Question 1

Write an equation showing the net reaction that occurs when a strong base is added to a CO32-/HCO3- buffer solution (for carbonic acid, Ka1 = 4.2 × 10-7, Ka2 = 2.4 × 10-8):

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Question 2

Calculate the pH at the equivalence point for the titration of 0.22 M HCN with 0.22 M NaOH.(Ka = 4.9 × 10-10 for HCN)

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Question 3

A saturated sodium carbonate solution at 0°C contains 7.1 g of dissolved sodium carbonate per 100.mL of solution.The solubility product constant for sodium carbonate at this temperature is

Accepted Answer

A)  1.2
B)  0.30
C)  3.0 × 10-4
D)  0.90
E)  1.2 × 10-3F) B) and C)
G) D) and E)

Question 4

The Ksp of CaF2 is 4 × 10-11.What is the maximum concentration of Ca2+ possible in a 0.10 M NaF solution?

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Question 5

Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 × 10-10) solution.

Accepted Answer

A)  5.15
B)  8.71
C)  5.85
D)  9.91
E)  13.0F) C) and D)
G) B) and E)

Question 6

An environmental chemist obtained a 200.mL sample of lake water believed to be contaminated with a single monoprotic strong acid.Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint.What is the pH of the lake?

Accepted Answer

The answer of An environmental chemist obtained a 200.mL sample...

Question 7

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C6H5COOH) is added 1.00 mL of 12.0 M HCl.What is the percentage ionization of the benzoic acid in the resulting solution? [Ka(C6H5COOH) = 6.5 × 10-5]

Accepted Answer

A)  3.3%
B)  12%
C)  1.3%
D)  0.52%
E)  0.065%F) C) and D)
G) A) and E)

Question 8

Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa and compare your answer to the percent ionization you would calculate if the sodium formate were not present.Explain the difference, if any.(Ka = 1.7 × 10-4)

Accepted Answer

3.4%; the addition of formate ...

Question 9

Consider a buffer solution prepared from HOCl and NaOCl.Which is the net ionic equation for the reaction that occurs when NaOH is added to this buffer?

Accepted Answer

A)  OH- + HOCl  →\rarr→  H2O + OCl-
B)  OH- + OCl-  →\rarr→  HOCl + O2-
C)  Na+ + HOCl  →\rarr→ NaCl + OH-
D)  H+ + HOCl  →\rarr→  H2 + OCl-
E)  NaOH + HOCl  →\rarr→ H2O + NaCl F) B) and C)
G) A) and D)

Question 10

Will a precipitate of AgCl form when 0.050 mol NaCl(s)and 0.050 mol AgNO3(s)are dissolved in 500.mL of 3.0 M NH3? [Kf for Ag(NH3)2+ is 1.5 × 107; Ksp(AgCl)= 1.6 × 10-10]

Accepted Answer

Question 11

Methyl red is a common acid-base indicator.It has a Ka equal to 6.3 × 10-6.Its un-ionized form is red and its anionic form is yellow.What color would a methyl red solution have at pH = 7.8?

Accepted Answer

A)  green
B)  red
C)  blue
D)  yellow
E)  violetF) C) and D)
G) C) and E)

Question 12

A saturated sodium carbonate solution at 100°C contains 45.5 g of dissolved sodium carbonate per 100.mL of solution.The solubility product constant for sodium carbonate at this temperature is

Accepted Answer

A)  79.0
B)  0.316
C)  0.0790
D)  36.8
E)  316F) A) and B)
G) All of the above

Question 13

An environmental chemist obtained a 200.mL sample of lake water believed to be contaminated with a single monoprotic strong acid.Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint.What is the concentration of H+ in the lake?

Accepted Answer

Question 14

Calculate the equilibrium constant Kc for the following overall reaction:
AgCl(s)+ 2CN-(aq)   
Ag(CN)2-(aq)+ Cl-(aq)
For AgCl, Ksp = 1.6 × 10-10; for Ag(CN)2-, Kf = 1.0 × 1021.

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Question 15

At 25 °C, the base ionization constant for NH3 is 1.8 × 10-5.If 0.0800 mole of solid magnesium chloride is dissolved in a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100.ml of 0.150 M ammonia, will a precipitate of magnesium hydroxide form? (Assume the volume of the solution is unchanged.The solubility product constant for magnesium hydroxide is 1.5 × 10-11.)

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Question 16

A sample of rainwater collected near a lead smelter is analyzed for acid content.Experiments show that a 100.mL sample of the rainwater is neutralized by 22.4 milliters of 0.0122 M NaOH.Assuming that the acid present is sulfurous acid, which resulted from the reaction of SO2 with water, what is the molarity of acid in the rainwater?

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Question 17

The pH at the equivalence point of a titration may differ from 7.0 due to

Accepted Answer

A)  the initial concentration of the standard solution.
B)  the indicator used.
C)  the self-ionization of H2O.
D)  the initial pH of the unknown.
E)  hydrolysis of the salt formed.F) B) and C)
G) D) and E)

Question 18

A solution is prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl.What is the pH of this solution? [Ka(HOCl) = 3.2 × 10-8]

Accepted Answer

A)  4.10
B)  7.00
C)  7.19
D)  7.49
E)  7.80F) A) and D)
G) B) and E)

Question 19

Calculate the molar solubility of AgBr in a 0.25M solution of NH3(aq) (Ksp (AgBr) = 7.7 x 10-13 ; Kf (Ag(NH3) 2+) = 1.5 x 107.

Accepted Answer

A)  8.8 x 10-7 M
B)  3.4 x 10-3 M
C)  8.4 x 10-4 M
D)  2.5 x 10-1 M
E)  9.7 x 102 MF) B) and C)
G) B) and D)

Question 20

What is the optimum pH of a sodium formate/formic acid buffer? (For formic acid, Ka = 1.7 × 10-4)

Accepted Answer

Exam 16: Acid-Base Equilibria and Solubility Equilibria

Calculate the molar solubility of AgBr in a 0.25M solution of NH₃(aq) (K_sp (AgBr) = 7.7 x 10^-13 ; K_f (Ag(NH₃) ₂⁺) = 1.5 x 10⁷.

Correct Answer
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A saturated sodium carbonate solution at 100°C contains 45.5 g of dissolved sodium carbonate per 100.mL of solution.The solubility product constant for sodium carbonate at this temperature is

Correct Answer
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Calculate the pH at the equivalence point for the titration of 0.22 M HCN with 0.22 M NaOH.(K_a = 4.9 × 10^-10 for HCN)

Correct Answer
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Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (K_a = 4.9 × 10^-10) solution.

Correct Answer
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The pH at the equivalence point of a titration may differ from 7.0 due to

Correct Answer
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Methyl red is a common acid-base indicator.It has a K_a equal to 6.3 × 10^-6.Its un-ionized form is red and its anionic form is yellow.What color would a methyl red solution have at pH = 7.8?

Correct Answer
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Consider a buffer solution prepared from HOCl and NaOCl.Which is the net ionic equation for the reaction that occurs when NaOH is added to this buffer?

Correct Answer
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An environmental chemist obtained a 200.mL sample of lake water believed to be contaminated with a single monoprotic strong acid.Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint.What is the concentration of H⁺ in the lake?

Correct Answer
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An environmental chemist obtained a 200.mL sample of lake water believed to be contaminated with a single monoprotic strong acid.Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint.What is the pH of the lake?

Correct Answer
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Will a precipitate of AgCl form when 0.050 mol NaCl(s)and 0.050 mol AgNO₃(s)are dissolved in 500.mL of 3.0 M NH₃? [K_fforAg(NH₃)₂⁺is 1.5 × 10⁷; K_sp(AgCl)= 1.6 × 10^-10]

Correct Answer
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Write an equation showing the net reaction that occurs when a strong base is added to a CO₃^2-/HCO₃^- buffer solution (for carbonic acid, K_a1 = 4.2 × 10^-7, K_a2 = 2.4 × 10^-8):

Correct Answer
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Correct Answer
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A saturated sodium carbonate solution at 0°C contains 7.1 g of dissolved sodium carbonate per 100.mL of solution.The solubility product constant for sodium carbonate at this temperature is

Correct Answer
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The K_sp of CaF₂ is 4 × 10^-11.What is the maximum concentration of Ca²⁺ possible in a 0.10 M NaF solution?

Correct Answer
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Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa and compare your answer to the percent ionization you would calculate if the sodium formate were not present.Explain the difference, if any.(K_a = 1.7 × 10^-4)

Correct Answer
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3.4%; the addition of formate ...
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A solution is prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl.What is the pH of this solution? [K_a(HOCl) = 3.2 × 10^-8]

Correct Answer
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Correct Answer
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Calculate the equilibrium constant K_c for the following overall reaction: AgCl(s)+ 2CN^-(aq) Ag(CN)₂^-(aq)+ Cl^-(aq) For AgCl, K_sp = 1.6 × 10^-10; for Ag(CN)₂^-, K_f = 1.0 × 10²¹.

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What is the optimum pH of a sodium formate/formic acid buffer? (For formic acid, K_a = 1.7 × 10^-4)

Correct Answer
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To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C₆H₅COOH) is added 1.00 mL of 12.0 M HCl.What is the percentage ionization of the benzoic acid in the resulting solution? [K_a(C₆H₅COOH) = 6.5 × 10^-5]

Correct Answer
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Exam 16: Acid-Base Equilibria and Solubility Equilibria

Calculate the molar solubility of AgBr in a 0.25M solution of NH3(aq) (Ksp (AgBr) = 7.7 x 10-13 ; Kf (Ag(NH3) 2+) = 1.5 x 107.

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A saturated sodium carbonate solution at 100°C contains 45.5 g of dissolved sodium carbonate per 100.mL of solution.The solubility product constant for sodium carbonate at this temperature is

Correct AnswerverifiedShow Answer

Calculate the pH at the equivalence point for the titration of 0.22 M HCN with 0.22 M NaOH.(Ka = 4.9 × 10-10 for HCN)

Correct AnswerverifiedShow Answer

Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 × 10-10) solution.

Correct AnswerverifiedShow Answer

The pH at the equivalence point of a titration may differ from 7.0 due to

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Methyl red is a common acid-base indicator.It has a Ka equal to 6.3 × 10-6.Its un-ionized form is red and its anionic form is yellow.What color would a methyl red solution have at pH = 7.8?

Correct AnswerverifiedShow Answer

Consider a buffer solution prepared from HOCl and NaOCl.Which is the net ionic equation for the reaction that occurs when NaOH is added to this buffer?

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An environmental chemist obtained a 200.mL sample of lake water believed to be contaminated with a single monoprotic strong acid.Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint.What is the concentration of H+ in the lake?

Correct AnswerverifiedShow Answer

An environmental chemist obtained a 200.mL sample of lake water believed to be contaminated with a single monoprotic strong acid.Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint.What is the pH of the lake?

Correct AnswerverifiedShow Answer

Will a precipitate of AgCl form when 0.050 mol NaCl(s)and 0.050 mol AgNO3(s)are dissolved in 500.mL of 3.0 M NH3? [Kf for Ag(NH3)2+ is 1.5 × 107; Ksp(AgCl)= 1.6 × 10-10]

Correct AnswerverifiedShow Answer

Write an equation showing the net reaction that occurs when a strong base is added to a CO32-/HCO3- buffer solution (for carbonic acid, Ka1 = 4.2 × 10-7, Ka2 = 2.4 × 10-8):

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A saturated sodium carbonate solution at 0°C contains 7.1 g of dissolved sodium carbonate per 100.mL of solution.The solubility product constant for sodium carbonate at this temperature is

Correct AnswerverifiedShow Answer

The Ksp of CaF2 is 4 × 10-11.What is the maximum concentration of Ca2+ possible in a 0.10 M NaF solution?

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Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa and compare your answer to the percent ionization you would calculate if the sodium formate were not present.Explain the difference, if any.(Ka = 1.7 × 10-4)

Correct Answerverified3.4%; the addition of formate ...View AnswerShow Answer

A solution is prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl.What is the pH of this solution? [Ka(HOCl) = 3.2 × 10-8]

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Correct AnswerverifiedShow Answer

Calculate the equilibrium constant Kc for the following overall reaction: AgCl(s)+ 2CN-(aq) Ag(CN)2-(aq)+ Cl-(aq) For AgCl, Ksp = 1.6 × 10-10; for Ag(CN)2-, Kf = 1.0 × 1021.

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What is the optimum pH of a sodium formate/formic acid buffer? (For formic acid, Ka = 1.7 × 10-4)

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To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C6H5COOH) is added 1.00 mL of 12.0 M HCl.What is the percentage ionization of the benzoic acid in the resulting solution? [Ka(C6H5COOH) = 6.5 × 10-5]

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Calculate the molar solubility of AgBr in a 0.25M solution of NH₃(aq) (K_sp (AgBr) = 7.7 x 10^-13 ; K_f (Ag(NH₃) ₂⁺) = 1.5 x 10⁷.

Correct Answer
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Correct Answer
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Calculate the pH at the equivalence point for the titration of 0.22 M HCN with 0.22 M NaOH.(K_a = 4.9 × 10^-10 for HCN)

Correct Answer
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Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (K_a = 4.9 × 10^-10) solution.

Correct Answer
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Correct Answer
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Methyl red is a common acid-base indicator.It has a K_a equal to 6.3 × 10^-6.Its un-ionized form is red and its anionic form is yellow.What color would a methyl red solution have at pH = 7.8?

Correct Answer
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Correct Answer
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An environmental chemist obtained a 200.mL sample of lake water believed to be contaminated with a single monoprotic strong acid.Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint.What is the concentration of H⁺ in the lake?

Correct Answer
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Correct Answer
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Will a precipitate of AgCl form when 0.050 mol NaCl(s)and 0.050 mol AgNO₃(s)are dissolved in 500.mL of 3.0 M NH₃? [K_fforAg(NH₃)₂⁺is 1.5 × 10⁷; K_sp(AgCl)= 1.6 × 10^-10]

Correct Answer
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Write an equation showing the net reaction that occurs when a strong base is added to a CO₃^2-/HCO₃^- buffer solution (for carbonic acid, K_a1 = 4.2 × 10^-7, K_a2 = 2.4 × 10^-8):

Correct Answer
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Correct Answer
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Correct Answer
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The K_sp of CaF₂ is 4 × 10^-11.What is the maximum concentration of Ca²⁺ possible in a 0.10 M NaF solution?

Correct Answer
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Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa and compare your answer to the percent ionization you would calculate if the sodium formate were not present.Explain the difference, if any.(K_a = 1.7 × 10^-4)

Correct Answer
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3.4%; the addition of formate ...
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A solution is prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl.What is the pH of this solution? [K_a(HOCl) = 3.2 × 10^-8]

Correct Answer
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Correct Answer
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Calculate the equilibrium constant K_c for the following overall reaction: AgCl(s)+ 2CN^-(aq) Ag(CN)₂^-(aq)+ Cl^-(aq) For AgCl, K_sp = 1.6 × 10^-10; for Ag(CN)₂^-, K_f = 1.0 × 10²¹.

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What is the optimum pH of a sodium formate/formic acid buffer? (For formic acid, K_a = 1.7 × 10^-4)

Correct Answer
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To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C₆H₅COOH) is added 1.00 mL of 12.0 M HCl.What is the percentage ionization of the benzoic acid in the resulting solution? [K_a(C₆H₅COOH) = 6.5 × 10^-5]

Correct Answer
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