Question 1

The solubility of silver chloride is greater in 0.01 M NH3(aq)because of formation of the coordination complex Ag(NH3)2+(aq).

Accepted Answer

A) True 
 B)False

Question 2

Which of the following water-insoluble salts is more soluble in 1.0 M HClO4(aq)?

Accepted Answer

A) AgBr 
B) PbF2 
C) Hg2Br2  
D) PbI2  
E) AgClO4 
A) AgBr 
B) PbF2 
C) Hg2Br2  
D) PbI2  
E) AgClO4

Question 3

Calculate the [H+] in an aqueous solution that is 0.0755 M HF and 0.100 M NaF.The value of Ka for HF is 3.5 * 10-4.

Accepted Answer

A) 4.6 * 10-4 M 
B) 2.6 *10-4 M 
C) 3.5 * 10-4 M 
D) 0.176 M 
E) 0.0755 M 
A) 4.6 * 10-4 M 
B) 2.6 *10-4 M 
C) 3.5 * 10-4 M 
D) 0.176 M 
E) 0.0755 M

Question 4

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer HA(aq)/NaA(aq).The Ka of HA is 4.1 *10-5.

Accepted Answer

4.1 * 10<s

Question 5

At the stoichiometric point in the titration of 0.260 M CH3NH2(aq)with 0.260 M HCl(aq),

Accepted Answer

A) the pH is less than 7. 
B) [CH3NH3+] = 0.260 M. 
C) the pH is 7.0. 
D) [CH3NH2] = 0.130 M. 
E) the pH is greater than 7. 
A) the pH is less than 7. 
B) [CH3NH3+] = 0.260 M. 
C) the pH is 7.0. 
D) [CH3NH2] = 0.130 M. 
E) the pH is greater than 7.

Question 6

What is the pH of an aqueous solution that is 0.12 M C6H5NH2 (Kb = 4.3 * 10-10)and 0.018 M C6H5NH3Cl?

Accepted Answer

A) 5.46 
B) 10.19 
C) 4.63 
D) 3.81 
E) 8.54 
A) 5.46 
B) 10.19 
C) 4.63 
D) 3.81 
E) 8.54

Question 7

What is the pH at the half-stoichiometric point for the titration of 0.22 M HNO2(aq)with 0.10 M KOH(aq)? For HNO2,Ka = 4.3 * 10-4.

Accepted Answer

A) 2.31 
B) 7.00 
C) 2.01 
D) 3.37 
E) 2.16 
A) 2.31 
B) 7.00 
C) 2.01 
D) 3.37 
E) 2.16

Question 8

Consider the titration of 10.0 mL of 0.100 M (CH3)3N(aq)with 0.100 M HClO4(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of acid?

Accepted Answer

Question 9

The weak base,B,has Kb = 3.1 × 10-4.The pH of a solution in which [B] = [BH+] is

Accepted Answer

A) 3.51 
B) 10.79 
C) 7.00 
D) 10.49 
E) 5.92 
A) 3.51 
B) 10.79 
C) 7.00 
D) 10.49 
E) 5.92

Question 10

The following compounds are available as 0.10 M aqueous solutions.   Which two solutions could be used to prepare a buffer with a pH of ~ 7?

Accepted Answer

The answer of The following compounds are available as 0.10...

Question 11

The titration curve for the titration of 0.100 M Na2CO3(aq)with 0.100 M HClO4(aq)is:   Estimate pKb1.

Accepted Answer

A) 8.5 
B) 6.4 
C) 3.7 
D) 10.3 
E) 7.6 
A) 8.5 
B) 6.4 
C) 3.7 
D) 10.3 
E) 7.6

Question 12

What is the pH of an aqueous solution that is 0.60 (CH3)3N (Kb = 6.5 * 10-5)and 0.95 M (CH3)3NHCl?

Accepted Answer

A) 4.39 
B) 10.01 
C) 3.99 
D) 9.81 
E) 9.61 
A) 4.39 
B) 10.01 
C) 3.99 
D) 9.81 
E) 9.61

Question 13

At the stoichiometric point in the titration of 0.130 M HCOOH(aq)with 0.130 M KOH(aq),

Accepted Answer

A) the pH is 7.0. 
B) [HCOOH] = 0.0650 M. 
C) [HCO2-] = 0.130 M. 
D) the pH is greater than 7. 
E) the pH is less than 7. 
A) the pH is 7.0. 
B) [HCOOH] = 0.0650 M. 
C) [HCO2-] = 0.130 M. 
D) the pH is greater than 7. 
E) the pH is less than 7.

Question 14

Choose the effective pH range of an aniline/anilinium chloride buffer.The value of the Kb for aniline is 4.3 * 10-10.

Accepted Answer

A) 3.6-5.6 
B) 8.4-10.4 
C) 1.1-3.1 
D) 5.1-7.1 
E) 10.1-12.1 
A) 3.6-5.6 
B) 8.4-10.4 
C) 1.1-3.1 
D) 5.1-7.1 
E) 10.1-12.1

Question 15

Calculate the value of the equilibrium constant for the reaction AgCl(s)+ 2NH3(aq) →Ag(NH3)2+(aq)+ Cl-(aq)
Given Ksp = 1.6 * 10-10 for silver chloride and Kf = 1.6 * 107 for the ammonia complex of Ag+ ions,Ag(NH3)2+.

Accepted Answer

A) 1.0 * 10-17  
B) 6.3 * 109  
C) 6.3 * 10-8  
D) 1.0 * 1017  
E) 2.6 * 10-3  
A) 1.0 * 10-17  
B) 6.3 * 109  
C) 6.3 * 10-8  
D) 1.0 * 1017  
E) 2.6 * 10-3

Question 16

The following compounds are available as 0.10 M aqueous solutions.   Which two solutions could be used to prepare a buffer with a pH of ~ 2.5?

Accepted Answer

The answer of The following compounds are available as 0.10...

Question 17

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH3COOH(aq)with 0.036 M NaOH(aq)? For acetic acid,Ka = 1.8 * 10-5.

Accepted Answer

A) 0.018 M 
B) 0.0090 M 
C) 0.024 M 
D) 0.012 M 
E) 0.036 M 
A) 0.018 M 
B) 0.0090 M 
C) 0.024 M 
D) 0.012 M 
E) 0.036 M

Question 18

If a small amount of a strong base is added to buffer made up of a weak acid,HA,and the sodium salt of its conjugate base,NaA,the pH of the buffer solution does not change appreciably because

Accepted Answer

A) the Ka of HA is changed. 
B) No reaction occurs. 
C) the strong base reacts with A- to give HA,which is a weak acid. 
D) the strong base reacts with HA to give AOH and H+. 
E) the strong base reacts with HA to give A- which is a weak base. 
A) the Ka of HA is changed. 
B) No reaction occurs. 
C) the strong base reacts with A- to give HA,which is a weak acid. 
D) the strong base reacts with HA to give AOH and H+. 
E) the strong base reacts with HA to give A- which is a weak base.

Question 19

What is the pH at the stoichiometric point for the titration of 0.26 M CH3NH2(aq)with 0.26 M HClO4(aq)? For CH3NH2,Kb = 3.6 * 10-4.

Accepted Answer

A) 5.72 
B) 7.00 
C) 5.57 
D) 2.16 
E) 2.01 
A) 5.72 
B) 7.00 
C) 5.57 
D) 2.16 
E) 2.01

Question 20

When pyridinium chloride is added to C5H5N(aq),

Accepted Answer

A) the pH of the solution does not change. 
B) the pH of the solution increases. 
C) the pH of the solution decreases. 
D) the Kb increases. 
E) the equilibrium concentration of NH3(aq)decreases. 
A) the pH of the solution does not change. 
B) the pH of the solution increases. 
C) the pH of the solution decreases. 
D) the Kb increases. 
E) the equilibrium concentration of NH3(aq)decreases.

The solubility of silver chloride is greater in 0.01 M NH₃(aq)because of formation of the coordination complex Ag(NH₃)₂⁺(aq).

Which of the following water-insoluble salts is more soluble in 1.0 M HClO₄(aq)?

Calculate the [H⁺] in an aqueous solution that is 0.0755 M HF and 0.100 M NaF.The value of K_a for HF is 3.5 * 10^-4.

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer HA(aq)/NaA(aq).The K_a of HA is 4.1 *10^-5.

At the stoichiometric point in the titration of 0.260 M CH₃NH₂(aq)with 0.260 M HCl(aq),

What is the pH of an aqueous solution that is 0.12 M C₆H₅NH₂ (K_b = 4.3 * 10^-10)and 0.018 M C₆H₅NH₃Cl?

What is the pH at the half-stoichiometric point for the titration of 0.22 M HNO₂(aq)with 0.10 M KOH(aq)? For HNO₂,K_a = 4.3 * 10^-4.

Consider the titration of 10.0 mL of 0.100 M (CH₃)₃N(aq)with 0.100 M HClO₄(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of acid?

The weak base,B,has K_b = 3.1 × 10^-⁴.The pH of a solution in which [B] = [BH⁺] is

The following compounds are available as 0.10 M aqueous solutions. Which two solutions could be used to prepare a buffer with a pH of ~ 7?

The titration curve for the titration of 0.100 M Na₂CO₃(aq)with 0.100 M HClO₄(aq)is: Estimate pK_b1.

What is the pH of an aqueous solution that is 0.60 (CH₃)₃N (K_b = 6.5 * 10^-5)and 0.95 M (CH₃)₃NHCl?

At the stoichiometric point in the titration of 0.130 M HCOOH(aq)with 0.130 M KOH(aq),

Choose the effective pH range of an aniline/anilinium chloride buffer.The value of the K_b for aniline is 4.3 * 10^-10.

Calculate the value of the equilibrium constant for the reaction AgCl(s)+ 2NH₃(aq) →Ag(NH₃)₂+(aq)+ Cl^-(aq) Given K_sp = 1.6 * 10^-¹⁰ for silver chloride and K_f = 1.6 * 10⁷ for the ammonia complex of Ag⁺ ions,Ag(NH₃)²⁺.

The following compounds are available as 0.10 M aqueous solutions. Which two solutions could be used to prepare a buffer with a pH of ~ 2.5?

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH₃COOH(aq)with 0.036 M NaOH(aq)? For acetic acid,K_a = 1.8 * 10^-5.

If a small amount of a strong base is added to buffer made up of a weak acid,HA,and the sodium salt of its conjugate base,NaA,the pH of the buffer solution does not change appreciably because

What is the pH at the stoichiometric point for the titration of 0.26 M CH₃NH₂(aq)with 0.26 M HClO₄(aq)? For CH₃NH₂,K_b = 3.6 * 10^-⁴.

When pyridinium chloride is added to C₅H₅N(aq),

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Exam 13: Aqueous Equilibria

The solubility of silver chloride is greater in 0.01 M NH3(aq)because of formation of the coordination complex Ag(NH3)2+(aq).

Which of the following water-insoluble salts is more soluble in 1.0 M HClO4(aq)?

Calculate the [H+] in an aqueous solution that is 0.0755 M HF and 0.100 M NaF.The value of Ka for HF is 3.5 * 10-4.

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer HA(aq)/NaA(aq).The Ka of HA is 4.1 *10-5.

At the stoichiometric point in the titration of 0.260 M CH3NH2(aq)with 0.260 M HCl(aq),

What is the pH of an aqueous solution that is 0.12 M C6H5NH2 (Kb = 4.3 * 10-10)and 0.018 M C6H5NH3Cl?

What is the pH at the half-stoichiometric point for the titration of 0.22 M HNO2(aq)with 0.10 M KOH(aq)? For HNO2,Ka = 4.3 * 10-4.

Consider the titration of 10.0 mL of 0.100 M (CH3)3N(aq)with 0.100 M HClO4(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of acid?

The weak base,B,has Kb = 3.1 × 10-4.The pH of a solution in which [B] = [BH+] is

The following compounds are available as 0.10 M aqueous solutions. Which two solutions could be used to prepare a buffer with a pH of ~ 7?

The titration curve for the titration of 0.100 M Na2CO3(aq)with 0.100 M HClO4(aq)is: Estimate pKb1.

What is the pH of an aqueous solution that is 0.60 (CH3)3N (Kb = 6.5 * 10-5)and 0.95 M (CH3)3NHCl?

At the stoichiometric point in the titration of 0.130 M HCOOH(aq)with 0.130 M KOH(aq),

Choose the effective pH range of an aniline/anilinium chloride buffer.The value of the Kb for aniline is 4.3 * 10-10.

Calculate the value of the equilibrium constant for the reaction AgCl(s)+ 2NH3(aq) →Ag(NH3)2+(aq)+ Cl-(aq) Given Ksp = 1.6 * 10-10 for silver chloride and Kf = 1.6 * 107 for the ammonia complex of Ag+ ions,Ag(NH3)2+.

The following compounds are available as 0.10 M aqueous solutions. Which two solutions could be used to prepare a buffer with a pH of ~ 2.5?

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH3COOH(aq)with 0.036 M NaOH(aq)? For acetic acid,Ka = 1.8 * 10-5.

If a small amount of a strong base is added to buffer made up of a weak acid,HA,and the sodium salt of its conjugate base,NaA,the pH of the buffer solution does not change appreciably because

What is the pH at the stoichiometric point for the titration of 0.26 M CH3NH2(aq)with 0.26 M HClO4(aq)? For CH3NH2,Kb = 3.6 * 10-4.

When pyridinium chloride is added to C5H5N(aq),

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The solubility of silver chloride is greater in 0.01 M NH₃(aq)because of formation of the coordination complex Ag(NH₃)₂⁺(aq).

Which of the following water-insoluble salts is more soluble in 1.0 M HClO₄(aq)?

Calculate the [H⁺] in an aqueous solution that is 0.0755 M HF and 0.100 M NaF.The value of K_a for HF is 3.5 * 10^-4.

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer HA(aq)/NaA(aq).The K_a of HA is 4.1 *10^-5.

At the stoichiometric point in the titration of 0.260 M CH₃NH₂(aq)with 0.260 M HCl(aq),

What is the pH of an aqueous solution that is 0.12 M C₆H₅NH₂ (K_b = 4.3 * 10^-10)and 0.018 M C₆H₅NH₃Cl?

What is the pH at the half-stoichiometric point for the titration of 0.22 M HNO₂(aq)with 0.10 M KOH(aq)? For HNO₂,K_a = 4.3 * 10^-4.

Consider the titration of 10.0 mL of 0.100 M (CH₃)₃N(aq)with 0.100 M HClO₄(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of acid?

The weak base,B,has K_b = 3.1 × 10^-⁴.The pH of a solution in which [B] = [BH⁺] is

The titration curve for the titration of 0.100 M Na₂CO₃(aq)with 0.100 M HClO₄(aq)is: Estimate pK_b1.

What is the pH of an aqueous solution that is 0.60 (CH₃)₃N (K_b = 6.5 * 10^-5)and 0.95 M (CH₃)₃NHCl?

Choose the effective pH range of an aniline/anilinium chloride buffer.The value of the K_b for aniline is 4.3 * 10^-10.

Calculate the value of the equilibrium constant for the reaction AgCl(s)+ 2NH₃(aq) →Ag(NH₃)₂+(aq)+ Cl^-(aq) Given K_sp = 1.6 * 10^-¹⁰ for silver chloride and K_f = 1.6 * 10⁷ for the ammonia complex of Ag⁺ ions,Ag(NH₃)²⁺.

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH₃COOH(aq)with 0.036 M NaOH(aq)? For acetic acid,K_a = 1.8 * 10^-5.

What is the pH at the stoichiometric point for the titration of 0.26 M CH₃NH₂(aq)with 0.26 M HClO₄(aq)? For CH₃NH₂,K_b = 3.6 * 10^-⁴.

When pyridinium chloride is added to C₅H₅N(aq),