Question 1

Calculate the pH of a 0.02 M solution of KOH.

Accepted Answer

A) 1.7 
B) 15.7 
C) 14.0 
D) 12.3 
E) cannot calculate answer unless a volume is given 
A) 1.7 
B) 15.7 
C) 14.0 
D) 12.3 
E) cannot calculate answer unless a volume is given D

Question 2

The pH of a 1.0 M sodium acetate solution is:

Accepted Answer

A) 7.0 
B) greater than 7.0 
C) less than 7.0 
D) not enough information given 
E) none of these (A-
D)  
A) 7.0 
B) greater than 7.0 
C) less than 7.0 
D) not enough information given 
E) none of these (A-
D)  B

Question 3

In the reaction: CaO(s)+ SO2(g) $\to$CaSO3(s)

Accepted Answer

A) Ca2+ acts as a Lewis acid and SO32- acts as a Lewis base. 
B) O2- acts as a Lewis base and SO2 acts as a Lewis acid. 
C) O2- acts as a Lewis base and Ca2+ acts as a Lewis acid. 
D) CaO is the Lewis acid and CaSO3 is its conjugate base. 
E) SO2 is the Lewis acid and CaSO3 is its conjugate base. 
A) Ca2+ acts as a Lewis acid and SO32- acts as a Lewis base. 
B) O2- acts as a Lewis base and SO2 acts as a Lewis acid. 
C) O2- acts as a Lewis base and Ca2+ acts as a Lewis acid. 
D) CaO is the Lewis acid and CaSO3 is its conjugate base. 
E) SO2 is the Lewis acid and CaSO3 is its conjugate base. B

Question 4

The hydrogen halides (HF,HCl,HBr,and HI)are all polar molecules.The strength of the acid each forms in water is based on which of the following?

Accepted Answer

A) the polarity of the molecule 
B) the size of the molecule 
C) the strength of the bond 
D) two of these 
E) none of these 
A) the polarity of the molecule 
B) the size of the molecule 
C) the strength of the bond 
D) two of these 
E) none of these

Question 5

What is the equilibrium concentration of H2PO4- in a 0.202 M solution of H3PO4(aq)? (Ka1 = 7.5 $\times$10-3,Ka2 = 6.2 $\times$10-8,Ka3 = 4.8 $\times$10-13)

Accepted Answer

A) 1.1 $\times$ 10-4 M 
B) 3.5 $\times$ 10-2 M 
C) 3.9 $\times$ 10-2 M 
D) 7.5 $\times$ 10-3 M 
E) 6.2 $\times$ 10-8 M 
A) 1.1 $\times$ 10-4 M 
B) 3.5 $\times$ 10-2 M 
C) 3.9 $\times$ 10-2 M 
D) 7.5 $\times$ 10-3 M 
E) 6.2 $\times$ 10-8 M

Question 6

Calculate the pH of a 0.49 M solution of NaC2H3O2 (for HC2H3O2 Ka = 1.8 $\times$ 10-5).

Accepted Answer

A) 4.78 
B) 9.22 
C) 8.95 
D) 5.05 
E) none of these 
A) 4.78 
B) 9.22 
C) 8.95 
D) 5.05 
E) none of these

Question 7

As water is heated,its pH decreases.This means that:

Accepted Answer

A) The water is no longer neutral. 
B) [H+] > [OH-] 
C) [OH-] > [H+] 
D) A and B are correct. 
E) None of these. 
A) The water is no longer neutral. 
B) [H+] > [OH-] 
C) [OH-] > [H+] 
D) A and B are correct. 
E) None of these.

Question 8

The pKa of HOCl is 7.5.Calculate the pH of a 0.31 M solution of HOCl.

Accepted Answer

A) 7.50 
B) 6.50 
C) 4.00 
D) 10.00 
E) 0.31 
A) 7.50 
B) 6.50 
C) 4.00 
D) 10.00 
E) 0.31

Question 9

The equilibrium constant for the reaction A- + H+   HA is called:

Accepted Answer

A) Ka 
B) Kb 
C)    
D)    
E) KwKa 
A) Ka 
B) Kb 
C)    
D)    
E) KwKa

Question 10

Given that the Ka for HOCl is 3.45 $\times$ 10-8,calculate the K value for the reaction of HOCl with OH-.

Accepted Answer

A) 3.45 $\times$ 106 
B) 3.45 
C) 3.45 $\times$10-22 
D) 2.90 $\times$ 10-7 
E) 2.90 $\times$ 1021 
A) 3.45 $\times$ 106 
B) 3.45 
C) 3.45 $\times$10-22 
D) 2.90 $\times$ 10-7 
E) 2.90 $\times$ 1021

Question 11

The two acid dissociation constants for carbonic acid,H2CO3,are 4.3 $\times$ 10-7 and 4.8 $\times$ 10-11 at 25°C.The base constant,Kb,or hydrolysis constant for HCO3- is:

Accepted Answer

A) 4.3 $\times$ 10-7 
B) 4.8 $\times$ 10-11 
C) 2.1 $\times$ 10-17 
D) 2.3 $\times$ 10-8 
E) 6.2 $\times$ 10-22 
A) 4.3 $\times$ 10-7 
B) 4.8 $\times$ 10-11 
C) 2.1 $\times$ 10-17 
D) 2.3 $\times$ 10-8 
E) 6.2 $\times$ 10-22

Question 12

The pH of a 0.118 M solution of an aqueous weak acid (HA)is 3.20.The Ka for the weak acid is:

Accepted Answer

A) 5.4 $\times$ 10-3 
B) 4.0 $\times$ 10-7 
C) 3.4 $\times$ 10-6 
D) 3.2 
E) none of these 
A) 5.4 $\times$ 10-3 
B) 4.0 $\times$ 10-7 
C) 3.4 $\times$ 10-6 
D) 3.2 
E) none of these

Question 13

Consider the reaction HNO2(aq)+ H2O(l)   H3O+(aq)+ NO2-(aq).Which species is a conjugate base?

Accepted Answer

A) HNO2(aq) 
B) H2O(l) 
C) H3O+(aq) 
D) NO2-(aq) 
E) two of these 
A) HNO2(aq) 
B) H2O(l) 
C) H3O+(aq) 
D) NO2-(aq) 
E) two of these

Question 14

Calculate the pOH of a 4.9 M solution of HCl.

Accepted Answer

A) -0.69 
B) 13.31 
C) 14.69 
D) 0.69 
E) -0.96 
A) -0.69 
B) 13.31 
C) 14.69 
D) 0.69 
E) -0.96

Question 15

The pH of a solution of 1.9 M H2A (Ka1 = 1.0 $\times$ 10-6 and Ka2 is 1.0 $\times$ 10-10)is:

Accepted Answer

A) 10.00 
B) 5.72 
C) 11.14 
D) 2.86 
E) none of these 
A) 10.00 
B) 5.72 
C) 11.14 
D) 2.86 
E) none of these

Question 16

Which of the following is the correct order for increasing pHs for equimolar solutions of HNO3,KCl,NH4Cl,KOH,and NaC2H3O2? (Ka for HC2H3O2 is 1.80 $\times$ 10-5,Ka for NH4+ is 5.56 $\times$10-10).

Accepted Answer

A) KCl,NH4Cl,HNO3,KOH,NaC2H3O2 
B) HNO3,KCl,NH4Cl,KOH,NaC2H3O2 
C) NH4Cl,HNO3,KCl,KOH,NaC2H3O2 
D) HNO3,NH4Cl,KCl,NaC2H3O2,KOH 
E) none of these 
A) KCl,NH4Cl,HNO3,KOH,NaC2H3O2 
B) HNO3,KCl,NH4Cl,KOH,NaC2H3O2 
C) NH4Cl,HNO3,KCl,KOH,NaC2H3O2 
D) HNO3,NH4Cl,KCl,NaC2H3O2,KOH 
E) none of these

Question 17

Consider the reaction HOCl + FS1U1P1-S1S1P0   HF + OClS1U1P1-S1S1P0
-Given that Ka for HOCl is 3.5 $\times$ 10-8 and the Ka for HF is 7.2 $\times$ 10-4 (both at 25°C),which of the following is true concerning K for the above reaction at 25°C?

Accepted Answer

A) K is greater than 1. 
B) K is less than 1. 
C) K is equal to 1. 
D) Cannot be determined with the above information. 
E) None of these (A-
D) . 
A) K is greater than 1. 
B) K is less than 1. 
C) K is equal to 1. 
D) Cannot be determined with the above information. 
E) None of these (A-
D) .

Question 18

Calculate the [H+] in a solution that has a pH of 8.73.

Accepted Answer

A) 1.9 $\times$ 10-9 M 
B) 5.4 $\times$ 10-6 M 
C) 8.7 $\times$ 10-9 M 
D) 9.4 $\times$10-1 M 
E) 7.2 $\times$ 10-1 M 
A) 1.9 $\times$ 10-9 M 
B) 5.4 $\times$ 10-6 M 
C) 8.7 $\times$ 10-9 M 
D) 9.4 $\times$10-1 M 
E) 7.2 $\times$ 10-1 M

Question 19

What is the equilibrium constant for the following reaction? N3- + H3O+   HN3 + H2O The Ka value for HN3 = 1.9 $\times$ 10-5.

Accepted Answer

A) 5.3 $\times$ 10-10 
B) 1.9 $\times$ 10-9 
C) 1.9 $\times$ 10-5 
D) 5.3 $\times$ 104 
E) 1.9 $\times$ 109 
A) 5.3 $\times$ 10-10 
B) 1.9 $\times$ 10-9 
C) 1.9 $\times$ 10-5 
D) 5.3 $\times$ 104 
E) 1.9 $\times$ 109

Question 20

What is the pH of a 0.73 M KCl solution?

Accepted Answer

A) 0.14 
B) 7.00 
C) 13.86 
D) 3.65 
E) 9.20 
A) 0.14 
B) 7.00 
C) 13.86 
D) 3.65 
E) 9.20

Calculate the pH of a 0.02 M solution of KOH.

The pH of a 1.0 M sodium acetate solution is:

In the reaction: CaO(s)+ SO₂(g) $\to$ CaSO₃(s)

The hydrogen halides (HF,HCl,HBr,and HI)are all polar molecules.The strength of the acid each forms in water is based on which of the following?

What is the equilibrium concentration of H₂PO₄^- in a 0.202 M solution of H₃PO₄(aq)? (K_a1 = 7.5 $\times$ 10^-³,K_a2 = 6.2 $\times$ 10^-⁸,K_a3 = 4.8 $\times$ 10^-¹³)

Calculate the pH of a 0.49 M solution of NaC₂H₃O₂ (for HC₂H₃O₂ K_a = 1.8 $\times$ 10^-⁵).

As water is heated,its pH decreases.This means that:

The pK_a of HOCl is 7.5.Calculate the pH of a 0.31 M solution of HOCl.

The equilibrium constant for the reaction A^- + H⁺ HA is called:

Given that the K_a for HOCl is 3.45 $\times$ 10^-⁸,calculate the K value for the reaction of HOCl with OH^-.

The two acid dissociation constants for carbonic acid,H₂CO₃,are 4.3 $\times$ 10^-⁷ and 4.8 $\times$ 10^-¹¹ at 25°C.The base constant,K_b,or hydrolysis constant for HCO₃^- is:

The pH of a 0.118 M solution of an aqueous weak acid (HA)is 3.20.The K_a for the weak acid is:

Consider the reaction HNO₂(aq)+ H₂O(l) H₃O⁺(aq)+ NO₂^-(aq).Which species is a conjugate base?

Calculate the pOH of a 4.9 M solution of HCl.

The pH of a solution of 1.9 M H₂A (K_a1= 1.0 $\times$ 10^-⁶ and K_a2is 1.0 $\times$ 10^-¹⁰)is:

Which of the following is the correct order for increasing pHs for equimolar solutions of HNO₃,KCl,NH₄Cl,KOH,and NaC₂H₃O₂? (K_a for HC₂H₃O₂ is 1.80 $\times$ 10^-⁵,K_a for NH₄⁺ is 5.56 $\times$ 10^-¹⁰).

Calculate the [H⁺] in a solution that has a pH of 8.73.

What is the pH of a 0.73 M KCl solution?

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Exam 14: Acids and Bases

Calculate the pH of a 0.02 M solution of KOH.

The pH of a 1.0 M sodium acetate solution is:

In the reaction: CaO(s)+ SO2(g) →\to→ CaSO3(s)

The hydrogen halides (HF,HCl,HBr,and HI)are all polar molecules.The strength of the acid each forms in water is based on which of the following?

What is the equilibrium concentration of H2PO4- in a 0.202 M solution of H3PO4(aq)? (Ka1 = 7.5 ×\times× 10-3,Ka2 = 6.2 ×\times× 10-8,Ka3 = 4.8 ×\times× 10-13)

Calculate the pH of a 0.49 M solution of NaC2H3O2 (for HC2H3O2 Ka = 1.8 ×\times× 10-5).

As water is heated,its pH decreases.This means that:

The pKa of HOCl is 7.5.Calculate the pH of a 0.31 M solution of HOCl.

The equilibrium constant for the reaction A- + H+ HA is called:

Given that the Ka for HOCl is 3.45 ×\times× 10-8,calculate the K value for the reaction of HOCl with OH-.

The two acid dissociation constants for carbonic acid,H2CO3,are 4.3 ×\times× 10-7 and 4.8 ×\times× 10-11 at 25°C.The base constant,Kb,or hydrolysis constant for HCO3- is:

The pH of a 0.118 M solution of an aqueous weak acid (HA)is 3.20.The Ka for the weak acid is:

Consider the reaction HNO2(aq)+ H2O(l) H3O+(aq)+ NO2-(aq).Which species is a conjugate base?

Calculate the pOH of a 4.9 M solution of HCl.

The pH of a solution of 1.9 M H2A (Ka1 = 1.0 ×\times× 10-6 and Ka2 is 1.0 ×\times× 10-10)is:

Which of the following is the correct order for increasing pHs for equimolar solutions of HNO3,KCl,NH4Cl,KOH,and NaC2H3O2? (Ka for HC2H3O2 is 1.80 ×\times× 10-5,Ka for NH4+ is 5.56 ×\times× 10-10).

Consider the reaction HOCl + F- HF + OCl- -Given that Ka for HOCl is 3.5 ×\times× 10-8 and the Ka for HF is 7.2 ×\times× 10-4 (both at 25°C),which of the following is true concerning K for the above reaction at 25°C?

Calculate the [H+] in a solution that has a pH of 8.73.

What is the equilibrium constant for the following reaction? N3- + H3O+ HN3 + H2O The Ka value for HN3 = 1.9 ×\times× 10-5.

What is the pH of a 0.73 M KCl solution?

Chemical Foundations

Atoms, molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions Stoichiometry

Gases

Thermochemistry

Atomic Structure and Periodicity

Bonding: General Concepts

Covalent Bonding: Orbitals

Liquids and Solids

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Solubility and Complex Ion Equilibria

Spontaneity, entropy, and Free Energy

Electrochemistry

The Nucleus: a Chemists View

The Representative Elements

Transition Metals and Coordination Chemistry

Organic and Biological Molecules

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In the reaction: CaO(s)+ SO₂(g) $\to$ CaSO₃(s)

What is the equilibrium concentration of H₂PO₄^- in a 0.202 M solution of H₃PO₄(aq)? (K_a1 = 7.5 $\times$ 10^-³,K_a2 = 6.2 $\times$ 10^-⁸,K_a3 = 4.8 $\times$ 10^-¹³)

Calculate the pH of a 0.49 M solution of NaC₂H₃O₂ (for HC₂H₃O₂ K_a = 1.8 $\times$ 10^-⁵).

The pK_a of HOCl is 7.5.Calculate the pH of a 0.31 M solution of HOCl.

The equilibrium constant for the reaction A^- + H⁺ HA is called:

Given that the K_a for HOCl is 3.45 $\times$ 10^-⁸,calculate the K value for the reaction of HOCl with OH^-.

The two acid dissociation constants for carbonic acid,H₂CO₃,are 4.3 $\times$ 10^-⁷ and 4.8 $\times$ 10^-¹¹ at 25°C.The base constant,K_b,or hydrolysis constant for HCO₃^- is:

The pH of a 0.118 M solution of an aqueous weak acid (HA)is 3.20.The K_a for the weak acid is:

Consider the reaction HNO₂(aq)+ H₂O(l) H₃O⁺(aq)+ NO₂^-(aq).Which species is a conjugate base?

The pH of a solution of 1.9 M H₂A (K_a1= 1.0 $\times$ 10^-⁶ and K_a2is 1.0 $\times$ 10^-¹⁰)is:

Which of the following is the correct order for increasing pHs for equimolar solutions of HNO₃,KCl,NH₄Cl,KOH,and NaC₂H₃O₂? (K_a for HC₂H₃O₂ is 1.80 $\times$ 10^-⁵,K_a for NH₄⁺ is 5.56 $\times$ 10^-¹⁰).

Calculate the [H⁺] in a solution that has a pH of 8.73.