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Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro
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Chapter 4 Problems

Chapter: 4 Problem: 2SAQ

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 4.164

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 2E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 4.138

Chemistry: A Molecular Approach 3
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 magne

Chapter: 4 Problem: 3E

Chemistry: A Molecular Approach 3
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)?

Chapter: 4 Problem: 3SAQ

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 4.45

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 4.68

Chemistry: A Molecular Approach 3
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).

Chapter: 4 Problem: 4E

Chemistry: A Molecular Approach 3
Problem 4E What is an aqueous solution? What is the difference between the solute and the solvent?

Chapter: 4 Problem: 4.91

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 4SAQ

Chemistry: A Molecular Approach 3
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%

Chapter: 4 Problem: 4.115

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 5E

Chemistry: A Molecular Approach 3
Problem 5E What is molarity? How is it useful?

Chapter: 4 Problem: 5SAQ

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 6E

Chemistry: A Molecular Approach 3
Problem 6E Explain how a strong electrolyte, a weak electrolyte, and a nonelectrolyte differ.

Chapter: 4 Problem: 4.22

Chemistry: A Molecular Approach 3
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)

Chapter: 4 Problem: 4.165

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 6SAQ

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 7SAQ

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 7E

Chemistry: A Molecular Approach 3
Problem 7E Explain the difference between a strong acid and a weak acid.

Chapter: 4 Problem: 4.139

Chemistry: A Molecular Approach 3
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 pa

Chapter: 4 Problem: 8E

Chemistry: A Molecular Approach 3
Problem 8E What does it mean for a compound to be soluble? Insoluble?

Chapter: 4 Problem: 8SAQ

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 4.116

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 9E

Chemistry: A Molecular Approach 3
Problem 9E What are the solubility rules? How are they useful?

Chapter: 4 Problem: 4.92

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 9SAQ

Chemistry: A Molecular Approach 3
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) \(\mathrm{CuCl}_{2}(a q)\)

Chapter: 4 Problem: 4.69

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 4.166

Chemistry: A Molecular Approach 3
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 t

Chapter: 4 Problem: 10E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 4.46

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 11E

Chemistry: A Molecular Approach 3
Problem 11E What is a precipitation reaction? Give an example.

Chapter: 4 Problem: 10SAQ

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 11SAQ

Chemistry: A Molecular Approach 3
What is the net ionic equation for the reaction that occurs when aqueous solutions of KOH and HNO3 are mixed?

Chapter: 4 Problem: 12E

Chemistry: A Molecular Approach 3
Problem 12E How can you predict whether a precipitation reaction will occur upon mixing two aqueous solutions?

Chapter: 4 Problem: 4.14

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 12SAQ

Chemistry: A Molecular Approach 3
What is the net ionic equation for the reaction that occurs when aqueous solutions of KHCO3 and HBr are mixed?

Chapter: 4 Problem: 13E

Chemistry: A Molecular Approach 3
Problem 13E Explain how a molecular equation, a complete ionic equation, and a net ionic equation differ.

Chapter: 4 Problem: 4.23

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 13SAQ

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

Chapter: 4 Problem: 14E

Chemistry: A Molecular Approach 3
Problem 14E What is the Arrhenius definition of an acid? A base?

Chapter: 4 Problem: 4.47

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 4.117

Chemistry: A Molecular Approach 3
(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 stom

Chapter: 4 Problem: 14SAQ

Chemistry: A Molecular Approach 3
Sodium reacts with water according to the reaction: Identify the oxidizing agent. a) Na(s) b) H2O(l) c) NaOH(aq) d) H2(aq)

Chapter: 4 Problem: 4.93

Chemistry: A Molecular Approach 3
What are the similarities and differences between acid-base titrations and redox titrations?

Chapter: 4 Problem: 4.167

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 15E

Chemistry: A Molecular Approach 3
Problem 15E What is an acidbase reaction? Give an example.

Chapter: 4 Problem: 15SAQ

Chemistry: A Molecular Approach 3
Identify the correct balanced equation for the combustion of propane (C3H8).

Chapter: 4 Problem: 16E

Chemistry: A Molecular Approach 3
Problem 16E Explain the principles behind an acidbase titration. What is an indicator?

Chapter: 4 Problem: 17E

Chemistry: A Molecular Approach 3
Problem 17E What is a gas-evolution reaction? Give an example.

Chapter: 4 Problem: 4.141

Chemistry: A Molecular Approach 3
Based on oxidation number consideration, explain why carbon monoxide (CO) is flammable but carbon dioxide (CO2) is not

Chapter: 4 Problem: 18E

Chemistry: A Molecular Approach 3
Problem 18E What reactant types give rise to gas-evolution reactions?

Chapter: 4 Problem: 4.24

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 19E

Chemistry: A Molecular Approach 3
Problem 19E What is an oxidationreduction reaction? Give an example.

Chapter: 4 Problem: 20E

Chemistry: A Molecular Approach 3
Problem 20E What are oxidation states?

Chapter: 4 Problem: 4.7

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 21E

Chemistry: A Molecular Approach 3
Problem 21E How can oxidation states be used to identify redox reactions?

Chapter: 4 Problem: 22E

Chemistry: A Molecular Approach 3
Problem 22E In a redox reaction, which reactant is the oxidizing agent? The reducing agent?

Chapter: 4 Problem: 4.48

Chemistry: A Molecular Approach 3
Give the oxidation number for the following species: H2, Se8, P4, O, U, As4, B12.

Chapter: 4 Problem: 23E

Chemistry: A Molecular Approach 3

Chapter: 4 Problem: 4.118

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 24E

Chemistry: A Molecular Approach 3
Problem 24E What is a combustion reaction? Why are they important? Give an example.

Chapter: 4 Problem: 4.168

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 25E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 26E

Chemistry: A Molecular Approach 3
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 e

Chapter: 4 Problem: 4.25

Chemistry: A Molecular Approach 3
List the general properties of acids and bases

Chapter: 4 Problem: 4.94

Chemistry: A Molecular Approach 3
Explain why potassium permanganate (KMnO4) and potassium dichromate (K2Cr2O7) can serve as internal indicators in redox titrations.

Chapter: 4 Problem: 27E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 4.142

Chemistry: A Molecular Approach 3
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)

Chapter: 4 Problem: 28E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 29E

Chemistry: A Molecular Approach 3
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 p

Chapter: 4 Problem: 4.71

Chemistry: A Molecular Approach 3
Describe the basic steps involved in diluting a solution of known concentration.

Chapter: 4 Problem: 30E

Chemistry: A Molecular Approach 3
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 pr

Chapter: 4 Problem: 31E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 32E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 33E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 34E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 4.119

Chemistry: A Molecular Approach 3
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(

Chapter: 4 Problem: 35E

Chemistry: A Molecular Approach 3
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) ? 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)

Chapter: 4 Problem: 4.169

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 36E

Chemistry: A Molecular Approach 3
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(

Chapter: 4 Problem: 4.49

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 4.95

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 4.143

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 37E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 38E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 39E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 4.72

Chemistry: A Molecular Approach 3
Write the equation that enables us to calculate the concentration of a diluted solution. Give units for all the terms.

Chapter: 4 Problem: 40E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 41E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 42E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 43E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 4.26

Chemistry: A Molecular Approach 3
Give Arrhenius and Brnsteds definitions of an acid and a base. Why are Brnsteds definitions more useful in describing acid-base properties?

Chapter: 4 Problem: 44E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 45E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 46E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 4.5

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 4.144

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 91E

Chemistry: A Molecular Approach 3
Assign oxidation states to each atom in each element, ion, or compound. a. Ag b. Ag+ c. CaF2 d. H2S e. CO32- f. CrO42-

Chapter: 4 Problem: 92E

Chemistry: A Molecular Approach 3
Assign oxidation states to each atom in each element, ion, or compound. a. Cl2 b. Fe3+ c. CuCl2 d. CH4 e. Cr2O72- f. HSO4 -

Chapter: 4 Problem: 4.73

Chemistry: A Molecular Approach 3
Describe how to prepare 1.00 L of 0.646 M HCl solution, starting with a 2.00 M HCl solution.

Chapter: 4 Problem: 4.96

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 93E

Chemistry: A Molecular Approach 3
What is the oxidation state of Cr in each compound? a. CrO b. CrO3 c. Cr2O3

Chapter: 4 Problem: 94E

Chemistry: A Molecular Approach 3
What is the oxidation state of Cl in each ion? a. ClO- b. ClO2- c. ClO3- d. ClO4-

Chapter: 4 Problem: 4.17

Chemistry: A Molecular Approach 3
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 ne

Chapter: 4 Problem: 95E

Chemistry: A Molecular Approach 3
Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent.

Chapter: 4 Problem: 4.27

Chemistry: A Molecular Approach 3
Give an example of a monoprotic acid, a diprotic acid, and a triprotic acid.

Chapter: 4 Problem: 4.145

Chemistry: A Molecular Approach 3
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 neutrali

Chapter: 4 Problem: 96E

Chemistry: A Molecular Approach 3
Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent.

Chapter: 4 Problem: 4.12

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 97E

Chemistry: A Molecular Approach 3
Complete and balance each combustion reaction equation.

Chapter: 4 Problem: 98E

Chemistry: A Molecular Approach 3
Complete and balance each combustion reaction equation:

Chapter: 4 Problem: 99E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 101E

Chemistry: A Molecular Approach 3
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 bicarb

Chapter: 4 Problem: 53E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 100E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 4.171

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 54E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 102E

Chemistry: A Molecular Approach 3
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 hydrochlori

Chapter: 4 Problem: 4.51

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 55E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 103E

Chemistry: A Molecular Approach 3
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.)

Chapter: 4 Problem: 4.97

Chemistry: A Molecular Approach 3
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 t

Chapter: 4 Problem: 56E

Chemistry: A Molecular Approach 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

Chapter: 4 Problem: 104E

Chemistry: A Molecular Approach 3
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 bal

Chapter: 4 Problem: 4.74

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 4.121

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 57E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 105E

Chemistry: A Molecular Approach 3
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 sal

Chapter: 4 Problem: 58E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 106E

Chemistry: A Molecular Approach 3
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 ,

Chapter: 4 Problem: 4.146

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 59E

Chemistry: A Molecular Approach 3
A laboratory procedure calls for making 400.0 mL of a 1.1 M NaNO3 solution. What mass of NaNO3 (in g) is needed?

Chapter: 4 Problem: 107E

Chemistry: A Molecular Approach 3
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 hyd

Chapter: 4 Problem: 60E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 108E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 61E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 109E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 4.172

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 62E

Chemistry: A Molecular Approach 3
If 3.5 L of a 4.8 M SrCl2 solution is diluted to 45 L, what is the molarity of the diluted solution?

Chapter: 4 Problem: 111E

Chemistry: A Molecular Approach 3
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 s

Chapter: 4 Problem: 63E

Chemistry: A Molecular Approach 3
To what volume should you dilute 50.0 mL of a 12 M stock HNO3 solution to obtain a 0.100 M HNO3 solution?

Chapter: 4 Problem: 110E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 4.28

Chemistry: A Molecular Approach 3
What are the characteristics of an acid-base neutralization reaction?

Chapter: 4 Problem: 4.98

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 64E

Chemistry: A Molecular Approach 3
To what volume should you dilute 25 mL of a 10.0 M H2SO4 solution to obtain a 0.150 M H2SO4 solution?

Chapter: 4 Problem: 112E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 4.52

Chemistry: A Molecular Approach 3
Which of the following metals can react with water? (a) Au, (b) Li, (c) Hg, (d) Ca, (e) Pt

Chapter: 4 Problem: 4.75

Chemistry: A Molecular Approach 3
How would you prepare 60.0 mL of 0.200 M HNO3 from a stock solution of 4.00 M HNO3?

Chapter: 4 Problem: 66E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 113E

Chemistry: A Molecular Approach 3
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-.

Chapter: 4 Problem: 67E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 114E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 68E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 115E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 69E

Chemistry: A Molecular Approach 3
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 perc

Chapter: 4 Problem: 116E

Chemistry: A Molecular Approach 3
Find the volume of \(0.110 \mathrm{M}\) hydrochloric acid necessary to react completely with \(1.52 \mathrm{~g} \mathrm{Al}(\mathrm{OH})_3\).

Chapter: 4 Problem: 70E

Chemistry: A Molecular Approach 3
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 pe

Chapter: 4 Problem: 117E

Chemistry: A Molecular Approach 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.

Chapter: 4 Problem: 4.29

Chemistry: A Molecular Approach 3
What factors qualify a compound as a salt? Specify which of the following compounds are salts: CH4, NaF, NaOH, CaO, BaSO4, HNO3, NH3, KBr?

Chapter: 4 Problem: 4.122

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 71E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 118E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 72E

Chemistry: A Molecular Approach 3
Classify each compound as a strong electrolyte or nonelectrolyte. a. MgBr2 b. C12H22O11 c. Na2CO3 d. KOH

Chapter: 4 Problem: 119E

Chemistry: A Molecular Approach 3
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, pr

Chapter: 4 Problem: 73E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 120E

Chemistry: A Molecular Approach 3
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 t

Chapter: 4 Problem: 74E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 121E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 4.99

Chemistry: A Molecular Approach 3
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 8H2

Chapter: 4 Problem: 75E

Chemistry: A Molecular Approach 3
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) ?

Chapter: 4 Problem: 123E

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 4.147

Chemistry: A Molecular Approach 3
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 reac

Chapter: 4 Problem: 4.173

Chemistry: A Molecular Approach 3
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 Chemist

Chapter: 4 Problem: 76E

Chemistry: A Molecular Approach 3
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) ?

Chapter: 4 Problem: 122E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 77E

Chemistry: A Molecular Approach 3
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 magnesiu

Chapter: 4 Problem: 124E

Chemistry: A Molecular Approach 3
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 ilmenitesand mixture contains 22.

Chapter: 4 Problem: 10

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 78E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 125E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 11

Chemistry: A Molecular Approach 3
What is a precipitation reaction? Give an example.

Chapter: 4 Problem: 79E

Chemistry: A Molecular Approach 3
Write balanced complete ionic and net ionic equations for each reaction.

Chapter: 4 Problem: 126E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 12

Chemistry: A Molecular Approach 3
How can you predict whether a precipitation reaction will occur upon mixing two aqueous solutions?

Chapter: 4 Problem: 80E

Chemistry: A Molecular Approach 3
Write balanced complete ionic and net ionic equations for each reaction.

Chapter: 4 Problem: 127E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 4.3

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 13

Chemistry: A Molecular Approach 3
Explain how a molecular equation, a complete ionic equation, and a net ionic equation differ

Chapter: 4 Problem: 81E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 128E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 4.53

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 4.148

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 4.174

Chemistry: A Molecular Approach 3
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 unit

Chapter: 4 Problem: 14

Chemistry: A Molecular Approach 3
What is the Arrhenius definition of an acid? A base?

Chapter: 4 Problem: 82E

Chemistry: A Molecular Approach 3
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 a

Chapter: 4 Problem: 129E

Chemistry: A Molecular Approach 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 capaci

Chapter: 4 Problem: 4.76

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 15

Chemistry: A Molecular Approach 3
What is an acidbase reaction? Give an example. 16. Explain the principles behind an acidbase titration.

Chapter: 4 Problem: 83E

Chemistry: A Molecular Approach 3
Problem 83E Write balanced molecular and net ionic equations for the reaction between hydrobromic acid and potassium hydroxide.

Chapter: 4 Problem: 130E

Chemistry: A Molecular Approach 3
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 chelatin

Chapter: 4 Problem: 4.123

Chemistry: A Molecular Approach 3
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?

Chapter: 4 Problem: 16

Chemistry: A Molecular Approach 3
Explain the principles behind an acidbase titration. What is an indicator?

Chapter: 4 Problem: 84E

Chemistry: A Molecular Approach 3
Problem 84E Write balanced molecular and net ionic equations for the reaction between nitric acid and calcium hydroxide.

Chapter: 4 Problem: 131E

Chemistry: A Molecular Approach 3
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: Notice that the reaction produces O2, which can be breathed, and absorbs CO2

Chapter: 4 Problem: 17

Chemistry: A Molecular Approach 3
What is a gas-evolution reaction? Give an example.

Chapter: 4 Problem: 90E

Chemistry: A Molecular Approach 3
Complete and balance each gas-evolution equation.

Chapter: 4 Problem: 132E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 18

Chemistry: A Molecular Approach 3
What reactant types give rise to gas-evolution reactions?

Chapter: 4 Problem: 91AE

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 133E

Chemistry: A Molecular Approach 3
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.

Chapter: 4 Problem: 19

Chemistry: A Molecular Approach 3
What is an oxidationreduction reaction? Give an example.

Chapter: 4 Problem: 92

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 134E

Chemistry: A Molecular Approach 3
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

Chapter: 4 Problem: 4.1

Chemistry: A Molecular Approach 3
A 15.0-mL sample of an oxalic acid solution requires 25.2 mL of 0.149 M NaOH for neutralization. Calcul