Chemistry

Chemistry: The Central Science | 13th Edition | ISBN: 9780321910417 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
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Author: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
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ISBN: 9780321910417
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Chapter: Problem: 48E

Chemistry: The Central Science 13
Problem 48E Oxidation-Reduction Reactions (Section) Determine the oxidation number of sulfur in each of the following substances: (a) barium sulfate, BaSO4, (b) sulfurous acid, H2SO3, (c) strontium sulfide, SrS, (d) hydrogen sulfide, H2S. (e) Locate sulfur in the periodic table in Exercise 4.47;

Chapter: Problem: 115IE

Chemistry: The Central Science 13
Federal regulations set an upper limit of 50 parts per million (ppm) of \(N H_{3}\) in the air in a work environment [that is, 50 molecules of \(N H_{3}\)(g) for every million molecules in the air]. Air from a manufacturing operation was drawn through a solution containing \(\text { 1. } 00 \times 10

Chapter: Problem: 114IE

Chemistry: The Central Science 13
The U.S. 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, \(\mathrm{AsO}_{4}^{3-}\), what mass of sodium arsenate would be present in a 1.00-L sample of drinking water t

Chapter: Problem: 112IE

Chemistry: The Central Science 13
Problem 112IE 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 percen

Chapter: Problem: 113IE

Chemistry: The Central Science 13
Problem 113IE 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

Chapter: Problem: 111IE

Chemistry: The Central Science 13
Problem 111IE 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 on

Chapter: Problem: 1DE

Chemistry: The Central Science 13
Problem 1DE You are cleaning out a chemistry lab and find three unlabeled bottles, each containing white powder. Nearby these bottles are three loose labels: Sodium sulfide,' Sodium bicarbonate' and Sodium chloride.' Lets design an experiment to figure out which label goes with which bottle. (a)

Chapter: Problem: 1E

Chemistry: The Central Science 13
Visualizing Concepts Which of the following schematic drawings best describes a solution of \(\mathrm{Li}_{2} \mathrm{SO}_{4}\) in water (water molecules not shown for simplicity)? [Section 4.1] Equation Transcription:

Chapter: Problem: 2E

Chemistry: The Central Science 13
Visualizing Concepts Aqueous solutions of three different substances, AX, AY, and AZ, are represented by the three accompanying diagrams. Identify each substance as a strong electrolyte, a weak electrolyte, or a nonelectrolyte. [Section 4.1]

Chapter: Problem: 3E

Chemistry: The Central Science 13
Visualizing Concepts Use the molecular representations shown here to classify each compound as a nonelectrolyte, a weak electrolyte, or a strong electrolyte (see Figure 4.6 for element color scheme). [Sections 4.1 and 4.3]

Chapter: Problem: 4E

Chemistry: The Central Science 13
Problem 4E Visualizing Concepts The concept of chemical equilibrium is very important. Which one of the following statements is the most correct way to think about equilibrium? (a) If a system is at equilibrium, nothing is happening. (b) If a system is at equilibrium, the rate of

Chapter: Problem: 5E

Chemistry: The Central Science 13
Visualizing Concepts You are presented with a white solid and told that due to careless labeling it is not clear if the substance is barium chloride, lead chloride, or zinc chloride. When you transfer the solid to a beaker and add water, the solid dissolves to give a clear solution. Next a \(\mathr

Chapter: Problem: 6E

Chemistry: The Central Science 13
Problem 6E Visualizing Concepts We have seen that ions in aqueous solution are stabilized by the attractions between the ions and the water molecules. Why then do some pairs of ions in solution form precipitates? [Section]

Chapter: Problem: 7E

Chemistry: The Central Science 13
Problem 7E Visualizing Concepts Which of the following ions will always be a spectator ion in a precipitation reaction?(a) CI-, (b) NO3- (c) NH4+, (d) S2-, (e) SO4 2-.[Section]

Chapter: Problem: 8E

Chemistry: The Central Science 13
Problem 8E Visualizing Concepts The labels have fallen off three bottles containing powdered samples of metals; one contains zinc, one lead, and the other platinum. You have three solutions at your disposal: 1 M sodium nitrate, 1 M nitric acid, and 1 M nickel nitrate. How could you use these soluti

Chapter: Problem: 9E

Chemistry: The Central Science 13
Problem 9E Visualizing Concepts Explain how a redox reaction involves electrons in the same way that a neutralization reaction involves protons. [Sections]

Chapter: Problem: 11E

Chemistry: The Central Science 13
Visualizing Concepts Which data set, of the two graphed here, would you expect to observe from a titration like that shown in Figure 4.18? [Section 4.6]

Chapter: Problem: 10E

Chemistry: The Central Science 13
Problem 10E Visualizing Concepts If you want to double the concentration of a solution, how could you do it? [Section]

Chapter: Problem: 12E

Chemistry: The Central Science 13
Problem 12E Visualizing Concepts You are titrating an acidic solution with a basic one, and just realized you forgot to add the indicator that tells you when the equivalence point is reached. In this titration, the indicator turns blue at the equivalence point from an initially colorless solution

Chapter: Problem: 13E

Chemistry: The Central Science 13
Problem 13E General Properties of Aqueous Solutions (Section) State whether each of the statements below is true or false. Justify your answer in each case. (a) Electrolyte solutions conduct electricity because electrons are moving through the solution. (b) If you add a nonelectrolyte to an aqueo

Chapter: Problem: 14E

Chemistry: The Central Science 13
Problem 14E General Properties of Aqueous Solutions (Section) State whether each of the statements below is true or false. Justify your answer in each case. (a) When methanol, CH3OH, is dissolved in water, a conducting solution results. (b) When acetic acid, CH3COOH, dissolves in

Chapter: Problem: 15E

Chemistry: The Central Science 13
Problem 15E General Properties of Aqueous Solutions (Section) We have learned in this chapter that many ionic solids dissolve in water as strong electrolytes; that is, as separated ions in solution. Which statement is most correct about this process? (a) Water is a strong acid and therefore is go

Chapter: Problem: 16E

Chemistry: The Central Science 13
Problem 16E General Properties of Aqueous Solutions (Section) Would you expect that anions would be physically closer to the oxygen or to the hydrogens of water molecules that surround it in solution?

Chapter: Problem: 17E

Chemistry: The Central Science 13
Problem 17E General Properties of Aqueous Solutions (Section) Specify what ions are present in solution upon dissolving each of the following substances in water: (a) FeCI2, (b) HNO3, (c) (NH4)2SO4, (d) Ca(OH)2.

Chapter: Problem: 19E

Chemistry: The Central Science 13
Problem 19E General Properties of Aqueous Solutions (Section) Formic acid, HCOOH, is a weak electrolyte. What solutes are present in an aqueous solution of this compound? Write the chemical equation for the ionization of HCOOH

Chapter: Problem: 18E

Chemistry: The Central Science 13
Problem 18E General Properties of Aqueous Solutions (Section) Specify what ions are present upon dissolving each of the following substances in water: (a) Mgl2, (b) K2CO3, (c) HCIO4, (d) NaCH3COO.

Chapter: Problem: 20E

Chemistry: The Central Science 13
Problem 20E General Properties of Aqueous Solutions (Section) Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous acid, HCIO, is a weak electrolyte; and ammonium chloride, NH4CI, is a strong electrolyte, (a) What are the solutes present in aqueous solutions of each compound? (b) If 0.1 mol of each

Chapter: Problem: 21E

Chemistry: The Central Science 13
Problem 21E Precipitation Reactions (Section) Using solubility guidelines, predict whether each of the following compounds is soluble or insoluble in water: (a) MgBr2, (b) Pbl2, (c) (NH4)2CO3, (d) Sr(OH)2, (e) ZnSO4

Chapter: Problem: 22E

Chemistry: The Central Science 13
Problem 22E Precipitation Reactions (Section) Predict whether each of the following compounds is soluble in water: (a) Agl, (b) Na2CO3, (c) BaCI2, (d) AI(OH)3, (e) Zn(CH3COO)2.

Chapter: Problem: 23E

Chemistry: The Central Science 13
Problem 23E Precipitation Reactions (Section) Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction, (a) Na2CO3 and AgNO3, (b) NaNO3 and NiSO4, (c) FeSO4 and Pb(NO3)2.

Chapter: Problem: 24E

Chemistry: The Central Science 13
Problem 24E Precipitation Reactions (Section) Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction, (a) NaCH3COO and HCI, (b) KOH and Cu(NO3)2, (c) Na2S and CdSO4.

Chapter: Problem: 25E

Chemistry: The Central Science 13
Problem 25E Precipitation Reactions (Section) Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (a) potassium carbonate and magnesium sulfate (b) lead nitrate and lithium sulfide (c) ammonium phosphate and calcium chlorid

Chapter: Problem: 26E

Chemistry: The Central Science 13
Precipitation Reactions (Section 4.2) Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. (a) \(\mathrm{Cr}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}(a q

Chapter: Problem: 28E

Chemistry: The Central Science 13
Problem 28E Precipitation Reactions (Section) Separate samples of a solution of an unknown ionic compound are treated with dilute AgNO3, Pb(NO3)2, and BaCI2.Precipitates form in all three cases. Which of the following could be the anion of the unknown salt: BrO, CO32-, NO3-?

Chapter: Problem: 27E

Chemistry: The Central Science 13
Problem 27E Precipitation Reactions (Section) Separate samples of a solution of an unknown salt are treated with dilute solutions of HBr, H2SO4, and NaOH. A precipitate forms in all three cases. Which of the following cations could be present in the unknown salt solution: K+, Pb2+, Ba2+?

Chapter: Problem: 29E

Chemistry: The Central Science 13
Problem 29E You know that an unlabeled bottle contains an aqueous solution of one of the following: AgNO3, CaCI2, or AI2(SO4)3. A friend suggests that you test a portion of the solution with Ba(NO3)2 and then with NaCI solutions. According to your friend's logic, which of these chemical reactions c

Chapter: Problem: 30E

Chemistry: The Central Science 13
Problem 30E Precipitation Reactions (Section) Three solutions are mixed together to form a single solution; in the final solution, there are 0.2 mol Pb(CH3COO)2, 0.1 mol Na2S, and 0.1 mol CaCI2 present. What solid(s) will precipitate?

Chapter: Problem: 31E

Chemistry: The Central Science 13
Problem 31E Acids, Bases, and Neutralization Reactions (Section) Which of the following solutions is the most acidic? (a) 0.2 MLiOH, (b) 0.2 MHI, (c) 1.0 M methyl alcohol (CH3OH).

Chapter: Problem: 33E

Chemistry: The Central Science 13
Problem 33E Acids, Bases, and Neutralization Reactions (Section) State whether each of the following statements is true or false. Justify your answer in each case. (a) Sulfuric acid is a monoprotic acid. (b) HCI is a weak acid. (c) Methanol is a base.

Chapter: Problem: 32E

Chemistry: The Central Science 13
Problem 32E Acids, Bases, and Neutralization Reactions (Section) Which of the following solutions is the most basic? (a) 0.6 MNH3, (b) 0.150 MKOH, (c) 0.100 MBa(OH)2.

Chapter: Problem: 35E

Chemistry: The Central Science 13
Problem 35E Acids, Bases, and Neutralization Reactions (Section) Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions, (a)

Chapter: Problem: 34E

Chemistry: The Central Science 13
Problem 34E Acids, Bases, and Neutralization Reactions (Section) State whether each of the following statements is true or false. Justify your answer in each case. (a) NH3 contains no OH- ions, and yet its aqueous solutions are basic. (b) HF is a strong acid. (c) Althou

Chapter: Problem: 36E

Chemistry: The Central Science 13
Problem 36E Acids, Bases, and Neutralization Reactions (Section) An aqueous solution of an unknown solute is tested with litmus paper and found to be acidic. The solution is weakly conducting compared with a solution of NaCI of the same concentration. Which of the following substances could the u

Chapter: Problem: 37E

Chemistry: The Central Science 13
Problem 37E Acids, Bases, and Neutralization Reactions (Section) Classify each of the following substances as a nonelectrolyte.weak electrolyte, or strong electrolyte in water: (a) H2SO3, (b) C2H5OH (ethanol), (c) NH3, (d) KCIO3, (e) Cu(NO3)2.

Chapter: Problem: 38E

Chemistry: The Central Science 13
Problem 38E Acids, Bases, and Neutralization Reactions (Section) Classify each of the following aqueous solutions as a nonelectrolyte, weak electrolyte, or strong electrolyte: (a) LiCIO4, (b) HCIO, (c) CH3CH2CH2OH (propanol), (d) HCIO3, (e) CuSO4, (f) C12H22O11 (sucrose).

Chapter: Problem: 39E

Chemistry: The Central Science 13
Acids, Bases, and Neutralization Reactions (Section 4.3) Complete and balance the following molecular equations, and then write the net ionic equation for each: (a) \(\mathrm{HBr}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow\) (b) \(\mathrm{Cu}(\mathrm{OH})_{2}(s)+\mathrm{HClO}_{4}(a q)

Chapter: Problem: 41E

Chemistry: The Central Science 13
Problem 41E Acids, Bases, and Neutralization Reactions (Section) Write balanced molecular and net ionic equations for the following reactions, and identify the gas formed in each: (a) solid cadmium sulfide reacts with an aqueous solution of sulfuric acid (b) solid magnesium carbonate reacts with

Chapter: Problem: 40E

Chemistry: The Central Science 13
Problem 40E Acids, Bases, and Neutralization Reactions (Section) Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (a) Aqueous acetic acid is neutralized by aqueous barium hydroxide. (b) Solid chromium(lll) hydroxide react

Chapter: Problem: 42E

Chemistry: The Central Science 13
Acids, Bases, and Neutralization Reactions (Section 4.3) Because the oxide ion is basic, metal oxides react readily with acids. (a) Write the net ionic equation for the following reaction: \(\mathrm{FeO}(s)+2 \mathrm{HClO}_{4}(a q) \longrightarrow \mathrm{Fe}\left(\mathrm{ClO}_{4}\right)_{2}(a q)+

Chapter: Problem: 43E

Chemistry: The Central Science 13
Problem 43E Acids, Bases, and Neutralization Reactions (Section) Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions, (a) Write a balanced molecular equation and a net ionic equation for the reaction that occurs when each substance rea

Chapter: Problem: 44E

Chemistry: The Central Science 13
Problem 44E Acids, Bases, and Neutralization Reactions (Section) As K2O dissolves in water, the oxide ion reacts with water molecules to form hydroxide ions, (a) Write the molecular and net ionic equations for this reaction, (b) Based on the definitions of acid and base, what ion is the base in thi

Chapter: Problem: 45E

Chemistry: The Central Science 13
Problem 45E Oxidation-Reduction Reactions (Section) True or false: (a) If a substance is oxidized, it is gaining electrons. (b) If an ion is oxidized, its oxidation number increases.

Chapter: Problem: 46E

Chemistry: The Central Science 13
Problem 46E Oxidation-Reduction Reactions (Section) True or false: (a) Oxidation can occur without oxygen. (b) Oxidation can occur without reduction.

Chapter: Problem: 47E

Chemistry: The Central Science 13
Oxidation-Reduction Reactions (Section 4.4) (a) Which region of the periodic table shown here contains elements that are easiest to oxidize? (b) Which region contains the least readily oxidized elements?

Chapter: Problem: 49E

Chemistry: The Central Science 13
Problem 49E Oxidation-Reduction Reactions (Section) Determine the oxidation number for the indicated element in each of the following substances: (a) S in SO2, (b) C in COCI2, (c) Mn in KMnO4, (d) Br in HBrO, (e) P in PF3, (f) 0 in K2O2.

Chapter: Problem: 50E

Chemistry: The Central Science 13
Problem 50E Oxidation-Reduction Reactions (Section) Determine the oxidation number for the indicated element in each of the following compounds: (a) Co in LiCoO2, (b) Alin NaAIH4, (c) C in CH3OH (methanol), (d) N in GaN, (e) Cl in HCIO2, (f) Cr in BaCr04.

Chapter: Problem: 51E

Chemistry: The Central Science 13
Oxidation-Reduction Reactions (Section 4.4) Which element is oxidized and which is reduced in the following reactions? (a) \(\mathrm{N}_{2}(g)+3\ \mathrm{H}_{2}(g) \longrightarrow 2\ \mathrm{NH}_{3}(g)\) (b) \(3\ \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{Al}(s) \longrightarrow 3\

Chapter: Problem: 53E

Chemistry: The Central Science 13
Problem 53E Oxidation-Reduction Reactions (Section) Write balanced molecular and net ionic equations for the reactions of (a) manganese with dilute sulfuric acid, (b) chromium with hydrobromic acid, (c) tin with hydrochloric acid, (d) aluminum with formic acid, HCOOH.

Chapter: Problem: 52E

Chemistry: The Central Science 13
Oxidation-Reduction Reactions (Section 4.4) Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or neutralization reactions. (a) \(\mathrm{P}_{4}(s)+10\ \mathrm{HClO}

Chapter: Problem: 54E

Chemistry: The Central Science 13
Problem 54E Oxidation-Reduction Reactions (Section) Write balanced molecular and net ionic equations for the reactions of (a) hydrochloric acid with nickel, (b) dilute sulphuric acid with iron, (c) hydrobromic acid with magnesium, (d) acetic acid, CH3COOH, with zinc.

Chapter: Problem: 55E

Chemistry: The Central Science 13
Oxidation-Reduction Reactions (Section 4.4) Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Iron metal is added to a solution of copper(II) nitrate, (b) zinc metal is added to a solution of magnesium sulfate,

Chapter: Problem: 56E

Chemistry: The Central Science 13
Oxidation-Reduction Reactions (Section 4.4) Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Nickel metal is added to a solution of copper(II) nitrate, (b) a solution of zinc nitrate is added to a solution of

Chapter: Problem: 57E

Chemistry: The Central Science 13
Problem 57E Oxidation-Reduction Reactions (Section) The metal cadmium tends to form Cd2+ ions. The following observations are made: (i) When a strip of zinc metal is placed in CdCI2(aq), cadmium metal is deposited on the strip, (ii) When a strip of cadmium metal is placed in Ni(NO3)2(aq), nickel me

Chapter: Problem: 58E

Chemistry: The Central Science 13
Oxidation-Reduction Reactions (Section 4.4) The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens: \(\mathrm{Br}_{2}(a q)+2\ \mathrm{NaI}(a q) & \longrightarrow 2\ \mathrm{NaBr}(a q)+\mathrm{I}_{2}(a q)\) \(

Chapter: Problem: 59E

Chemistry: The Central Science 13
Problem 59E Concentrations of Solutions (Section) (a) Is the concentration of a solution an intensive or an extensive property? (b) What is the difference between 0.50 mol HCI and 0.50 M HCI?

Chapter: Problem: 60E

Chemistry: The Central Science 13
Problem 60E Concentrations of Solutions (Section) Your lab partner tells you that he has prepared a solution that contains 1.50 moles of NaOH in 1.50 L of aqueous solution, and therefore that the concentration of NaOH is 1.5 M. (a) Is he correct? (b) If not, what is the correct concentration?

Chapter: Problem: 61E

Chemistry: The Central Science 13
Problem 61E Concentrations of Solutions (Section) (a) Calculate the molarity of a solution that contains 0.175 mol ZnCI2 in exactly 150 ml of solution, (b) How many moles of protons are present in 35.0 ml of a 4.50 M solution of nitric acid? (c) How many milliliters of a 6.00 M NaOH solution are ne

Chapter: Problem: 62E

Chemistry: The Central Science 13
Problem 62E Concentrations of Solutions (Section) (a) Calculate the molarity of a solution made by dissolving 12.5 grams of Na2CrO4 in enough water to form exactly 750 ml of solution, (b) How many moles of KBr are present in 150 ml of a 0.112 M solution? (c) How many milliliters of 6.1 M HCI soluti

Chapter: Problem: 63E

Chemistry: The Central Science 13
Problem 63E Concentrations of Solutions (Section) The average adult human male has a total blood volume of 5.0 L. If the concentration of sodium ion in this average individual is 0.135 M, what is the mass of sodium ion circulating in the blood?

Chapter: Problem: 64E

Chemistry: The Central Science 13
Problem 64E Concentrations of Solutions (Section) A person suffering from hyponatremia has a sodium ion concentration in the blood of 0.118 M and a total blood volume of 4.6 L. What mass of sodium chloride would need to be added to the blood to bring the sodium ion concentration up to 0.138 M, assu

Chapter: Problem: 65E

Chemistry: The Central Science 13
Problem 65E Concentrations of Solutions (Section) The concentration of alcohol (CH3CH2OH) in blood, called the 'blood alcohol concentration' or BAC, is given in units of grams of alcohol per 100 ml of blood. The legal definition of intoxication, in many states of the United States, is that the BAC

Chapter: Problem: 66E

Chemistry: The Central Science 13
Problem 66E Concentrations of Solutions (Section) The average adult male has a total blood volume of 5.0 L. After drinking a few beers, he has a BAC of 0.10 (see Exercise). What mass of alcohol is circulating in his blood? Exercise The concentration of alcohol (CH3CH2OH) in blood, called the 'b

Chapter: Problem: 67E

Chemistry: The Central Science 13
Problem 67E Concentrations of Solutions (Section) (a) How many grams of ethanol, CH3CH2OH, should you dissolve in water to make 1.00 L of vodka (which is an aqueous solution that is 6.86 Methanol)? (b) Using the density of ethanol (0.789 g/mL), calculate the volume of ethanol you need to make 1.0

Chapter: Problem: 68E

Chemistry: The Central Science 13
Problem 68E Concentrations of Solutions (Section) One cup of fresh orange juice contains 124 mg of ascorbic acid (vitamin C, C6H8O6). Given that one cup = 236.6 mL, calculate the molarity of vitamin C in organic juice.

Chapter: Problem: 69E

Chemistry: The Central Science 13
Problem 69E Concentrations of Solutions (Section) (a) Which will have the highest concentration of potassium ion: 0.20 M KCI, 0.15 MK2CrO4, or 0.080 M K3PO4? (b) Which will contain the greater number of moles of potassium ion: 30.0 ml of 0.15 M K2CrO4 or 25.0 ml of 0.080 M K3PO4?

Chapter: Problem: 70E

Chemistry: The Central Science 13
Problem 70E Concentrations of Solutions (Section) In each of the following pairs, indicate which has the higher concentration of I- ion: (a) 0.10 M Bal2 or 0.25 MKl solution, (b) 100 ml of 0.10 MKl solution or 200 ml of 0.040 M Znl2 solution, (c) 3.2 M HI solution or a solution made by dissolving

Chapter: Problem: 71E

Chemistry: The Central Science 13
Problem 71E Concentrations of Solutions (Section) Indicate the concentration of each ion or molecule present in the following solutions: (a) 0.25 MNaNO3, (b) 1.3 x 10-2 MMgSO4, (c) 0 . 0 1 5 0 MC6H12O6, (d) a mixture of45.0 ml of 0.272 M NaCI and 65.0 ml of 0.0247 M (NH4)2CO3. Assume that the vo

Chapter: Problem: 72E

Chemistry: The Central Science 13
Problem 72E Concentrations of Solutions (Section) Indicate the concentration of each ion present in the solution formed by mixing (a) 42.0 ml of 0.170 MNaOH with 37.6 ml of 0.400 MNaOH, (b) 44.0 ml of 0.100 MNa2S04 with 25.0 ml of 0.150 M KCI, (c) 3.60 g KCI in 75.0 ml of 0.250 M CaCI2 solution.

Chapter: Problem: 73E

Chemistry: The Central Science 13
Problem 73E Concentrations of Solutions (Section) (a) You have a stock solution of 14.8 MNH3. How many millilitres of this solution should you dilute to make 1000.0 ml of 0.250 MNH3? (b) If you take a 10.0-mL portion of the stock solution and dilute it to a total volume of 0.500 L, what will be the

Chapter: Problem: 75E

Chemistry: The Central Science 13
Problem 75E Concentrations of Solutions (Section) (a) Starting with solid sucrose, C12H22O11, describe how you would prepare 250 ml of a 0.250 M sucrose solution, (b) Describe how you would prepare 350.0 ml of 0.100 M C12H22O11 starting with 3.00 L of 1.50 MC12H22O11.

Chapter: Problem: 74E

Chemistry: The Central Science 13
Problem 74E Concentrations of Solutions (Section) (a) How many milliliters of a stock solution of 6.0 M HN03 would you have to use to prepare 110 ml of 0.500 MHNO3? (b) If you dilute 10.0 ml of the stock solution to a final volume of 0.250 L, what will be the concentration of the diluted solution?

Chapter: Problem: 77E

Chemistry: The Central Science 13
Problem 77E Concentrations of Solutions (Section) Pure acetic acid, known as glacial acetic acid, is a liquid with a density of 1.049 g/mL at 25 C. Calculate the molarity of a solution of acetic acid made by dissolving 20.00 ml of glacial acetic acid at 25 C in enough water to make 250.0 ml of solu

Chapter: Problem: 78E

Chemistry: The Central Science 13
Problem 78E Concentrations of Solutions (Section) Glycerol, C3H8O3, is a substance used extensively in the manufacture of cosmetics, foodstuffs, antifreeze, and plastics. Glycerol is a water-soluble liquid with a density of 1.2656 g/mL at 15 C. Calculate the molarity of a solution of glycerol mad

Chapter: Problem: 76E

Chemistry: The Central Science 13
Problem 76E Concentrations of Solutions (Section) (a) How many grams of solid silver nitrate would you need to prepare 200.0 ml of a 0.150 M AgNO3 solution? (b) An experiment calls for you to use 100 ml of 0.50 M HNO3 solution. All you have available is a bottle of 3.6 MHNO3. How many milliliters o

Chapter: Problem: 79E

Chemistry: The Central Science 13
Problem 79E Solution Stoichiometry and Chemical Analysis (Section) You want to analyze a silver nitrate solution, (a) You could add HCI(aq) to the solution to precipitate out AgCI(s). What volume of a 0.150 MHC\(aq) solution is needed to precipitate the silver ions from 15.0 ml of a 0.200 M AgN03 s

Chapter: Problem: 80E

Chemistry: The Central Science 13
Problem 80E Solution Stoichiometry and Chemical Analysis (Section) You want to analyze a cadmium nitrate solution. What mass of NaOH is needed to precipitate the Cd2+ ions from 35.0 ml of 0.500 MCd(NO3)2 solution?

Chapter: Problem: 81E

Chemistry: The Central Science 13
Problem 81E Solution Stoichiometry and Chemical Analysis (Section) (a)What volume of 0.115 MHCIO4 solution is needed to neutralize 50.00 ml of 0.0875 M NaOH? (b) What volume of 0.128 M HCI is needed to neutralize 2.87 g of Mg(OH)2? (c) If 25.8 ml of an AgNO3 solution is needed to precipitate all th

Chapter: Problem: 82E

Chemistry: The Central Science 13
Problem 82E Solution Stoichiometry and Chemical Analysis (Section) (a) How many milliliters of 0.120 M HCI are needed to completely neutralize 50.0 ml of 0.101 MBa(OH)2 solution? (b) How many milliliters of 0.125 MH2SO4 are needed to neutralize 0.200 g of NaOH? (c) If 55.8 ml of a BaCI2 solution

Chapter: Problem: 83E

Chemistry: The Central Science 13
Solution Stoichiometry and Chemical Analysis (Section 4.6) Some sulfuric acid is spilled on a lab bench. You can neutralize the acid by sprinkling sodium bicarbonate on it and then mopping up the resultant solution. The sodium bicarbonate reacts with sulfuric acid according to: \(2\ \mathrm{NaHCO}_

Chapter: Problem: 84E

Chemistry: The Central Science 13
Solution Stoichiometry and Chemical Analysis (Section 4.6) The distinctive odor of vinegar is due to acetic acid, \(\mathrm {CH_3COOH}\), which reacts with sodium hydroxide according to: \(\mathrm{CH}_{3} \mathrm{COO}(a q)+\mathrm{NaOH}(a q) \longrightarrow{\mathrm{H}_{2} \mathrm{O}(l)}+\mathrm{NaC

Chapter: Problem: 85E

Chemistry: The Central Science 13
Problem 85E Solution Stoichiometry and Chemical Analysis (Section) A4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100.0 ml of water. An acid-base indicator is added and the resulting solution is titrated with 2.50 M HCI(aq) solution. The indicator changes color signaling that t

Chapter: Problem: 88E

Chemistry: The Central Science 13
Problem 88E Solution Stoichiometry and Chemical Analysis (Section) A solution is made by mixing 15.0 g of Sr(OH)2 and 55.0 ml of 0.200 MHN03. (a) Write a balanced equation for the reaction that occurs between the solutes, (b) Calculate the concentration of each ion remaining in solution, (c) Is t

Chapter: Problem: 86E

Chemistry: The Central Science 13
Problem 86E Solution Stoichiometry and Chemical Analysis (Section) An 8.65-g sample of an unknown group 2A metal hydroxide is dissolved in 85.0 ml of water. An acid-base indicator is added and the resulting solution is titrated with 2.50 M HCI(ag) solution. The indicator changes color signaling t

Chapter: Problem: 87E

Chemistry: The Central Science 13
Problem 87E Solution Stoichiometry and Chemical Analysis (Section) A solution of 100.0 ml of 0.200 M KOH is mixed with a solution of 200.0 ml of 0.150 M NiS04. (a) Write the balanced chemical equation for the reaction that occurs, (b) What precipitate forms? (c) What is the limiting reactant? (d)

Chapter: Problem: 89E

Chemistry: The Central Science 13
Problem 89E Stoichiometry and Chemical Analysis (Section) A 0.5895-g sample of impure magnesium hydroxide is dissolved in 100.0 ml of 0.2050 MHCl solution. The excess acid then needs 19.85 ml of 0.1020 MNaOH for neutralization. Calculate the percentage by mass of magnesium hydroxide in the samp

Chapter: Problem: 90E

Chemistry: The Central Science 13
Problem 90E Stoichiometry and Chemical Analysis (Section) A 1.248-g sample of limestone rock is pulverized and then treated with 30.00 ml of 1.035 M HCI solution. The excess acid then requires 11.56 ml of 1.010 MNaOH for neutralization. Calculate the percentage by mass of calcium carbonate

Chapter: Problem: 91AE

Chemistry: The Central Science 13
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 i

Chapter: Problem: 92AE

Chemistry: The Central Science 13
The accompanying photo shows the reaction between a solution of \(\mathrm {Cd(NO_3)_2}\) and one of \(\mathrm {Na_2S}\). (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?

Chapter: Problem: 93AE

Chemistry: The Central Science 13
Problem 93AE 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. Thi

Chapter: Problem: 94AE

Chemistry: The Central Science 13
You choose to investigate some of the solubility guidelines for two ions not listed in Table 4.1, the chromate ion \(\left(\mathrm{CrO}_{4}^{2-}\right)\) and the oxalate ion \(\left(\mathrm{C}_{2} \mathrm{O}_{4}{ }^{2-}\right)\). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts

Chapter: Problem: 95AE

Chemistry: The Central Science 13
Problem 95AE 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) Mg

Chapter: Problem: 96AE

Chemistry: The Central Science 13
The commercial production of nitric acid involves the following chemical reactions: \(4\ \mathrm{NH}_{3}(g)+5\ \mathrm{O}_{2}(g) & \longrightarrow 4\ \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)\) \(2\ \mathrm{NO}(g)+\mathrm{O}_{2}(g) & \longrightarrow 2\ \mathrm{NO}_{2}(g)\) \(3\ \mathrm

Chapter: Problem: 97AE

Chemistry: The Central Science 13
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 ba

Chapter: Problem: 98AE

Chemistry: The Central Science 13
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

Chapter: Problem: 99AE

Chemistry: The Central Science 13
Problem 99AE 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?

Chapter: Problem: 100AE

Chemistry: The Central Science 13
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?

Chapter: Problem: 101AE

Chemistry: The Central Science 13
Problem 101AE 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

Chapter: Problem: 102AE

Chemistry: The Central Science 13
Problem 102AE 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

Chapter: Problem: 103AE

Chemistry: The Central Science 13
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 concentrati

Chapter: Problem: 104AE

Chemistry: The Central Science 13
Problem 104AE 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?

Chapter: Problem: 105IE

Chemistry: The Central Science 13
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)

Chapter: Problem: 106IE

Chemistry: The Central Science 13
Problem 106IE (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 i

Chapter: Problem: 107IE

Chemistry: The Central Science 13
Problem 107IE 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 bari

Chapter: Problem: 109IE

Chemistry: The Central Science 13
Problem 109IE 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?

Chapter: Problem: 108IE

Chemistry: The Central Science 13
Problem 108IE 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

Chapter: Problem: 110IE

Chemistry: The Central Science 13
Problem 110IE 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 t

Chapter: Problem: 4.1

Chemistry: The Central Science 13
Which of the following schematic drawings best describes a solution of \(Li_2SO_4\) in water (water molecules not shown for simplicity)? [Section 4.1]

Chapter: Problem: 4.2

Chemistry: The Central Science 13
Aqueous solutions of three different substances, AX, AY, and AZ, are represented by the three accompanying diagrams. Identify each substance as a strong electrolyte, a weak electrolyte, or a nonelectrolyte. [Section 4.1] + + + + + AX AY AZ (a) (b) (c)

Chapter: Problem: 4.3

Chemistry: The Central Science 13
Use the molecular representations shown here to classify each compound as a nonelectrolyte, a weak electrolyte, or a strong electrolyte (see Figure 4.6 for element color scheme). [Sections 4.1 and 4.3] (a) (b) (c)

Chapter: Problem: 4.4

Chemistry: The Central Science 13
The concept of chemical equilibrium is very important. Which one of the following statements is the most correct way to think about equilibrium? (a) If a system is at equilibrium, nothing is happening. (b) If a system is at equilibrium, the rate of the forward reaction is equal to the rate of the bac

Chapter: Problem: 4.5

Chemistry: The Central Science 13
You are presented with a white solid and told that due to careless labeling it is not clear if the substance is barium chloride, lead chloride, or zinc chloride. When you transfer the solid to a beaker and add water, the solid dissolves to give a clear solution. Next a Na2SO41aq2 solution is added an

Chapter: Problem: 4.6

Chemistry: The Central Science 13
We have seen that ions in aqueous solution are stabilized by the attractions between the ions and the water molecules. Why then do some pairs of ions in solution form precipitates? [Section 4.2]

Chapter: Problem: 4.7

Chemistry: The Central Science 13
Which of the following ions will always be a spectator ion in a precipitation reaction? (a) Cl -, (b) NO3 -, (c) NH4 +, (d) S2-, (e) SO4 2-. [Section 4.2]

Chapter: Problem: 4.8

Chemistry: The Central Science 13
The labels have fallen off three bottles containing powdered samples of metals; one contains zinc, one lead, and the other platinum. You have three solutions at your disposal: 1 M sodium nitrate, 1 M nitric acid, and 1 M nickel nitrate. How could you use these solutions to determine the identities of

Chapter: Problem: 4.9

Chemistry: The Central Science 13
Explain how a redox reaction involves electrons in the same way that a neutralization reaction involves protons. [Sections 4.3 and 4.4]

Chapter: Problem: 4.10

Chemistry: The Central Science 13
If you want to double the concentration of a solution, how could you do it? [Section 4.5]

Chapter: Problem: 4.11

Chemistry: The Central Science 13
Which data set, of the two graphed here, would you expect to observe from a titration like that shown in Figure 4.18? [Section 4.6] 0 2 4 6 8 10 12 No color Highly colored mL standard solution Color from indicator

Chapter: Problem: 4.12

Chemistry: The Central Science 13
You are titrating an acidic solution with a basic one, and just realized you forgot to add the indicator that tells you when the equivalence point is reached. In this titration, the indicator turns blue at the equivalence point from an initially colorless solution. You quickly grab a bottle of indica

Chapter: Problem: 4.13

Chemistry: The Central Science 13
State whether each of the statements below is true or false. Justify your answer in each case. (a) Electrolyte solutions conduct electricity because electrons are moving through the solution. (b) If you add a nonelectrolyte to an aqueous solution that already contains an electrolyte, the electrical c

Chapter: Problem: 4.14

Chemistry: The Central Science 13
State whether each of the statements below is true or false. Justify your answer in each case. (a) When methanol, CH3OH, is dissolved in water, a conducting solution results. (b) When acetic acid, CH3COOH, dissolves in water, the solution is weakly conducting and acidic in nature.

Chapter: Problem: 4.15

Chemistry: The Central Science 13
We have learned in this chapter that many ionic solids dissolve in water as strong electrolytes; that is, as separated ions in solution. Which statement is most correct about this process? (a) Water is a strong acid and therefore is good at dissolving ionic solids. (b) Water is good at solvating ions

Chapter: Problem: 4.16

Chemistry: The Central Science 13
Would you expect that anions would be physically closer to the oxygen or to the hydrogens of water molecules that surround it in solution?

Chapter: Problem: 4.17

Chemistry: The Central Science 13
Specify what ions are present in solution upon dissolving each of the following substances in water: (a) FeCl2, (b) HNO3, (c) 1NH422SO4, (d) Ca1OH22.

Chapter: Problem: 4.18

Chemistry: The Central Science 13
Specify what ions are present upon dissolving each of the following substances in water: (a) MgI2, (b) K2CO3, (c) HClO4, (d) NaCH3COO

Chapter: Problem: 4.19

Chemistry: The Central Science 13
Formic acid, HCOOH, is a weak electrolyte. What solutes are present in an aqueous solution of this compound? Write the chemical equation for the ionization of HCOOH.

Chapter: Problem: 4.20

Chemistry: The Central Science 13
Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH4Cl, is a strong electrolyte. (a) What are the solutes present in aqueous solutions of each compound? (b) If 0.1 mol of each compound is dissolved in solution, which one contains 0.2 mol o

Chapter: Problem: 4.21

Chemistry: The Central Science 13
Using solubility guidelines, predict whether each of the following compounds is soluble or insoluble in water: (a) MgBr2, (b) PbI2, (c) 1NH422CO3, (d) Sr1OH22, (e) ZnSO4.

Chapter: Problem: 4.22

Chemistry: The Central Science 13
Predict whether each of the following compounds is soluble in water: (a) AgI, (b) Na2CO3, (c) BaCl2, (d) Al1OH23, (e) Zn(CH3COO)2.

Chapter: Problem: 4.23

Chemistry: The Central Science 13
Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. (a) Na2CO3 and AgNO3, (b) NaNO3 and NiSO4, (c) FeSO4 and Pb1NO322.

Chapter: Problem: 4.24

Chemistry: The Central Science 13
Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. (a) NaCH3COO and HCl, (b) KOH and Cu1NO322, (c) Na2S and CdSO4.

Chapter: Problem: 4.25

Chemistry: The Central Science 13
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (a) potassium carbonate and magnesium sulfate (b) lead nitrate and lithium sulfide (c) ammonium phosphate and calcium chloride

Chapter: Problem: 4.26

Chemistry: The Central Science 13
Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. (a) Cr21SO4231aq2 + 1NH422CO31aq2 (b) Ba1NO3221aq2 + K2SO41aq2 (c) Fe1NO3221aq2 + KOH1aq2

Chapter: Problem: 4.27

Chemistry: The Central Science 13
Separate samples of a solution of an unknown salt are treated with dilute solutions of HBr, H2SO4, and NaOH. A precipitate forms in all three cases. Which of the following cations could be present in the unknown salt solution: K+, Pb2+, Ba 2+?

Chapter: Problem: 4.28

Chemistry: The Central Science 13
Separate samples of a solution of an unknown ionic compound are treated with dilute AgNO3, Pb1NO322, and BaCl2. Precipitates form in all three cases. Which of the following could be the anion of the unknown salt: Br -, CO32-, NO3-?

Chapter: Problem: 4.29

Chemistry: The Central Science 13
You know that an unlabeled bottle contains an aqueous solution of one of the following: AgNO3, CaCl2, or Al21SO423. A friend suggests that you test a portion of the solution with Ba1NO322 and then with NaCl solutions. According to your friends logic, which of these chemical reactions could occur, thu

Chapter: Problem: 4.30

Chemistry: The Central Science 13
Three solutions are mixed together to form a single solution; in the final solution, there are 0.2 mol Pb1CH3COO)2, 0.1 mol Na2S, and 0.1 mol CaCl2 present. What solid(s) will precipitate?

Chapter: Problem: 4.31

Chemistry: The Central Science 13
Which of the following solutions is the most acidic? (a) 0.2 M LiOH, (b) 0.2 M HI, (c) 1.0 M methyl alcohol 1CH3OH)

Chapter: Problem: 4.32

Chemistry: The Central Science 13
Which of the following solutions is the most basic? (a) 0.6 M NH3, (b) 0.150 M KOH, (c) 0.100 M Ba1OH22.

Chapter: Problem: 4.33

Chemistry: The Central Science 13
State whether each of the following statements is true or false. Justify your answer in each case. (a) Sulfuric acid is a monoprotic acid. (b) HCl is a weak acid. (c) Methanol is a base

Chapter: Problem: 4.34

Chemistry: The Central Science 13
State whether each of the following statements is true or false. Justify your answer in each case. (a) NH3 contains no OH- ions, and yet its aqueous solutions are basic. (b) HF is a strong acid. (c) Although sulfuric acid is a strong electrolyte, an aqueous solution of H2SO4 contains more HSO4 - ions

Chapter: Problem: 4.35

Chemistry: The Central Science 13
Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (a) HF, (b) acetonitrile, CH3CN, (c) NaClO4, (d) Ba1OH22.

Chapter: Problem: 4.36

Chemistry: The Central Science 13
An aqueous solution of an unknown solute is tested with litmus paper and found to be acidic. The solution is weakly conducting compared with a solution of NaCl of the same concentration. Which of the following substances could the unknown be: KOH, NH3, HNO3, KClO2, H3PO3, CH3COCH3 (acetone)?

Chapter: Problem: 4.37

Chemistry: The Central Science 13
Classify each of the following substances as a nonelectrolyte, weak electrolyte, or strong electrolyte in water: (a) H2SO3, (b) C2H5OH (ethanol), (c) NH3, (d) KClO3, (e) Cu1NO322.

Chapter: Problem: 4.38

Chemistry: The Central Science 13
Classify each of the following aqueous solutions as a nonelectrolyte, weak electrolyte, or strong electrolyte: (a) LiClO4, (b) HClO, (c) CH3CH2CH2OH (propanol), (d) HClO3, (e) CuSO4, (f) C12H22O11 (sucrose).

Chapter: Problem: 4.39

Chemistry: The Central Science 13
Complete and balance the following molecular equations, and then write the net ionic equation for each: (a) HBr1aq2 + Ca1OH221aq2 (b) Cu1OH221s2 + HClO41aq2 (c) Al1OH231s2 + HNO31aq2

Chapter: Problem: 4.40

Chemistry: The Central Science 13
Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (a) Aqueous acetic acid is neutralized by aqueous barium hydroxide. (b) Solid chromium(III) hydroxide reacts with nitrous acid. (c) Aqueous nitric acid and aqueous ammonia react

Chapter: Problem: 4.41

Chemistry: The Central Science 13
Write balanced molecular and net ionic equations for the following reactions, and identify the gas formed in each: (a) solid cadmium sulfide reacts with an aqueous solution of sulfuric acid; (b) solid magnesium carbonate reacts with an aqueous solution of perchloric acid.

Chapter: Problem: 4.42

Chemistry: The Central Science 13
Because the oxide ion is basic, metal oxides react readily with acids. (a) Write the net ionic equation for the following reaction: FeO1s2 + 2 HClO41aq2 Fe1ClO4221aq2 + H2O1l2 (b) Based on the equation in part (a), write the net ionic equation for the reaction that occurs between NiO(s) and an aqueou

Chapter: Problem: 4.43

Chemistry: The Central Science 13
Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions. (a) Write a balanced molecular equation and a net ionic equation for the reaction that occurs when each substance reacts with a hydrochloric acid solution. (b) By observing the reactio

Chapter: Problem: 4.44

Chemistry: The Central Science 13
As K2O dissolves in water, the oxide ion reacts with water molecules to form hydroxide ions. (a) Write the molecular and net ionic equations for this reaction. (b) Based on the definitions of acid and base, what ion is the base in this reaction? (c) What is the acid in the reaction? (d) What is the s

Chapter: Problem: 4.45

Chemistry: The Central Science 13
True or false: (a) If a substance is oxidized, it is gaining electrons. (b) If an ion is oxidized, its oxidation number increases.

Chapter: Problem: 4.46

Chemistry: The Central Science 13
True or false: (a) Oxidation can occur without oxygen. (b) Oxidation can occur without reduction

Chapter: Problem: 4.47a

Chemistry: The Central Science 13
(a) Which region of the periodic table shown here contains elements that are easiest to oxidize?

Chapter: Problem: 4.47b

Chemistry: The Central Science 13
(b) Which region contains the least readily oxidized elements?

Chapter: Problem: 4.48

Chemistry: The Central Science 13
Determine the oxidation number of sulfur in each of the following substances: (a) barium sulfate, BaSO4, (b) sulfurous acid, H2SO3, (c) strontium sulfide, SrS, (d) hydrogen sulfide, H2S. (e) Locate sulfur in the periodic table in Exercise 4.47; what region is it in? (f) Which region(s) of the period

Chapter: Problem: 4.49

Chemistry: The Central Science 13
Determine the oxidation number for the indicated element in each of the following substances: (a) S in SO2, (b) C in COCl2, (c) Mn in KMnO4, (d) Br in HBrO, (e) P in PF3, (f) O in K2O2.

Chapter: Problem: 4.50

Chemistry: The Central Science 13
Determine the oxidation number for the indicated element in each of the following compounds: (a) Co in LiCoO2, (b) Al in NaAlH4, (c) C in CH3OH (methanol), (d) N in GaN, (e) Cl in HClO2, (f) Cr in BaCrO4.

Chapter: Problem: 4.51

Chemistry: The Central Science 13
Which element is oxidized and which is reduced in the following reactions? (a) N21g2 + 3 H21g2 2 NH31g2 (b) 3 Fe1NO3221aq2 + 2 Al1s2 3 Fe1s2 + 2 Al1NO3231aq2 (c) Cl21aq2 + 2 NaI1aq2 I21aq2 + 2 NaCl1aq2 (d) PbS1s2 + 4 H2O21aq2 PbSO41s2 + 4 H2O1l2

Chapter: Problem: 4.52

Chemistry: The Central Science 13
Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or neutralization reactions. (a) P41s2 + 10 HClO1aq2 + 6 H2O1l2 4 H3PO41aq2 + 10 HCl1aq2 (b) Br21l) + 2 K1s2 2 KBr1s

Chapter: Problem: 4.53

Chemistry: The Central Science 13
Write balanced molecular and net ionic equations for the reactions of (a) manganese with dilute sulfuric acid, (b) chromium with hydrobromic acid, (c) tin with hydrochloric acid, (d) aluminum with formic acid, HCOOH.

Chapter: Problem: 4.54

Chemistry: The Central Science 13
Write balanced molecular and net ionic equations for the reactions of (a) hydrochloric acid with nickel, (b) dilute sulfuric acid with iron, (c) hydrobromic acid with magnesium, (d) acetic acid, CH3COOH, with zinc.

Chapter: Problem: 4.55

Chemistry: The Central Science 13
Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Iron metal is added to a solution of copper(II) nitrate, (b) zinc metal is added to a solution of magnesium sulfate, (c) hydrobromic acid is added to tin metal, (

Chapter: Problem: 4.56

Chemistry: The Central Science 13
Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Nickel metal is added to a solution of copper(II) nitrate, (b) a solution of zinc nitrate is added to a solution of magnesium sulfate, (c) hydrochloric acid is ad

Chapter: Problem: 4.57

Chemistry: The Central Science 13
The metal cadmium tends to form Cd2+ ions. The following observations are made: (i) When a strip of zinc metal is placed in CdCl21aq), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in Ni1NO3221aq), nickel metal is deposited on the strip. (a) Write net ionic equ

Chapter: Problem: 4.58

Chemistry: The Central Science 13
The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens: Br21aq2 + 2 NaI1aq2 2 NaBr1aq2 + I21aq2 Cl21aq2 + 2 NaBr1aq2 2 NaCl1aq2 + Br21aq2 (a) Which elemental halogen would you predict is the most stable, upon mixing wi

Chapter: Problem: 4.59a

Chemistry: The Central Science 13
(a) Is the concentration of a solution an intensive or an extensive property?

Chapter: Problem: 4.59b

Chemistry: The Central Science 13
(b) What is the difference between 0.50 mol HCl and 0.50 M HCl?

Chapter: Problem: 4.60

Chemistry: The Central Science 13
Your lab partner tells you that he has prepared a solution that contains 1.50 moles of NaOH in 1.50 L of aqueous solution, and therefore that the concentration of NaOH is 1.5 M. (a) Is he correct? (b) If not, what is the correct concentration?

Chapter: Problem: 4.61a

Chemistry: The Central Science 13
(a) Calculate the molarity of a solution that contains 0.175 mol ZnCl2 in exactly 150 mL of solution.

Chapter: Problem: 4.61b

Chemistry: The Central Science 13
(b) How many moles of protons are present in 35.0 mL of a 4.50 M solution of nitric acid? (c) How many milliliters of a 6.00 M NaOH solution are needed to provide 0.350 mol of NaOH?

Chapter: Problem: 4.62a

Chemistry: The Central Science 13
(a) Calculate the molarity of a solution made by dissolving 12.5 grams of Na2CrO4 in enough water to form exactly 750 mL of solution.

Chapter: Problem: 4.62b

Chemistry: The Central Science 13
(b) How many moles of KBr are present in 150 mL of a 0.112 M solution? (c) How many milliliters of 6.1 M HCl solution are needed to obtain 0.150 mol of HCl?

Chapter: Problem: 4.63

Chemistry: The Central Science 13
The average adult human male has a total blood volume of 5.0 L. If the concentration of sodium ion in this average individual is 0.135 M, what is the mass of sodium ion circulating in the blood?

Chapter: Problem: 4.64

Chemistry: The Central Science 13
A person suffering from hyponatremia has a sodium ion concentration in the blood of 0.118 M and a total blood volume of 4.6 L. What mass of sodium chloride would need to be added to the blood to bring the sodium ion concentration up to 0.138 M, assuming no change in blood volume?

Chapter: Problem: 4.65

Chemistry: The Central Science 13
The concentration of alcohol 1CH3CH2OH2 in blood, called the blood alcohol concentration or BAC, is given in units of grams of alcohol per 100 mL of blood. The legal definition of intoxication, in many states of the United States, is that the BAC is 0.08 or higher. What is the concentration of alcoho

Chapter: Problem: 4.66

Chemistry: The Central Science 13
The average adult male has a total blood volume of 5.0 L. After drinking a few beers, he has a BAC of 0.10 (see Exercise 4.65). What mass of alcohol is circulating in his blood?

Chapter: Problem: 4.67a

Chemistry: The Central Science 13
(a) How many grams of ethanol, CH3CH2OH, should you dissolve in water to make 1.00 L of vodka (which is an aqueous solution that is 6.86 M ethanol)?

Chapter: Problem: 4.67b

Chemistry: The Central Science 13
(b) Using the density of ethanol (0.789 g/mL), calculate the volume of ethanol you need to make 1.00 L of vodka

Chapter: Problem: 4.68

Chemistry: The Central Science 13
One cup of fresh orange juice contains 124 mg of ascorbic acid (vitamin C, C6H8O6). Given that one cup = 236.6 mL, calculate the molarity of vitamin C in organic juice

Chapter: Problem: 4.69a

Chemistry: The Central Science 13
(a) Which will have the highest concentration of potassium ion: 0.20 M KCl, 0.15 M K2CrO4, or 0.080 M K3PO4?

Chapter: Problem: 4.69b

Chemistry: The Central Science 13
(b) Which will contain the greater number of moles of potassium ion: 30.0 mL of 0.15 M K2CrO4 or 25.0 mL of 0.080 M K3PO4?

Chapter: Problem: 4.70

Chemistry: The Central Science 13
In each of the following pairs, indicate which has the higher concentration of I - ion: (a) 0.10 M BaI2 or 0.25 M KI solution, (b) 100 mL of 0.10 M KI solution or 200 mL of 0.040 M ZnI2 solution, (c) 3.2 M HI solution or a solution made by dissolving 145 g of NaI in water to make 150 mL of solution.

Chapter: Problem: 4.71

Chemistry: The Central Science 13
Indicate the concentration of each ion or molecule present in the following solutions: (a) 0.25 M NaNO3, ( b ) 1.3 * 10-2 M MgSO4, ( c ) 0.0150 M C6H12O6, (d) a mixture of 45.0 mL of 0.272 M NaCl and 65.0 mL of 0.0247 M 1NH422CO3. Assume that the volumes are additive.

Chapter: Problem: 4.72

Chemistry: The Central Science 13
Indicate the concentration of each ion present in the solution formed by mixing (a) 42.0 mL of 0.170 M NaOH with 37.6 mL of 0.400 M NaOH, (b) 44.0 mL of 0.100 M Na2SO4 with 25.0 mL of 0.150 M KCl, (c) 3.60 g KCl in 75.0 mL of 0.250 M CaCl2 solution. Assume that the volumes are additive.

Chapter: Problem: 4.73a

Chemistry: The Central Science 13
(a) You have a stock solution of 14.8 M NH3. How many milliliters of this solution should you dilute to make 1000.0 mL of 0.250 M NH3?

Chapter: Problem: 4.73b

Chemistry: The Central Science 13
(b) If you take a 10.0-mL portion of the stock solution and dilute it to a total volume of 0.500 L, what will be the concentration of the final solution?

Chapter: Problem: 4.74a

Chemistry: The Central Science 13
(a) How many milliliters of a stock solution of 6.0 M HNO3 would you have to use to prepare 110 mL of 0.500 M HNO3?

Chapter: Problem: 4.74b

Chemistry: The Central Science 13
(b) If you dilute 10.0 mL of the stock solution to a final volume of 0.250 L, what will be the concentration of the diluted solution?

Chapter: Problem: 4.75a

Chemistry: The Central Science 13
(a) Starting with solid sucrose, C12H22O11, describe how you would prepare 250 mL of a 0.250 M sucrose solution.

Chapter: Problem: 4.75b

Chemistry: The Central Science 13
(b) Describe how you would prepare 350.0 mL of 0.100 M C12H22O11 starting with 3.00 L of 1.50 M C12H22O11.

Chapter: Problem: 4.76a

Chemistry: The Central Science 13
(a) How many grams of solid silver nitrate would you need to prepare 200.0 mL of a 0.150 M AgNO3 solution?

Chapter: Problem: 4.76b

Chemistry: The Central Science 13
(b) An experiment calls for you to use 100 mL of 0.50 M HNO3 solution. All you have available is a bottle of 3.6 M HNO3. How many milliliters of the 3.6 M HNO3 solution and of water do you need to prepare the desired solution?

Chapter: Problem: 4.77

Chemistry: The Central Science 13
Pure acetic acid, known as glacial acetic acid, is a liquid with a density of 1.049 g>mL at 25 C. Calculate the molarity of a solution of acetic acid made by dissolving 20.00 mL of glacial acetic acid at 25 C in enough water to make 250.0 mL of solution.

Chapter: Problem: 4.78

Chemistry: The Central Science 13
Glycerol, C3H8O3, is a substance used extensively in the manufacture of cosmetics, foodstuffs, antifreeze, and plastics. Glycerol is a water-soluble liquid with a density of 1.2656 g>mL at 15 C. Calculate the molarity of a solution of glycerol made by dissolving 50.000 mL glycerol at 15 C in enough w

Chapter: Problem: 4.79

Chemistry: The Central Science 13
You want to analyze a silver nitrate solution. (a) You could add HCl(aq) to the solution to precipitate out AgCl(s). What volume of a 0.150 M HCl(aq) solution is needed to precipitate the silver ions from 15.0 mL of a 0.200 M AgNO3 solution? (b) You could add solid KCl to the solution to precipitate

Chapter: Problem: 4.80

Chemistry: The Central Science 13
You want to analyze a cadmium nitrate solution. What mass of NaOH is needed to precipitate the Cd2+ ions from 35.0 mL of 0.500 M Cd(NO322 solution?

Chapter: Problem: 4.81a

Chemistry: The Central Science 13
(a) What volume of 0.115 M HClO4 solution is needed to neutralize 50.00 mL of 0.0875 M NaOH?

Chapter: Problem: 4.81b

Chemistry: The Central Science 13
(b) What volume of 0.128 M HCl is needed to neutralize 2.87 g of Mg1OH22?

Chapter: Problem: 4.81c

Chemistry: The Central Science 13
(c) If 25.8 mL of an AgNO3 solution is needed to precipitate all the Cl - ions in a 785-mg sample of KCl (forming AgCl), what is the molarity of the AgNO3 solution?

Chapter: Problem: 4.81d

Chemistry: The Central Science 13
(d) If 45.3 mL of a 0.108 M HCl solution is needed to neutralize a solution of KOH, how many grams of KOH must be present in the solution?

Chapter: Problem: 4.82a

Chemistry: The Central Science 13
(a) How many milliliters of 0.120 M HCl are needed to completely neutralize 50.0 mL of 0.101 M Ba1OH22 solution?

Chapter: Problem: 4.82b

Chemistry: The Central Science 13
(b) How many milliliters of 0.125 M H2SO4 are needed to neutralize 0.200 g of NaOH?

Chapter: Problem: 4.82c

Chemistry: The Central Science 13
(c) If 55.8 mL of a BaCl2 solution is needed to precipitate all the sulfate ion in a 752-mg sample of Na2SO4, what is the molarity of the BaCl2 solution?

Chapter: Problem: 4.82d

Chemistry: The Central Science 13
(d) If 42.7 mL of 0.208 M HCl solution is needed to neutralize a solution of Ca1OH22, how many grams of Ca1OH22 must be in the solution?

Chapter: Problem: 4.83

Chemistry: The Central Science 13
Some sulfuric acid is spilled on a lab bench. You can neutralize the acid by sprinkling sodium bicarbonate on it and then mopping up the resultant solution. The sodium bicarbonate reacts with sulfuric acid according to: 2 NaHCO31s2 + H2SO41aq2 Na2SO41aq2 + 2 H2O1l2 + 2 CO21g2 Sodium bicarbonate is ad

Chapter: Problem: 4.84

Chemistry: The Central Science 13
The distinctive odor of vinegar is due to acetic acid, CH3COOH, which reacts with sodium hydroxide according to: CH3COO1aq2 + NaOH1aq2 H2O1l2 + NaCH3OO1aq2 If 3.45 mL of vinegar needs 42.5 mL of 0.115 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.00-qt

Chapter: Problem: 4.85

Chemistry: The Central Science 13
A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acidbase indicator is added and the resulting solution is titrated with 2.50 M HCl(aq) solution. The indicator changes color signaling that the equivalence point has been reached after 17.0 mL of the hydrochlor

Chapter: Problem: 4.86

Chemistry: The Central Science 13
An 8.65-g sample of an unknown group 2A metal hydroxide is dissolved in 85.0 mL of water. An acidbase indicator is added and the resulting solution is titrated with 2.50 M HCl(aq) solution. The indicator changes color signaling that the equivalence point has been reached after 56.9 mL of the hydrochl

Chapter: Problem: 4.87

Chemistry: The Central Science 13
A solution of 100.0 mL of 0.200 M KOH is mixed with a solution of 200.0 mL of 0.150 M NiSO4. (a) Write the balanced chemical equation for the reaction that occurs. (b) What precipitate forms? (c) What is the limiting reactant? (d) How many grams of this precipitate form? (e) What is the concentration

Chapter: Problem: 4.88

Chemistry: The Central Science 13
A solution is made by mixing 15.0 g of Sr1OH22 and 55.0 mL of 0.200 M HNO3. (a) Write a balanced equation for the reaction that occurs between the solutes. (b) Calculate the concentration of each ion remaining in solution. (c) Is the resultant solution acidic or basic?

Chapter: Problem: 4.89

Chemistry: The Central Science 13
A 0.5895-g sample of impure magnesium hydroxide is dissolved in 100.0 mL of 0.2050 M HCl solution. The excess acid then needs 19.85 mL of 0.1020 M NaOH for neutralization. Calculate the percentage by mass of magnesium hydroxide in the sample, assuming that it is the only substance reacting with the H

Chapter: Problem: 4.90

Chemistry: The Central Science 13
A 1.248-g sample of limestone rock is pulverized and then treated with 30.00 mL of 1.035 M HCl solution. The excess acid then requires 11.56 mL of 1.010 M NaOH for neutralization. Calculate the percentage by mass of calcium carbonate in the rock, assuming that it is the only substance reacting with t

Chapter: Problem: 4.91

Chemistry: The Central Science 13
Uranium hexafluoride, UF6, is processed to produce fuel for nuclear reactors and nuclear weapons. UF6 is made from the reaction of elemental uranium with ClF3, which also produces Cl2 as a by- product. (a) Write the balanced molecular equation for the conversion of U and ClF3 into UF6 and Cl2. (b) Is

Chapter: Problem: 4.92

Chemistry: The Central Science 13
The accompanying photo shows the reaction between a solution of Cd1NO322 and one of Na2S. (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?

Chapter: Problem: 4.93

Chemistry: The Central Science 13
Suppose you have a solution that might contain any or all of the following cations: Ni 2+, Ag+, Sr 2+, and Mn2+. Addition of HCl solution causes a precipitate to form. After filtering off the precipitate, H2SO4 solution is added to the resulting solution and another precipitate forms. This is filtere

Chapter: Problem: 4.94

Chemistry: The Central Science 13
You choose to investigate some of the solubility guidelines for two ions not listed in Table 4.1, the chromate ion 1CrO4 2-2 and the oxalate ion 1C2O4 2 - 2. You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: Solution Solute Color of Solution A Na2CrO4 Yellow B 1NH422C2O4 Colorl

Chapter: Problem: 4.95

Chemistry: The Central Science 13
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 HCl in the stomach and each of the following substances used in various antacids: (a) Al1OH231s2, (b) Mg1OH221s2, (c) MgCO31s2, (d) NaA

Chapter: Problem: 4.96

Chemistry: The Central Science 13
The commercial production of nitric acid involves the following chemical reactions: 4 NH31g2 + 5 O21g2 4 NO1g2 + 6 H2O1g2 2 NO1g2 + O21g2 2 NO21g2 3 NO21g2 + H2O1l2 2 HNO31aq2 + NO1g2 (a) Which of these reactions are redox reactions? (b) In each redox reaction identify the element undergoing oxidatio

Chapter: Problem: 4.97

Chemistry: The Central Science 13
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 ba

Chapter: Problem: 4.98

Chemistry: The Central Science 13
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

Chapter: Problem: 4.99

Chemistry: The Central Science 13
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?

Chapter: Problem: 4.100

Chemistry: The Central Science 13
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?

Chapter: Problem: 4.101

Chemistry: The Central Science 13
Hard water contains Ca 2+, Mg2+, and Fe 2+, 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 contain

Chapter: Problem: 4.102

Chemistry: The Central Science 13
Tartaric acid, H2C4H4O6, 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 M NaOH solution to titrate both acidic protons in 50.

Chapter: Problem: 4.103a

Chemistry: The Central Science 13
(a) A strontium hydroxide solution is prepared by dissolving 12.50 g of Sr1OH22 in water to make 50.00 mL of solution. What is the molarity of this solution?

Chapter: Problem: 4.103b

Chemistry: The Central Science 13
(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.

Chapter: Problem: 4.103c

Chemistry: The Central Science 13
(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?

Chapter: Problem: 4.104

Chemistry: The Central Science 13
A solid sample of Zn1OH22 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 M NaOH solution, and it takes 88.5 mL of the NaOH solution to reach the equivalence point. What mass of Zn1OH22 was added to the HBr solution?

Chapter: Problem: 4.105

Chemistry: The Central Science 13
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 solu

Chapter: Problem: 4.106a

Chemistry: The Central Science 13
(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?

Chapter: Problem: 4.106b

Chemistry: The Central Science 13
(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?

Chapter: Problem: 4.107

Chemistry: The Central Science 13
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 o

Chapter: Problem: 4.108

Chemistry: The Central Science 13
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(OH21COOH21CH2COOH22, (which contains three acidic protons) is required to neutralize the

Chapter: Problem: 4.109

Chemistry: The Central Science 13
A sample of 7.75 g of Mg1OH22 is added to 25.0 mL of 0.200 M HNO3. (a) Write the chemical equation for the reaction that occurs. (b) Which is the limiting reactant in the reaction? (c) How many moles of Mg1OH22, HNO3, and Mg1NO322 are present after the reaction is complete?

Chapter: Problem: 4.110

Chemistry: The Central Science 13
Lead glass contains 1840% 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 o

Chapter: Problem: 4.111

Chemistry: The Central Science 13
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 go

Chapter: Problem: 4.112

Chemistry: The Central Science 13
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

Chapter: Problem: 4.113

Chemistry: The Central Science 13
The arsenic in a 1.22-g sample of a pesticide was converted to AsO4 3- by suitable chemical treatment. It was then titrated using Ag+ to form Ag3AsO4 as a precipitate. (a) What is the oxidation state of As in AsO4 3-? (b) Name Ag3AsO4 by analogy to the corresponding compound containing phosphorus in

Chapter: Problem: 4.114

Chemistry: The Central Science 13
The U.S. 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, AsO4 3-, what mass of sodium arsenate would be present in a 1.00-L sample of drinking water that just meets the

Chapter: Problem: 4.115

Chemistry: The Central Science 13
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 NH31g2 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 HCl. The NH3 reac

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