Question 1

The addition of hydrochloric acid and ________ to water produces a buffer solution.

Accepted Answer

A) HC6H5O 
B) NaOH 
C) NaCl 
D) C2H5NH2 
E) none of the above 
A) HC6H5O 
B) NaOH 
C) NaCl 
D) C2H5NH2 
E) none of the above

Question 2

Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.010 moles of acetic acid in 100 ml of water. The Ka of acetic acid is 1.77 × 10-5.

Accepted Answer

Question 3

In which aqueous system is CaF2 least soluble?

Accepted Answer

A) H2O 
B) 0.5 M HF 
C) 0.2 M HF 
D) 1.0 M HNO3 
E) 0.8 M KF 
A) H2O 
B) 0.5 M HF 
C) 0.2 M HF 
D) 1.0 M HNO3 
E) 0.8 M KF

Question 4

What is the molar solubility of silver carbonate (Ag2CO3)in water? The solubility-product constant for Ag2CO3 is 8.1 × 10-12 at 25 °C.

Accepted Answer

A) 1.4 × 10-6 
B) 2.0 × 10-4 
C) 4.0 × 10-6 
D) 1.3 × 10-4 
E) 2.7 × 10-12 
A) 1.4 × 10-6 
B) 2.0 × 10-4 
C) 4.0 × 10-6 
D) 1.3 × 10-4 
E) 2.7 × 10-12

Question 5

Human blood is ________.

Accepted Answer

A) neutral 
B) very basic 
C) slightly acidic 
D) very acidic 
E) slightly basic 
A) neutral 
B) very basic 
C) slightly acidic 
D) very acidic 
E) slightly basic

Question 6

The solubility of lead (II)chloride (PbCl2)is 1.6 × 10-2 M. What is the Ksp of PbCl2?

Accepted Answer

A) 5.0 × 10-4 
B) 4.1 × 10-6 
C) 3.1 × 10-7 
D) 1.6 × 10-5 
E) 1.6 × 10-2 
A) 5.0 × 10-4 
B) 4.1 × 10-6 
C) 3.1 × 10-7 
D) 1.6 × 10-5 
E) 1.6 × 10-2

Question 7

Calculate the pH of a solution prepared by dissolving 0.270 mol of formic acid (HCO2H)and 0.260 mol of sodium formate (NaCO2H)in water sufficient to yield 1.00 L of solution. The Ka of formic acid is 1.77 × 10-4.

Accepted Answer

A) 2.099 
B) 10.264 
C) 3.736 
D) 2.307 
E) 3.952 
A) 2.099 
B) 10.264 
C) 3.736 
D) 2.307 
E) 3.952

Question 8

Calculate the percent ionization of formic acid (HCO2H)in a solution that is 0.152 M in formic acid. The Ka of formic acid is 1.77 × 10-4.

Accepted Answer

A) 2.74 × 10-5 
B) 0.0180 
C) 3.44 
D) 0.581 
E) 8.44 
A) 2.74 × 10-5 
B) 0.0180 
C) 3.44 
D) 0.581 
E) 8.44

Question 9

Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10-5.

Accepted Answer

Question 10

-A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The concentration of the monoprotic acid is about ________ mol/L.

Accepted Answer

A) 25.0 
B) 0.0600 
C) 0.240 
D) 0.120 
E) 0.100 
A) 25.0 
B) 0.0600 
C) 0.240 
D) 0.120 
E) 0.100

Question 11

What is the pH of a buffer solution that is 0.172 M in hypochlorous acid (HClO)and 0.131 M in sodium hypochlorite? The Ka of hypochlorous acid is 3.8 × 10-8.

Accepted Answer

A) 14.12 
B) 6.70 
C) 9.07 
D) 7.54 
E) 7.30 
A) 14.12 
B) 6.70 
C) 9.07 
D) 7.54 
E) 7.30

Question 12

Which one of the following is not amphoteric?

Accepted Answer

A) Al(OH)3 
B) Ca(OH)2 
C) Cr(OH)3 
D) Zn(OH)2 
E) Sn(OH)2 
A) Al(OH)3 
B) Ca(OH)2 
C) Cr(OH)3 
D) Zn(OH)2 
E) Sn(OH)2

Question 13

Which of the following could be added to a solution of potassium fluoride to prepare a buffer?

Accepted Answer

A) sodium hydroxide 
B) potassium acetate 
C) hydrochloric acid 
D) sodium fluoride 
E) ammonia 
A) sodium hydroxide 
B) potassium acetate 
C) hydrochloric acid 
D) sodium fluoride 
E) ammonia

Question 14

The pH of a solution prepared by mixing 50.0 mL of 0.125 M KOH and 50.0 mL of 0.125 M HCl is ________.

Accepted Answer

A) 6.29 
B) 7.00 
C) 8.11 
D) 5.78 
E) 0.00 
A) 6.29 
B) 7.00 
C) 8.11 
D) 5.78 
E) 0.00

Question 15

A solution of NaF is added dropwise to a solution that is 0.0122 M in Ba2+. When the concentration of F- exceeds ________ M, BaF2 will precipitate. Neglect volume changes. For BaF, Ksp = 1.7 × 10-6.

Accepted Answer

A) 7.0 × 10-5 
B) 1.2 × 10-2 
C) 2.1 × 10-8 
D) 3.0 × 10-3  
E) 1.4 × 10-4 
A) 7.0 × 10-5 
B) 1.2 × 10-2 
C) 2.1 × 10-8 
D) 3.0 × 10-3  
E) 1.4 × 10-4

Question 16

A buffer solution with a pH of 4.31 is prepared with 1.0 M HC2H3O2 and ________ M NaC2H3O2. The Ka of HC2H3O2 is 1.8 × 10-5.

Accepted Answer

A) 0.37 
B) 0.74 
C) 4.2 × 10-6 
D) 8.8 × 10-10 
E) 0.18 
A) 0.37 
B) 0.74 
C) 4.2 × 10-6 
D) 8.8 × 10-10 
E) 0.18

Question 17

In which of the following aqueous solutions would you expect AgF to have the highest solubility?

Accepted Answer

A) 0.00750 M LiF 
B) 0.030 M AgNO3 
C) 0.023 M NaF 
D) 0.015 M KF 
E) AgF will have the same solubility in all solutions. 
A) 0.00750 M LiF 
B) 0.030 M AgNO3 
C) 0.023 M NaF 
D) 0.015 M KF 
E) AgF will have the same solubility in all solutions.

Question 18

A 50.0 mL sample of an aqueous H2SO4 solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H2SO4 is ________ M.

Accepted Answer

A) 0.234 
B) 0.469 
C) 0.150 
D) 0.300 
E) 0.938 
A) 0.234 
B) 0.469 
C) 0.150 
D) 0.300 
E) 0.938

Question 19

Which below best describe(s)the behavior of an amphoteric hydroxide in water?

Accepted Answer

A) With conc. aq. NaOH, its suspension dissolves. 
B) With conc. aq. HCl, its suspension dissolves. 
C) With conc. aq. NaOH, its clear solution forms a precipitate. 
D) With conc. aq. HCl, its clear solution forms a precipitate. 
E) With both conc. aq. NaOH and conc. aq. HCl, its suspension dissolves. 
A) With conc. aq. NaOH, its suspension dissolves. 
B) With conc. aq. HCl, its suspension dissolves. 
C) With conc. aq. NaOH, its clear solution forms a precipitate. 
D) With conc. aq. HCl, its clear solution forms a precipitate. 
E) With both conc. aq. NaOH and conc. aq. HCl, its suspension dissolves.

Question 20

A result of the common-ion effect is ________.

Accepted Answer

A) that some ions, such as Na+ (aq), frequently appear in solutions but do not participate in solubility equilibria 
B) that common ions, such as Na+ (aq), don't affect equilibrium constants 
C) that the selective precipitation of a metal ion, such as Ag+, is promoted by the addition of an appropriate counterion (X-)that produces a compound (AgX)with a very low solubility 
D)  that ions such as K+ and Na+ are common ions, so that their values in equilibrium constant expressions are always 1.00 
E) that common ions precipitate all counter-ions 
A) that some ions, such as Na+ (aq), frequently appear in solutions but do not participate in solubility equilibria 
B) that common ions, such as Na+ (aq), don't affect equilibrium constants 
C) that the selective precipitation of a metal ion, such as Ag+, is promoted by the addition of an appropriate counterion (X-)that produces a compound (AgX)with a very low solubility 
D)  that ions such as K+ and Na+ are common ions, so that their values in equilibrium constant expressions are always 1.00 
E) that common ions precipitate all counter-ions

Exam 17: Additional Aspects of Aqueous Equilibria

The addition of hydrochloric acid and ________ to water produces a buffer solution.

Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.010 moles of acetic acid in 100 ml of water. The Ka of acetic acid is 1.77 × 10-5.

In which aqueous system is CaF2 least soluble?

What is the molar solubility of silver carbonate (Ag2CO3)in water? The solubility-product constant for Ag2CO3 is 8.1 × 10-12 at 25 °C.

Human blood is ________.

The solubility of lead (II)chloride (PbCl2)is 1.6 × 10-2 M. What is the Ksp of PbCl2?

Calculate the pH of a solution prepared by dissolving 0.270 mol of formic acid (HCO2H)and 0.260 mol of sodium formate (NaCO2H)in water sufficient to yield 1.00 L of solution. The Ka of formic acid is 1.77 × 10-4.

Calculate the percent ionization of formic acid (HCO2H)in a solution that is 0.152 M in formic acid. The Ka of formic acid is 1.77 × 10-4.

Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10-5.

-A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The concentration of the monoprotic acid is about ________ mol/L.

What is the pH of a buffer solution that is 0.172 M in hypochlorous acid (HClO)and 0.131 M in sodium hypochlorite? The Ka of hypochlorous acid is 3.8 × 10-8.

Which one of the following is not amphoteric?

Which of the following could be added to a solution of potassium fluoride to prepare a buffer?

The pH of a solution prepared by mixing 50.0 mL of 0.125 M KOH and 50.0 mL of 0.125 M HCl is ________.

A solution of NaF is added dropwise to a solution that is 0.0122 M in Ba2+. When the concentration of F- exceeds ________ M, BaF2 will precipitate. Neglect volume changes. For BaF, Ksp = 1.7 × 10-6.

A buffer solution with a pH of 4.31 is prepared with 1.0 M HC2H3O2 and ________ M NaC2H3O2. The Ka of HC2H3O2 is 1.8 × 10-5.

In which of the following aqueous solutions would you expect AgF to have the highest solubility?

A 50.0 mL sample of an aqueous H2SO4 solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H2SO4 is ________ M.

Which below best describe(s)the behavior of an amphoteric hydroxide in water?

A result of the common-ion effect is ________.

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Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.010 moles of acetic acid in 100 ml of water. The K_a of acetic acid is 1.77 × 10^-5.

In which aqueous system is CaF₂ least soluble?

What is the molar solubility of silver carbonate (Ag₂CO₃)in water? The solubility-product constant for Ag₂CO₃ is 8.1 × 10^-12 at 25 °C.

The solubility of lead (II)chloride (PbCl₂)is 1.6 × 10^-2M. What is the K_sp of PbCl₂?

Calculate the pH of a solution prepared by dissolving 0.270 mol of formic acid (HCO₂H)and 0.260 mol of sodium formate (NaCO₂H)in water sufficient to yield 1.00 L of solution. The K_a of formic acid is 1.77 × 10^-4.

Calculate the percent ionization of formic acid (HCO₂H)in a solution that is 0.152 M in formic acid. The K_a of formic acid is 1.77 × 10^-4.

Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

What is the pH of a buffer solution that is 0.172 M in hypochlorous acid (HClO)and 0.131 M in sodium hypochlorite? The K_a of hypochlorous acid is 3.8 × 10^-⁸.

A solution of NaF is added dropwise to a solution that is 0.0122 M in Ba²⁺. When the concentration of F^- exceeds ________ M, BaF₂ will precipitate. Neglect volume changes. For BaF, Ksp = 1.7 × 10^-⁶.

A buffer solution with a pH of 4.31 is prepared with 1.0 M HC₂H₃O₂ and ________ M NaC₂H₃O₂. The Ka of HC₂H₃O₂is 1.8 × 10^-⁵.

A 50.0 mL sample of an aqueous H₂SO₄ solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H₂SO₄ is ________ M.