Question 1

The titration curve for the titration of 0.100 M H2SO3(aq)with 0.100 M KOH(aq)is given below.   
The major species in solution after 75 mL of KOH(aq)has been added are

Accepted Answer

A) HSO3-(aq)and Na+(aq). 
B) SO32-(aq),and Na+(aq). 
C) SO32-(aq),OH-(aq),and Na+(aq). 
D) H2SO3(aq),HSO3-,and Na+(aq). 
E) HSO3-(aq),SO32-(aq),and Na+(aq). 
A) HSO3-(aq)and Na+(aq). 
B) SO32-(aq),and Na+(aq). 
C) SO32-(aq),OH-(aq),and Na+(aq). 
D) H2SO3(aq),HSO3-,and Na+(aq). 
E) HSO3-(aq),SO32-(aq),and Na+(aq).

Question 2

The titration curve for the titration of 0.100 M Na2CO3(aq)with 0.100 M HClO4(aq)is:   
The main species in the solution after the addition of 35 mL of HClO4 are

Accepted Answer

A) HCO3-,H2CO3,Na+,and ClO4-. 
B) H2CO3,Na+,and ClO4-. 
C) CO32-,HCO3,Na+,and ClO4-. 
D) CO32-,Na+,and ClO4-. 
E) HCO3-,Na+,and ClO4-. 
A) HCO3-,H2CO3,Na+,and ClO4-. 
B) H2CO3,Na+,and ClO4-. 
C) CO32-,HCO3,Na+,and ClO4-. 
D) CO32-,Na+,and ClO4-. 
E) HCO3-,Na+,and ClO4-.

Question 3

Calculate the [OH-] in an aqueous solution that is 0.125 M NH3 and 0.300 M NH4Cl.The value of Kb for NH3 is 1.8 *10-5.

Accepted Answer

A) 0.425 M 
B) 0.125 M 
C) 1.8 * 10-5 M 
D) 7.5 *10-6 M 
E) 4.3 * 10-5 M 
A) 0.425 M 
B) 0.125 M 
C) 1.8 * 10-5 M 
D) 7.5 *10-6 M 
E) 4.3 * 10-5 M

Question 4

In the titration of 0.300 M CH3NH2(aq)with 0.300 M HCl(aq),what is the formula of the major species and what is its concentration at the equivalence point?

Accepted Answer

CH₃NH₃⁺(aq);

Question 5

Calculate the [OH-] in an aqueous solution that is 0.125 M NH3 and 0.125 M NH4Cl.The value of Kb for NH3 is 1.8 * 10-5.

Accepted Answer

A) 1.8 * 10-5 M 
B) 5.5 * 10-10 M 
C) 6.7 * 10-12 M 
D) 0.125 M 
E) 1.5 *10-3 M 
A) 1.8 * 10-5 M 
B) 5.5 * 10-10 M 
C) 6.7 * 10-12 M 
D) 0.125 M 
E) 1.5 *10-3 M

Question 6

The solubility of all except which the following compounds increases as the pH of the solution decreases?

Accepted Answer

A) CaF2 
B) Na2CO3 
C) PbSO3 
D) KClO4 
E) CuS 
A) CaF2 
B) Na2CO3 
C) PbSO3 
D) KClO4 
E) CuS

Question 7

The titration curve for the titration of 0.100 M Na2CO3(aq)with 0.100 M HClO4(aq)is:   Estimate pKb2.

Accepted Answer

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

Question 8

A solution is prepared by mixing equal volumes of 0.40 M HF(aq)with 0.40 M KOH(aq).This solution is a buffer.

Accepted Answer

A) True 
 B)False

Question 9

What is the pH of an aqueous solution that is 1.0 M HClO (Ka = 3.0 *10-8)and 0.75 M NaClO?

Accepted Answer

A) 7.64 
B) 7.40 
C) 6.36 
D) 7.52 
E) 6.60 
A) 7.64 
B) 7.40 
C) 6.36 
D) 7.52 
E) 6.60

Question 10

The titration curve for the titration of 0.100 M H2SO3(aq)with 0.100 M KOH(aq)is given below.   Estimate pKa1 and pKa2 of H2SO3.

Accepted Answer

pK_a1 ~ 2.0 a

Question 11

For the titration of 50.0 mL of 0.020 M aqueous salicylic acid with 0.020 M KOH(aq),calculate the pH after the addition of 55.0 mL of KOH(aq).For salycylic acid,pKa = 2.97.

Accepted Answer

A) 10.98 
B) 7.00 
C) 11.26 
D) 12.02 
E) 12.30 
A) 10.98 
B) 7.00 
C) 11.26 
D) 12.02 
E) 12.30

Question 12

For NH3,pKb = 4.74.What is the pH of an aqueous buffer solution that is 0.050 M NH3(aq)and 0.20 M NH4Cl(aq)?

Accepted Answer

A) 9.86 
B) 5.34 
C) 9.26 
D) 8.66 
E) 4.14 
A) 9.86 
B) 5.34 
C) 9.26 
D) 8.66 
E) 4.14

Question 13

Calculate the solubility product of calcium hydroxide given that the solubility of Ca(OH)2(s)in water at 25S1U1P1$\circ$S1S1P0C is 0.011 M.

Accepted Answer

A) 1.5 * 10-8  
B) 1.1 * 10-5  
C) 2.7 * 10-6  
D) 5.3 * 10-6  
E) 1.2 * 10-4  
A) 1.5 * 10-8  
B) 1.1 * 10-5  
C) 2.7 * 10-6  
D) 5.3 * 10-6  
E) 1.2 * 10-4

Question 14

Calculate the equilibrium constant for the reaction that occurs when perchloric acid is added to the buffer B(aq)/BHCl(aq).The Kb of B is 3.4 *10-5.

Accepted Answer

3.4 * 10<s

The titration curve for the titration of 0.100 M H₂SO₃(aq)with 0.100 M KOH(aq)is given below. The major species in solution after 75 mL of KOH(aq)has been added are

The titration curve for the titration of 0.100 M Na₂CO₃(aq)with 0.100 M HClO₄(aq)is: The main species in the solution after the addition of 35 mL of HClO₄ are

Calculate the [OH^-] in an aqueous solution that is 0.125 M NH₃ and 0.300 M NH₄Cl.The value of K_b for NH₃ is 1.8 *10^-5.

In the titration of 0.300 M CH₃NH₂(aq)with 0.300 M HCl(aq),what is the formula of the major species and what is its concentration at the equivalence point?

Calculate the [OH^-] in an aqueous solution that is 0.125 M NH₃ and 0.125 M NH₄Cl.The value of K_b for NH₃ is 1.8 * 10^-5.

The solubility of all except which the following compounds increases as the pH of the solution decreases?

The titration curve for the titration of 0.100 M Na₂CO₃(aq)with 0.100 M HClO₄(aq)is: Estimate pK_b2.

A solution is prepared by mixing equal volumes of 0.40 M HF(aq)with 0.40 M KOH(aq).This solution is a buffer.

What is the pH of an aqueous solution that is 1.0 M HClO (K_a = 3.0 *10^-8)and 0.75 M NaClO?

The titration curve for the titration of 0.100 M H₂SO₃(aq)with 0.100 M KOH(aq)is given below. Estimate pK_a1 and pK_a2 of H₂SO₃.

For the titration of 50.0 mL of 0.020 M aqueous salicylic acid with 0.020 M KOH(aq),calculate the pH after the addition of 55.0 mL of KOH(aq).For salycylic acid,pK_a = 2.97.

For NH₃,pK_b = 4.74.What is the pH of an aqueous buffer solution that is 0.050 M NH₃(aq)and 0.20 M NH₄Cl(aq)?

Calculate the solubility product of calcium hydroxide given that the solubility of Ca(OH)₂(s)in water at 25^$\circ$C is 0.011 M.

Calculate the equilibrium constant for the reaction that occurs when perchloric acid is added to the buffer B(aq)/BHCl(aq).The K_b of B is 3.4 *10^-5.

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Exam 13: Aqueous Equilibria

The titration curve for the titration of 0.100 M H2SO3(aq)with 0.100 M KOH(aq)is given below. The major species in solution after 75 mL of KOH(aq)has been added are

The titration curve for the titration of 0.100 M Na2CO3(aq)with 0.100 M HClO4(aq)is: The main species in the solution after the addition of 35 mL of HClO4 are

Calculate the [OH-] in an aqueous solution that is 0.125 M NH3 and 0.300 M NH4Cl.The value of Kb for NH3 is 1.8 *10-5.

In the titration of 0.300 M CH3NH2(aq)with 0.300 M HCl(aq),what is the formula of the major species and what is its concentration at the equivalence point?

Calculate the [OH-] in an aqueous solution that is 0.125 M NH3 and 0.125 M NH4Cl.The value of Kb for NH3 is 1.8 * 10-5.

The solubility of all except which the following compounds increases as the pH of the solution decreases?

The titration curve for the titration of 0.100 M Na2CO3(aq)with 0.100 M HClO4(aq)is: Estimate pKb2.

A solution is prepared by mixing equal volumes of 0.40 M HF(aq)with 0.40 M KOH(aq).This solution is a buffer.

What is the pH of an aqueous solution that is 1.0 M HClO (Ka = 3.0 *10-8)and 0.75 M NaClO?

The titration curve for the titration of 0.100 M H2SO3(aq)with 0.100 M KOH(aq)is given below. Estimate pKa1 and pKa2 of H2SO3.

For the titration of 50.0 mL of 0.020 M aqueous salicylic acid with 0.020 M KOH(aq),calculate the pH after the addition of 55.0 mL of KOH(aq).For salycylic acid,pKa = 2.97.

For NH3,pKb = 4.74.What is the pH of an aqueous buffer solution that is 0.050 M NH3(aq)and 0.20 M NH4Cl(aq)?

Calculate the solubility product of calcium hydroxide given that the solubility of Ca(OH)2(s)in water at 25 ∘\circ∘ C is 0.011 M.

Calculate the equilibrium constant for the reaction that occurs when perchloric acid is added to the buffer B(aq)/BHCl(aq).The Kb of B is 3.4 *10-5.

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Quantum Mechanics in Action: Atoms

Chemical Bonds

Molecular Shape and Structure

The Properties of Gases

Liquids and Solids

Inorganic Materials

Thermodynamics: The First Law

Thermodynamics: The Second and Third Laws

Physical Equilibria

Chemical Equilibria

Acids and Bases

Electrochemistry

Chemical Kinetics

The Elements: the Main Group Elements

The Elements: The D Block

Nuclear Chemistry

Organic Chemistry I

Organic Chemistry II

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The titration curve for the titration of 0.100 M H₂SO₃(aq)with 0.100 M KOH(aq)is given below. The major species in solution after 75 mL of KOH(aq)has been added are

The titration curve for the titration of 0.100 M Na₂CO₃(aq)with 0.100 M HClO₄(aq)is: The main species in the solution after the addition of 35 mL of HClO₄ are

Calculate the [OH^-] in an aqueous solution that is 0.125 M NH₃ and 0.300 M NH₄Cl.The value of K_b for NH₃ is 1.8 *10^-5.

In the titration of 0.300 M CH₃NH₂(aq)with 0.300 M HCl(aq),what is the formula of the major species and what is its concentration at the equivalence point?

Calculate the [OH^-] in an aqueous solution that is 0.125 M NH₃ and 0.125 M NH₄Cl.The value of K_b for NH₃ is 1.8 * 10^-5.

The titration curve for the titration of 0.100 M Na₂CO₃(aq)with 0.100 M HClO₄(aq)is: Estimate pK_b2.

What is the pH of an aqueous solution that is 1.0 M HClO (K_a = 3.0 *10^-8)and 0.75 M NaClO?

The titration curve for the titration of 0.100 M H₂SO₃(aq)with 0.100 M KOH(aq)is given below. Estimate pK_a1 and pK_a2 of H₂SO₃.

For the titration of 50.0 mL of 0.020 M aqueous salicylic acid with 0.020 M KOH(aq),calculate the pH after the addition of 55.0 mL of KOH(aq).For salycylic acid,pK_a = 2.97.

For NH₃,pK_b = 4.74.What is the pH of an aqueous buffer solution that is 0.050 M NH₃(aq)and 0.20 M NH₄Cl(aq)?

Calculate the solubility product of calcium hydroxide given that the solubility of Ca(OH)₂(s)in water at 25^$\circ$C is 0.011 M.

Calculate the equilibrium constant for the reaction that occurs when perchloric acid is added to the buffer B(aq)/BHCl(aq).The K_b of B is 3.4 *10^-5.