+ and Mg2+ ions. One way to soften water is to add phosphates. The phosphate ion forms insoluble precipitates with calcium and magnesium ions, removing them from solution. A solution is 0.050 M in calcium chloride and 0.085 M in magnesium nitrate. What mass of sodium phosphate would have to be added to 1.5 L of this solution to completely eliminate the hard water ions? Assume complete reaction.

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write “NO REACTION.” a. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{HNO}_{3}(a q) \rightarrow\) b. \(\mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3}(a q)+\mathrm{LiOH}(a q) \rightarrow\) c. liquid pentanol \(\left(\mathrm{C}_{5} \mathrm{H}_{12} \mathrm{O}\right)\) and gaseous oxygen d. aqueous strontium sulfide and aqueous copper(II) sulfate

An acid solution is 0.100 M in HCl and 0.200 M in H2SO4. What volume of a 0.150 M KOH solution would completely neutralize all the acid in 500.0 mL of this solution?

Find the mass of barium metal (in grams) that must react with O2 to produce enough barium oxide to prepare 1.0 L of a 0.10 M solution of OH-.

A solution contains Cr3+ ion and Mg2+ ion. The addition of 1.00 L of 1.51 M NaF solution causes the complete precipitation of these ions as CrF3(s) and MgF2(s). The total mass of the precipitate is 49.6 g. Find the mass of Cr3+ in the original solution.

Problem 115E The nitrogen in sodium nitrate and in ammonium sulfate is available to plants as fertilizer. Which is the more economical source of nitrogen, a fertilizer containing 30.0% sodium nitrate by weight and costing $9.00 per 100 lb or one containing 20.0% ammonium sulfate by weight and costing $8.10 per 100 lb?

Find the volume of \(0.110 \mathrm{M}\) hydrochloric acid necessary to react completely with \(1.52 \mathrm{~g} \mathrm{Al}(\mathrm{OH})_3\).

Treatment of gold metal with BrF3 and KF produces Br2 and KAuF4, a salt of gold. Identify the oxidizing agent and the reducing agent in this reaction. Find the mass of the gold salt that forms when a 73.5 g mixture of equal masses of all three reactants is prepared.

We prepare a solution by mixing 0.10 L of 0.12 M sodium chloride with 0.23 L of a 0.18 M MgCl2 solution. What volume of a 0.20 M silver nitrate solution do we need to precipitate all the Cl- ion in the solution as AgCl?

A solution contains one or more of the following ions: Ag+, Ca2+, and Cu2+. When you add sodium chloride to the solution, no precipitate forms. When you add sodium sulfate to the solution, a white precipitate forms. You filter off the precipitate and add sodium carbonate to the remaining solution, producing another precipitate. Which ions were present in the original solution? Write net ionic equations for the formation of each of the precipitates observed.

A solution contains one or more of the following ions: Hg22+, Ba2+, and Fe2+. When potassium chloride is added to the solution, a precipitate forms. The precipitate is filtered off, and potassium sulfate is added to the remaining solution, producing no precipitate. When potassium carbonate is added to the remaining solution, a precipitate forms. Which ions were present in the original solution? Write net ionic equations for the formation of each of the precipitates observed.

The reaction of NH3 and O2 forms NO and water. The NO can be used to convert P4 to P4O6, forming N2 in the process. The P4O6 can be treated with water to form H3PO3, which forms PH3 and H3PO4 when heated. Find the mass of PH3 that forms from the reaction of 1.00 g NH3.

A liquid fuel mixture contains 30.35% hexane (C6H14), 15.85% heptane (C7H16), and the rest octane (C8H18). What maximum mass of carbon dioxide is produced by the complete combustion of 10.0 kg of this fuel mixture?

An important reaction that takes place in a blast furnace during the production of iron is the formation of iron metal and CO2 from Fe2O3 and CO. Determine the mass of Fe2O3 required to form 910 kg of iron. Determine the amount of CO2 that forms in this process.

Titanium occurs in the magnetic mineral ilmenite ( FeTiO3 ), which is often found mixed up with sand. The ilmenite can be separated from the sand with magnets. The titanium can then be extracted from the ilmenite by the following set of reactions: Suppose that an ilmenite–sand mixture contains 22.8% ilmenite by mass and that the first reaction is carried out with a 90.8% yield. If the second reaction is carried out with an 85.9% yield, what mass of titanium can be obtained from 1.00 kg of the ilmenite–sand mixture?

A mixture of C3H8 and C2H2 has a mass of 2.0 g. It is burned in excess O2 to form a mixture of water and carbon dioxide that contains 1.5 times as many moles of CO2 as of water. Find the mass of C2H2 in the original mixture.

A mixture of 20.6 g of P and 79.4 g Cl2 reacts completely to form PCl3 and PCl5 as the only products. Find the mass of PCl3 that forms.

A solution contains Ag+ and Hg2+ ions. The addition of 0.100 L of 1.22 M NaI solution is just enough to precipitate all the ions as AgI and HgI2. The total mass of the precipitate is 28.1 g. Find the mass of AgI in the precipitate.

The water in lakes that have been acidified by acid rain (\(\mathrm{HNO}_{3}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\)) can be neutralized by a process called liming, in which limestone \(\left(\mathrm{CaCO}_{3}\right)\) is added to the acidified water. What mass of limestone (in kg) would completely neutralize a 15.2 billion-liter lake that is \(1.8\times10^{-5}\mathrm{\ M}\) in \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and \(8.7\times10^{-6}\mathrm{\ M}\) in \(\mathrm{HNO}_{3}\)?

Recall from Section 4.6 that sodium carbonate is often added to laundry detergents to soften hard water and make the detergent more effective. Suppose that a particular detergent mixture is designed to soften hard water that is 3.5 x 10-3 M in Ca2+ and 1.1 x 10-3 M in Mg2+ and that the average capacity of a washing machine is 19.5 gallons of water. If the detergent requires using 0.65 kg detergent per load of laundry, what percentage (by mass) of the detergent should be sodium carbonate in order to completely precipitate all of the calcium and magnesium ions in an average load of laundry water?

Lead poisoning is a serious condition resulting from the ingestion of lead in food, water, or other environmental sources. It affects the central nervous system, leading to a variety of symptoms such as distractibility, lethargy, and loss of motor coordination. Lead poisoning is treated with chelating agents, substances that bind to metal ions, allowing them to be eliminated in the urine. A modern chelating agent used for this purpose is succimer (C4H6O4S2). Suppose you are trying to determine the appropriate dose for succimer treatment of lead poisoning. What minimum mass of succimer (in mg) is needed to bind all of the lead in a patient’s bloodstream? Assume that patient blood lead levels are 45 g/dL , that total blood volume is 5.0 L, and that 1 mole of succimer binds 1 mole of lead.

A particular kind of emergency breathing apparatus—often placed in mines, caves, or other places where oxygen might become depleted or where the air might become poisoned— works via the following chemical reaction: Notice that the reaction produces O2, which can be breathed, and absorbs CO2, a product of respiration. Suppose you work for a company interested in producing a self-rescue breathing apparatus (based on the given reaction) that would allow the user to survive for 10 minutes in an emergency situation. What are the important chemical considerations in designing such a unit? Estimate how much KO2 would be required for the apparatus. (Find any necessary additional information—such as human breathing rates—from appropriate sources. Assume that normal air is 20% oxygen.)

Metallic aluminum reacts with MnO2 at elevated temperatures to form manganese metal and aluminum oxide. A mixture of the two reactants is 67.2% mole percent Al. Find the theoretical yield (in grams) of manganese from the reaction of 250 g of this mixture.

Hydrolysis of the compound B5H9 forms boric acid, H3BO3. Fusion of boric acid with sodium oxide forms a borate salt, Na2B4O7. Without writing complete equations, find the mass (in grams) of B5H9 required to form 151 g of the borate salt by this reaction sequence.

Consider the reaction: The molar mass of K is 39.09 g/mol and that of O2 is 32.00 g/mol. Without doing any calculations, pick the conditions under which potassium is the limiting reactant and explain your reasoning. a. 170 g K, 31 g O2 b. 16 g K, 2.5 g O2 c. 165 kg K, 28 kg O2 d. 1.5 g K, 0.38 g O2

Consider the reaction: A reaction mixture initially contains 5 moles of NO and 10 moles of H2. Without doing any calculations, determine which set of amounts best represents the mixture after the reactants have reacted as completely as possible. Explain your reasoning.

The following circle represents 1.0 liter of a solution with a solute concentration of 1 M: Explain what you would add (the amount of solute or volume of solvent) to the solution to obtain a solution represented by each diagram:

Consider the reaction: \(2 \ \mathrm{N}_{2} \mathrm{H}_{4}(g)+\mathrm{N}_{2} \mathrm{O}_{4}(g) \ \rightarrow \ 3 \ \mathrm{N}_{2}(g)+4 \ \mathrm{H}_{2} \mathrm{O}(g)\) Consider also this representation of an initial mixture of \(\mathrm{N}_{2} \mathrm{H}_{4}\) and \(\mathrm{N}_{2} \mathrm{O}_{4}\): Which diagram best represents the reaction mixture after the reactants have reacted as completely as possible?

Consider the generic ionic compounds with the formulas A2X and BY2 and the following solubility rules: A2X soluble; BY2 soluble; AY insoluble; BX soluble. Let A+ ions be represented by circles, B2+ ions be represented by squares, X2- ions be represented by triangles, and Y- ions be represented by diamonds. Solutions of the two compounds (A2X and BY2) can be represented as follows: Draw a molecular level representation showing the result of mixing the two solutions given and write an equation to represent the reaction.

Write a brief paragraph about a time that you used multiple sources to help make a decision. You can choose something as simple as a decision about which movie to see or which shoes to purchase or as serious as which colleges to apply to. Discuss how each source contributed to your decision and how you decided which ones were more or less influential. You may consult written sources as well as more informal ones such as conversations.

How does the structure of the community service program affect its perceived value? Is it part of academic study? Are there choices?

How would making community service mandatory affect the fact that many students volunteer for selfish reasons, namely, padding their resumes for college?

What values about community and education underlie a service requirement?

Explain the difference between a strong acid and a weak acid.

What influence does socioeconomic status play in such a requirement? For example, if students need to earn money in their free time, can required community service programs be designed to accommodate them?

How does a school system determine how many hours of service to require?

What are the cations and anions whose compounds are usually soluble? What are the exceptions? What are the anions whose compounds are mostly insoluble? What are the exceptions?

What is a precipitation reaction? Give an example.

How can you predict whether a precipitation reaction will occur upon mixing two aqueous solutions?

Explain how a molecular equation, a complete ionic equation, and a net ionic equation differ

What is the Arrhenius definition of an acid? A base?

What is an acidbase reaction? Give an example. 16. Explain the principles behind an acidbase titration.

Explain the principles behind an acidbase titration. What is an indicator?

What is a gas-evolution reaction? Give an example.

What reactant types give rise to gas-evolution reactions?

What is an oxidationreduction reaction? Give an example.

What are oxidation states?

How can oxidation states be used to identify redox reactions?

What happens to a substance when it becomes oxidized? Reduced?

In a redox reaction, which reactant is the oxidizing agent? The reducing agent?

What is a combustion reaction? Why are they important? Give an example.

Consider the unbalanced equation for the combustion of hexane: C6H14(g) + O2(g) S CO2(g) + H2O(g) Balance the equation and determine how many moles of O2 are required to react completely with 7.2 moles of C6H14.

Consider the unbalanced equation for the neutralization of acetic acid: \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Ba}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}(a q)\) Balance the equation and determine how many moles of \(\mathrm{Ba}(\mathrm{OH})_{2}\) are required to completely neutralize 0.461 mole of \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\).

Calculate how many moles of NO2 form when each quantity of reactant completely reacts. 2 N2O5 (g) S 4 NO2(g) + O2 (g) a. 2.5 mol N2O5 b. 6.8 mol N2O5 c. 15.2 g N2O5 d. 2.87 kg N2O5

Calculate how many moles of NH3 form when each quantity of reactant completely reacts. 3 N2H4(l) S 4 NH3(g) + N2(g) a. 2.6 mol N2H4 b. 3.55 mol N2H4 c. 65.3 g N2H4 d. 4.88 kg N2H4

Consider the balanced equation: SiO2(s) + 3 C(s) S SiC(s) + 2 CO(g) Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that is made.

Consider the balanced equation \(2\mathrm{\ N}_2\mathrm{H}_4(g)+\mathrm{N}_2\mathrm{O}_4(g)\rightarrow3\mathrm{\ N}_2(g)+4\mathrm{\ H}_2\mathrm{O}(g)\) Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that is made.

Hydrobromic acid dissolves solid iron according to the reaction: Fe(s) + 2 HBr(aq) S FeBr2(aq) + H2(g) What mass of HBr (in g) do you need to dissolve a 3.2 g pure iron bar on a padlock? What mass of H2 would the complete reaction of the iron bar produce?

Sulfuric acid dissolves aluminum metal according to the reaction: 2 Al(s) + 3 H2SO4(aq) S Al2(SO4)3(aq) + 3 H2(g) Suppose you want to dissolve an aluminum block with a mass of 15.2 g. What minimum mass of H2SO4 (in g) do you need? What mass of H2 gas (in g) does the complete reaction of the aluminum block produce?

For each of the reactions, calculate the mass (in grams) of the product that forms when 3.67 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant. a. Ba(s) + Cl2(g) S BaCl2(s) b. CaO(s) + CO2(g) S CaCO3(s) c. 2 Mg(s) + O2(g) S 2 MgO(s) d. 4 Al(s) + 3 O2(g) S 2 Al2O3(s)

For each of the reactions, calculate the mass (in grams) of the product that forms when 15.39 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant. a. 2 K(s) + Cl2(g) S 2 KCl(s) b. 2 K(s) + Br2(l) S 2 KBr(s) c. 4 Cr(s) + 3 O2(g) S 2 Cr2O3(s) d. 2 Sr(s) + O2(g) S 2 SrO(s)

For each of the acidbase reactions, calculate the mass (in grams) of each acid necessary to completely react with and neutralize 4.85 g of the base. a. HCl(aq) + NaOH(aq) S H2O(l) + NaCl(aq) b. 2 HNO3(aq) + Ca(OH)2(aq) S 2 H2O(l) + Ca(NO3)2(aq) c. H2SO4(aq) + 2 KOH(aq) S 2 H2O(l) + K2SO4(aq)

For each precipitation reaction, calculate how many grams of the first reactant are necessary to completely react with 55.8 g of the second reactant. a. 2 KI(aq) + Pb(NO3)2(aq) S PbI2(s) + 2 KNO3(aq) b. Na2CO3(aq) + CuCl2(aq) S CuCO3(s) + 2 NaCl(aq) c. K2SO4(aq) + Sr(NO3)2(aq) S SrSO4(s) + 2 KNO3(aq)

For the following reaction, determine the limiting reactant for each of the initial amounts of reactants. 2 Na(s) + Br2(g) S 2 NaBr(s) a. 2 mol Na, 2 mol Br2 b. 1.8 mol Na, 1.4 mol Br2 c. 2.5 mol Na, 1 mol Br2 d. 12.6 mol Na, 6.9 mol Br2

Find the limiting reactant for each initial amount of reactants. 4 Al(s) + 3 O2 (g) S 2 Al2O3(s) a. 1 mol Al, 1 mol O2 b. 4 mol Al, 2.6 mol O2 c. 16 mol Al, 13 mol O2 d. 7.4 mol Al, 6.5 mol O2

Consider the reaction: 4 HCl(g) + O2(g) S 2 H2O(g) + 2 Cl2(g) Each molecular diagram represents an initial mixture of the reactants. How many molecules of Cl2 would be formed from the reaction mixture that produces the greatest amount of products?

Consider the reaction: 2 CH3OH(g) + 3 O2(g) S 2 CO2(g) + 4 H2O(g) Each of the molecular diagrams represents an initial mixture of the reactants. How many CO2 molecules would be formed from the reaction mixture that produces the greatest amount of products?

Calculate the theoretical yield of the product (in moles) for each initial amount of reactants. Ti(s) + 2 Cl2(g) S TiCl4(s) a. 4 mol Ti, 4 mol Cl2 b. 7 mol Ti, 17 mol Cl2 c. 12.4 mol Ti, 18.8 mol Cl2

Calculate the theoretical yield of product (in moles) for each initial amount of reactants. \(3\ \mathrm{Mn}(s)+2\mathrm{\ O}_2(g)\rightarrow\mathrm{Mn}^3\mathrm{O}_4(s)\) a. \(3\mathrm{\ mol\ }\mathrm{Mn},\ 3\ \mathrm{mol}\mathrm{\ O}_2\) b. \(4\mathrm{\ mol\ }\mathrm{Mn},\ 7\ \mathrm{mol}\mathrm{\ O}_2\) c. \(27.5\mathrm{\ mol\ }\mathrm{Mn},\ 43.8\ \mathrm{mol}\mathrm{\ O}_2\)

Zinc(II) sulfide reacts with oxygen according to the reaction: 2 ZnS(s) + 3 O2(g) S 2 ZnO(s) + 2 SO2(g) A reaction mixture initially contains 4.2 mol ZnS and 6.8 mol O2. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?

Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s) + 2 HCl(aq) S FeCl2(s) + H2S(g) A reaction mixture initially contains 0.223 mol FeS and 0.652 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?

For the reaction shown, calculate the theoretical yield of product (in grams) for each initial amount of reactants. 2 Al(s) + 3 Cl2(g) S 2 AlCl3(s) a. 2.0 g Al, 2.0 g Cl2 b. 7.5 g Al, 24.8 g Cl2 c. 0.235 g Al, 1.15 g Cl2

For the reaction shown, calculate the theoretical yield of the product (in grams) for each initial amount of reactants. Ti(s) + 2 F2(g) S TiF4(s) a. 5.0 g Ti, 5.0 g F2 b. 2.4 g Ti, 1.6 g F2 c. 0.233 g Ti, 0.288 g F2

Iron(III) sulfide reacts with carbon monoxide according to the equation: Fe2O3(s) + 3 CO(g) S 2 Fe(s) + 3 CO2(g) A reaction mixture initially contains 22.55 g Fe2O3 and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?

Elemental phosphorus reacts with chlorine gas according to the equation: P4(s) + 6 Cl2(g) S 4 PCl3(l) A reaction mixture initially contains 45.69 g P4 and 131.3 g Cl2. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?

Lead ions can be precipitated from solution with KCl according to the reaction: Pb2+(aq) + 2 KCl(aq) S PbCl2(s) + 2 K+(aq) When 28.5 g KCl is added to a solution containing 25.7 g Pb2+ , a PbCl2 precipitate forms. The precipitate is filtered and dried and found to have a mass of 29.4 g. Determine the limiting reactant, theoretical yield of PbCl2, and percent yield for the reaction.

Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is 2 Mg(s) + O2(g) S 2 MgO(s) When 10.1 g of Mg reacts with 10.5 g O2, 11.9 g MgO is collected. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

Urea ( CH4N2O ) is a common fertilizer that is synthesized by the reaction of ammonia ( NH3 ) with carbon dioxide: 2 NH3(aq) + CO2(aq) S CH4N2O(aq) + H2O(l) In an industrial synthesis of urea, a chemist combines 136.4 kg of ammonia with 211.4 kg of carbon dioxide and obtains 168.4 kg of urea. Determine the limiting reactant, theoretical yield of urea, and percent yield for the reaction.

Many computer chips are manufactured from silicon, which occurs in nature as SiO2. When SiO2 is heated to melting, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 155.8 kg of SiO2 reacts with 78.3 kg of carbon to produce 66.1 kg of silicon. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

Calculate the molarity of each solution. a. 3.25 mol of LiCl in 2.78 L solution b. 28.33 g C6H12O6 in 1.28 L of solution c. 32.4 mg NaCl in 122.4 mL of solution

Calculate the molarity of each solution. a. 0.38 mol of LiNO3 in 6.14 L of solution b. 72.8 g C2H6O in 2.34 L of solution c. 12.87 mg KI in 112.4 mL of solution

What is the molarity of NO3 - in each solution? a. 0.150 M KNO3 b. 0.150 M Ca(NO3)2 c. 0.150 M Al(NO3)3

What is the molarity of Cl- in each solution? a. 0.200 M NaCl b. 0.150 M SrCl2 c. 0.100 M AlCl3

How many moles of KCl are contained in each solution? a. 0.556 L of a 2.3 M KCl solution b. 1.8 L of a 0.85 M KCl solution c. 114 mL of a 1.85 M KCl solution

What volume of 0.200 M ethanol solution contains each amount in moles of ethanol? a. 0.45 mol ethanol b. 1.22 mol ethanol c. 1.2 * 10-2 mol ethanol

A laboratory procedure calls for making 400.0 mL of a 1.1 M NaNO3 solution. What mass of NaNO3 (in g) is needed?

A chemist wants to make 5.5 L of a 0.300 M CaCl2 solution. What mass of CaCl2 (in g) should the chemist use?

If 123 mL of a 1.1 M glucose solution is diluted to 500.0 mL, what is the molarity of the diluted solution?

If 3.5 L of a 4.8 M SrCl2 solution is diluted to 45 L, what is the molarity of the diluted solution?

To what volume should you dilute 50.0 mL of a 12 M stock HNO3 solution to obtain a 0.100 M HNO3 solution?

To what volume should you dilute 25 mL of a 10.0 M H2SO4 solution to obtain a 0.150 M H2SO4 solution?

Consider the precipitation reaction: 2 Na3PO4(aq) + 3 CuCl2(aq) S Cu3(PO4)2(s) + 6 NaCl(aq) What volume of 0.175 M Na3PO4 solution is necessary to completely react with 95.4 mL of 0.102 M CuCl2 ?

Consider the reaction: Li2S(aq) + Co(NO3)2(aq) S 2 LiNO3(aq) + CoS(s) What volume of 0.150 M Li2S solution is required to completely react with 125 mL of 0.150 M Co(NO3)2 ?

What is the minimum amount of 6.0 M H2SO4 necessary to produce 25.0 g of H2 (g) according to the reaction between aluminum and sulfuric acid? 2 Al(s) + 3 H2SO4(aq) S Al2(SO4)3(aq) + 3 H2(g)

What is the molarity of ZnCl2 that forms when 25.0 g of zinc completely reacts with CuCl2 according to the following reaction? Assume a final volume of 275 mL. Zn(s) + CuCl2(aq) S ZnCl2(aq) + Cu(s)

A 25.0 mL sample of a 1.20 M potassium chloride solution is mixed with 15.0 mL of a 0.900 M barium nitrate solution and this precipitation reaction occurs: 2 KCl(aq) + Ba(NO3)2(aq) S BaCl2(s) + 2 KNO3(aq) The solid BaCl2 is collected, dried, and found to have a mass of 2.45 g. Determine the limiting reactant, the theoretical yield, and the percent yield.

A 55.0 mL sample of a 0.102 M potassium sulfate solution is mixed with 35.0 mL of a 0.114 M lead(II) acetate solution and this precipitation reaction occurs: K2SO4(aq) + Pb(C2H3O2)2(aq) S 2 KC2H3O2(aq) + PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 1.01 g. Determine the limiting reactant, the theoretical yield, and the percent yield.

For each compound (all water soluble), would you expect the resulting aqueous solution to conduct electrical current? a. CsCl b. CH3OH c. Ca(NO2)2 d. C6H12O6

Classify each compound as a strong electrolyte or nonelectrolyte. a. MgBr2 b. C12H22O11 c. Na2CO3 d. KOH

Determine whether each compound is soluble or insoluble. If the compound is soluble, list the ions present in solution. a. AgNO3 b. Pb(C2H3O2)2 c. KNO3 d. (NH4)2 S

Determine whether each compound is soluble or insoluble. For the soluble compounds, list the ions present in solution. a. AgI b. Cu3(PO4)2 c. CoCO3 d. K3PO4

Complete and balance each equation. If no reaction occurs, write NO REACTION. a. LiI(aq) + BaS(aq) S b. KCl(aq) + CaS(aq) S c. CrBr2(aq) + Na2CO3(aq) S d. NaOH(aq) + FeCl3(aq) S

Complete and balance each equation. If no reaction occurs, write “NO REACTION.” a. \(\mathrm{NaNO}_{3}(a q)+\mathrm{KCl}(a q) \ \rightarrow\) b. \(\mathrm{NaCl}(a q)+\mathrm{Hg}_{2}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}(a q) \ \rightarrow\) c. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(a q)+\mathrm{SrCl}_{2}(a q) \ \rightarrow\) d. \(\mathrm{NH}_{4} \mathrm{Cl}(a q)+\mathrm{AgNO}_{3}(a q) \ \rightarrow\)

Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write NO REACTION. a. potassium carbonate and lead(II) nitrate b. lithium sulfate and lead(II) acetate c. copper(II) nitrate and magnesium sulfide d. strontium nitrate and potassium iodide

Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write NO REACTION. a. sodium chloride and lead(II) acetate b. potassium sulfate and strontium iodide c. cesium chloride and calcium sulfide d. chromium(III) nitrate and sodium phosphate

Write balanced complete ionic and net ionic equations for each reaction. a. HCl(aq) + LiOH(aq) S H2O(l) + LiCl(aq) b. MgS(aq) + CuCl2(aq) S CuS(s) + MgCl2(aq) c. NaOH(aq) + HC2H3O2(aq) S H2O(l) + NaC2H3O2(aq) d. Na3PO4(aq) + NiCl2(aq) S Ni3(PO4)2(s) + NaCl(aq)

Write balanced complete ionic and net ionic equations for each reaction. a. K2SO4(aq) + CaI2(aq) S CaSO4(s) + KI(aq) b. NH4Cl(aq) + NaOH(aq) S H2O(l) + NH3(g) + NaCl(aq) c. AgNO3(aq) + NaCl(aq) S AgCl(s) + NaNO3(aq) d. HC2H3O2(aq) + K2CO3(aq) S H2O(l) + CO2(g) + KC2H3O2(aq)

Mercury(I) ions (Hg2 2+) can be removed from solution by precipitation with Cl- . Suppose that a solution contains aqueous Hg2(NO3)2. Write complete ionic and net ionic equations to show the reaction of aqueous Hg2(NO3)2 with aqueous sodium chloride to form solid Hg2Cl2 and aqueous sodium nitrate.

Lead(II) ions can be removed from solution by precipitation with sulfate ions. Suppose that a solution contains lead(II) nitrate. Write complete ionic and net ionic equations to show the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate.

Write balanced molecular and net ionic equations for the reaction between hydrobromic acid and potassium hydroxide.

Write balanced molecular and net ionic equations for the reaction between nitric acid and calcium hydroxide.

Complete and balance each acidbase equation. a. H2SO4(aq) + Ca(OH)2(aq) S b. HClO4(aq) + KOH(aq) S c. H2SO4(aq) + NaOH(aq) S

Complete and balance each acidbase equation. a. HI(aq) + LiOH(aq) S b. HC2H3O2(aq) + Ca(OH)2(aq) S c. HCl(aq) + Ba(OH)2(aq) S

A 25.00 mL sample of an unknown HClO4 solution requires titration with 22.62 mL of 0.2000 M NaOH to reach the equivalence point. What is the concentration of the unknown HClO4 solution? The neutralization reaction is HClO4(aq) + NaOH(aq) S H2O(l) + NaClO4(aq)

A 30.00 mL sample of an unknown H3PO4 solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.38 mL of NaOH solution is added. What is the concentration of the unknown H3PO4 solution? The neutralization reaction is H3PO4(aq) + 3 NaOH(aq) S 3 H2O(l) + Na3PO4(aq)

Complete and balance each gas-evolution equation. a. HBr(aq) + NiS(s) S b. NH4I(aq) + NaOH(aq) S c. HBr(aq) + Na2S(aq) S d. HClO4(aq) + Li2CO3(aq) S

Complete and balance each gas-evolution equation. a. HNO3(aq) + Na2SO3(aq) S b. HCl(aq) + KHCO3(aq) S c. HC2H3O2(aq) + NaHSO3(aq) S d. (NH4)2SO4(aq) + Ca(OH)2(aq) S

Assign oxidation states to each atom in each element, ion, or compound. a. Ag b. Ag+ c. CaF2 d. H2S e. CO3 2- f. CrO4 2-

Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. a. Al(s) + 3 Ag+(aq) S Al3+(aq) + 3 Ag(s) b. SO3(g) + H2O(l) S H2SO4(aq) c. Ba(s) + Cl2(g) S BaCl2(s) d. Mg(s) + Br2(l) S MgBr2(s)

Complete and balance each combustion reaction equation. a. S(s) + O2(g) S b. C3H6(g) + O2(g) S c. Ca(s) + O2(g) S d. C5H12S(l) + O2(g) S

Find the percent by mass of sodium chloride in a 1.35 M NaCl solution. The density of the solution is 1.05 g>mL.

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane ( C8H18 ) and calculate the mass (in kg) of carbon dioxide that is added to the atmosphere per 1.0 kg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)

Aspirin can be made in the laboratory by reacting acetic anhydride ( C4H6O3 ) with salicylic acid ( C7H6O3 ) to form aspirin ( C9H8O4 ) and acetic acid ( C2H4O2 ). The balanced equation is C4H6O3 + C7H6O3 S C9H8O4 + C2H4O2 In a laboratory synthesis, a student begins with 3.00 mL of acetic anhydride (density = 1.08 g>mL) and 1.25 g of salicylic acid. Once the reaction is complete, the student collects 1.22 g of aspirin. Determine the limiting reactant, theoretical yield of aspirin, and percent yield for the reaction.

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write NO REACTION. a. HCl(aq) + Hg2(NO3)2(aq) S b. KHSO3(aq) + HNO3(aq) S c. aqueous ammonium chloride and aqueous lead(II) nitrate d. aqueous ammonium chloride and aqueous calcium hydroxide

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write NO REACTION. a. H2SO4(aq) + HNO3(aq) S b. Cr(NO3)3(aq) + LiOH(aq) S c. liquid pentanol ( C5H12O ) and gaseous oxygen d. aqueous strontium sulfide and aqueous copper(II) sulfate

Find the volume of 0.110 M hydrochloric acid necessary to react completely with 1.52 g Al(OH)3.

Treatment of gold metal with BrF3 and KF produces Br2 and KAuF4, a salt of gold. Identify the oxidizing agent and the reducing agent in this reaction. Find the mass of the gold salt that forms when a 73.5 g mixture of equal masses of all three reactants is prepared.

We prepare a solution by mixing 0.10 L of 0.12 M sodium chloride with 0.23 L of a 0.18 M MgCl2 solution. What volume of a 0.20 M silver nitrate solution do we need to precipitate all the Cl- ion in the solution as AgCl?

A solution contains one or more of the following ions: Ag+, Ca2+ , and Cu2+. When you add sodium chloride to the solution, no precipitate forms. When you add sodium sulfate to the solution, a white precipitate forms. You filter off the precipitate and add sodium carbonate to the remaining solution, producing another precipitate. Which ions were present in the original solution? Write net ionic equations for the formation of each of the precipitates observed.

A solution contains one or more of the following ions: Hg2 2+ , Ba2+ , and Fe2+. When potassium chloride is added to the solution, a precipitate forms. The precipitate is filtered off, and potassium sulfate is added to the remaining solution, producing no precipitate. When potassium carbonate is added to the remaining solution, a precipitate forms. Which ions were present in the original solution? Write net ionic equations for the formation of each of the precipitates observed.

The reaction of NH3 and O2 forms NO and water. The NO can be used to convert P4 to P4O6, forming N2 in the process. The P4O6 can be treated with water to form H3PO3, which forms PH3 and H3PO4 when heated. Find the mass of PH3 that forms from the reaction of 1.00 g NH3.

An important reaction that takes place in a blast furnace during the production of iron is the formation of iron metal and CO2 from Fe2O3 and CO. Determine the mass of Fe2O3 required to form 910 kg of iron. Determine the amount of CO2 that forms in this process.

A liquid fuel mixture contains 30.35% hexane ( C6H14 ), 15.85% heptane ( C7H16 ), and the rest octane ( C8H18 ). What maximum mass of carbon dioxide is produced by the complete combustion of 10.0 kg of this fuel mixture?

Titanium occurs in the magnetic mineral ilmenite ( FeTiO3 ), which is often found mixed up with sand. The ilmenite can be separated from the sand with magnets. The titanium can then be extracted from the ilmenite by the following set of reactions: FeTiO3(s) + 3 Cl2(g) + 3 C(s) S 3 CO(g) + FeCl2(s) + TiCl4(g) TiCl4(g) + 2 Mg(s) S 2 MgCl2(l) + Ti(s) Suppose that an ilmenitesand mixture contains 22.8% ilmenite by mass and that the first reaction is carried out with a 90.8% yield. If the second reaction is carried out with an 85.9% yield, what mass of titanium can be obtained from 1.00 kg of the ilmenitesand mixture?

A mixture of \(\mathrm{C}_{3} \mathrm{H}_{8}\) and \(\mathrm{C}_{2} \mathrm{H}_{2}\) has a mass of 2.0 g. It is burned in excess \(\mathrm{O}_{2}\) to form a mixture of water and carbon dioxide that contains 1.5 times as many moles of \(\mathrm{CO}_{2}\) as of water. Find the mass of \(\mathrm{C}_{2} \mathrm{H}_{2}\) in the original mixture.

A mixture of 20.6 g of P and 79.4 g Cl2 reacts completely to form PCl3 and PCl5 as the only products. Find the mass of PCl3 that forms.

A solution contains Ag+ and Hg2+ ions. The addition of 0.100 L of 1.22 M NaI solution is just enough to precipitate all the ions as AgI and HgI2. The total mass of the precipitate is 28.1 g. Find the mass of AgI in the precipitate.

The water in lakes that have been acidified by acid rain (HNO3 and H2SO4 ) can be neutralized by a process called liming, in which limestone ( CaCO3 ) is added to the acidified water. What mass of limestone (in kg) would completely neutralize a 15.2 billion-liter lake that is 1.8 * 10-5 M in H2SO4 and 8.7 * 10-6 M in HNO3 ?

Recall from Section 4.6 that sodium carbonate is often added to laundry detergents to soften hard water and make the detergent more effective. Suppose that a particular detergent mixture is designed to soften hard water that is 3.5 * 10-3 M in Ca2+ and 1.1 * 10-3 M in Mg2+ and that the average capacity of a washing machine is 19.5 gallons of water. If the detergent requires using 0.65 kg detergent per load of laundry, what percentage (by mass) of the detergent should be sodium carbonate in order to completely precipitate all of the calcium and magnesium ions in an average load of laundry water?

Lead poisoning is a serious condition resulting from the ingestion of lead in food, water, or other environmental sources. It affects the central nervous system, leading to a variety of symptoms such as distractibility, lethargy, and loss of motor coordination. Lead poisoning is treated with chelating agents, substances that bind to metal ions, allowing them to be eliminated in the urine. A modern chelating agent used for this purpose is succimer ( C4H6O4S2 ). Suppose you are trying to determine the appropriate dose for succimer treatment of lead poisoning. What minimum mass of succimer (in mg) is needed to bind all of the lead in a patients bloodstream? Assume that patient blood lead levels are 45 mg>dL , that total blood volume is 5.0 L, and that 1 mole of succimer binds 1 mole of lead.

A particular kind of emergency breathing apparatusoften placed in mines, caves, or other places where oxygen might become depleted or where the air might become poisoned works via the following chemical reaction: 4 KO2 (s) + 2 CO2 (g) S 2 K2CO3 (s) + 3 O2(g) Notice that the reaction produces O2 , which can be breathed, and absorbs CO2, a product of respiration. Suppose you work for a company interested in producing a self-rescue breathing apparatus (based on the given reaction) that would allow the user to survive for 10 minutes in an emergency situation. What are the important chemical considerations in designing such a unit? Estimate how much KO2 would be required for the apparatus. (Find any necessary additional informationsuch as human breathing ratesfrom appropriate sources. Assume that normal air is 20% oxygen.)

Metallic aluminum reacts with MnO2 at elevated temperatures to form manganese metal and aluminum oxide. A mixture of the two reactants is 67.2% mole percent Al. Find the theoretical yield (in grams) of manganese from the reaction of 250 g of this mixture.

Hydrolysis of the compound B5H9 forms boric acid, H3BO3. Fusion of boric acid with sodium oxide forms a borate salt, Na2B4O7. Without writing complete equations, find the mass (in grams) of B5H9 required to form 151 g of the borate salt by this reaction sequence.

Consider the reaction: 4 K(s) + O2 (g) S 2 K2O(s) The molar mass of K is 39.09 g>mol and that of O2 is 32.00 g>mol. Without doing any calculations, pick the conditions under which potassium is the limiting reactant and explain your reasoning. a. 170 g K, 31 g O2 b. 16 g K, 2.5 g O2 c. 165 kg K, 28 kg O2 d. 1.5 g K, 0.38 g O2

Consider the reaction: 2 NO(g) + 5 H2 (g) S 2 NH3 (g) + 2 H2O(g) A reaction mixture initially contains 5 moles of NO and 10 moles of H2. Without doing any calculations, determine which set of amounts best represents the mixture after the reactants have reacted as completely as possible. Explain your reasoning. a. 1 mol NO, 0 mol H2, 4 mol NH3, 4 mol H2O b. 0 mol NO, 1 mol H2, 5 mol NH3, 5 mol H2O c. 3 mol NO, 5 mol H2, 2 mol NH3, 2 mol H2O d. 0 mol NO, 0 mol H2, 4 mol NH3, 4 mol H2O

The following circle represents 1.0 liter of a solution with a solute concentration of 1 M: Explain what you would add (the amount of solute or volume of solvent) to the solution to obtain a solution represented by each diagram:

Consider the reaction: \(2 \ \mathrm{N}_{2} \mathrm{H}_{4}(g)+\mathrm{N}_{2} \mathrm{O}_{4}(g) \ \rightarrow \ 3 \ \mathrm{N}_{2}(g)+4 \ \mathrm{H}_{2} \mathrm{O}(g)\) Consider also this representation of an initial mixture of \(\mathrm{N}_{2} \mathrm{H}_{4}\) and \(\mathrm{N}_{2} \mathrm{O}_{4}\): Which diagram best represents the reaction mixture after the reactants have reacted as completely as possible?

Consider the generic ionic compounds with the formulas A2X and BY2 and the following solubility rules: A2X soluble; BY2 soluble; AY insoluble; BX soluble. Let A+ ions be represented by circles, B2+ ions be represented by squares, X2- ions be represented by triangles, and Y- ions be represented by diamonds. Solutions of the two compounds (A2X and BY2) can be represented as follows: A+ X2 B2+ Y Draw a molecular level representation showing the result of mixing the two solutions given and write an equation to represent the reaction.