Question 1

What is the pH of 10.0 mL of 0.0020 M HCl?

Accepted Answer

A) 0.70 
B) 2.70 
C) 3.70 
D) 5.70 
E) 10.0 
A) 0.70 
B) 2.70 
C) 3.70 
D) 5.70 
E) 10.0

Question 2

The compound CH3NH2 reacts with water to form CH3NH3+ and OH-.What role does CH3NH2 play in this reaction?

Accepted Answer

Question 3

Calculate the pH of a 0.025 M solution of NaNO2 (Ka(HNO2)= 4.5 x 10-4)

Accepted Answer

Question 4

Identify the conjugate base of HPO42-

Accepted Answer

A) H2O 
B) H2PO4- 
C) H3PO4 
D) PO43- 
E) OH- 
A) H2O 
B) H2PO4- 
C) H3PO4 
D) PO43- 
E) OH-

Question 5

What mass of ammonium chloride must be added to 250.mL of water to give a solution with pH = 4.85? [Kb(NH3)= 1.8 × 10-5]

Accepted Answer

A) 4.7 g 
B) 75 g 
C) 2.3 × 10-3 g 
D) 19 g 
E) 10.g 
A) 4.7 g 
B) 75 g 
C) 2.3 × 10-3 g 
D) 19 g 
E) 10.g

Question 6

What is the pH of a solution prepared by mixing 10.0 mL of a strong acid solution with pH = 2.0 and 10.0 mL of a strong acid solution with pH = 6.0?

Accepted Answer

A) 2.0 
B) 2.3 
C) 4.0 
D) 6.0 
E) 8.0 
A) 2.0 
B) 2.3 
C) 4.0 
D) 6.0 
E) 8.0

Question 7

A 0.14 M HNO2 solution is 5.7% ionized.Calculate the H+ ion concentration.

Accepted Answer

A) 8.0 × 10-3 M 
B) 0.057 M 
C) 0.13 M 
D) 0.14 M 
E) 0.80 M 
A) 8.0 × 10-3 M 
B) 0.057 M 
C) 0.13 M 
D) 0.14 M 
E) 0.80 M

Question 8

The pH of a sample of river water is 6.0.A sample of effluent from a food processing plant has a pH of 4.0.What is the ratio of hydronium ion concentration in the effluent to the hydronium ion concentration in the river?

Accepted Answer

The hydronium ion concentratio

Question 9

Which solution will have the lowest pH?

Accepted Answer

A) 0.10 M HCN 
B) 0.10 M HNO3 
C) 0.10 M NaCl 
D) 0.10 M H2CO3 
E) 0.10 M NaOH 
A) 0.10 M HCN 
B) 0.10 M HNO3 
C) 0.10 M NaCl 
D) 0.10 M H2CO3 
E) 0.10 M NaOH

Question 10

Which of the following is both a Lewis Base and a Brønsted Acid

Accepted Answer

A) H2PO4- 
B) PO43- 
C) NH4+ 
D) F- 
E) BF3 
A) H2PO4- 
B) PO43- 
C) NH4+ 
D) F- 
E) BF3

Question 11

Arrange the acids H2Se, H2Te, and H2S in order of increasing acid strength.

Accepted Answer

A) H2S 2Se 2Te 
B) H2S 2Te 2Se 
C) H2Te 2S 2Se 
D) H2Se 2S 2Te 
E) H2Se 2Te 2S 
A) H2S 2Se 2Te 
B) H2S 2Te 2Se 
C) H2Te 2S 2Se 
D) H2Se 2S 2Te 
E) H2Se 2Te 2S

Question 12

Predict the direction in which the equilibrium will lie for the reaction H2CO3 + F- 
     
HCO3- + HF.Ka1( H2CO3)= 4.2 × 10-7; Ka(HF)= 7.1 × 10-4

Accepted Answer

A) to the right 
B) to the left 
C) in the middle 
A) to the right 
B) to the left 
C) in the middle

Question 13

HCN is classified as a weak acid in water.What does this classification mean?

Accepted Answer

A relatively small f

Question 14

Calculate the concentration of chromate ion (CrO42-)in a 0.450 M solution of chromic acid (H2CrO4).[For chromic acid, Ka1 = 0.18, Ka2 = 3.2 × 10-7.]

Accepted Answer

A) 3.2 × 10-7 M 
B) 1.5 × 10-6 M 
C) 0.081 M 
D) 1.1 × 10-6 M 
E) 0.21 M 
A) 3.2 × 10-7 M 
B) 1.5 × 10-6 M 
C) 0.081 M 
D) 1.1 × 10-6 M 
E) 0.21 M

Question 15

The hydrolysis of NH4F will result in which of the following types of solutions given: (Ka(NH4+)= 5.6 x 10-10, Kb(F-)= 1.4 x 10-11)

Accepted Answer

A) acidic, pH  7 
C) neutral, pH = 7 
A) acidic, pH  7 
C) neutral, pH = 7

Question 16

The OH- concentration in a 2.5 × 10-3 M Ba(OH)2 solution is

Accepted Answer

A) 4.0 × 10-12 M. 
B) 2.5 × 10-3 M. 
C) 5.0 × 10-3 M. 
D) 1.2 × 10-2 M. 
E) 0.025 M. 
A) 4.0 × 10-12 M. 
B) 2.5 × 10-3 M. 
C) 5.0 × 10-3 M. 
D) 1.2 × 10-2 M. 
E) 0.025 M.

Question 17

Which one of the following salts will form an acidic solution on dissolving in water?

Accepted Answer

A) LiBr 
B) NaF 
C) KOH 
D) FeCl3 
E) NaCN 
A) LiBr 
B) NaF 
C) KOH 
D) FeCl3 
E) NaCN

Question 18

Which one of the following equations represents the ionization of a weak monoprotic acid in water?

Accepted Answer

A) HCN(aq)+ H2O(l)     H3O+(aq)+ CN-(aq) 
B) HCN(aq)+ OH-(aq)     H2O(l)+ CN+(aq) 
C) CN- (aq)+ H2O(aq)     HCN(aq)+ OH-(aq) 
D) HCN(aq)+ OH- (aq)     H2O(l)+ CN-(aq) 
E) HCN(aq)+ NH3(aq)     NH4CN(aq) 
A) HCN(aq)+ H2O(l)     H3O+(aq)+ CN-(aq) 
B) HCN(aq)+ OH-(aq)     H2O(l)+ CN+(aq) 
C) CN- (aq)+ H2O(aq)     HCN(aq)+ OH-(aq) 
D) HCN(aq)+ OH- (aq)     H2O(l)+ CN-(aq) 
E) HCN(aq)+ NH3(aq)     NH4CN(aq)

Question 19

Al(OH)3 is an amphoteric hydroxide.Write a balanced ionic equation to show its reaction with HNO3.

Accepted Answer

Al(OH)₃ + 3

Question 20

Given the following Ka values, which anion is the strongest base?

Accepted Answer

A) F- 
B) HCOO- 
C) CN- 
D) NO2- 
E) CH3COO- 
A) F- 
B) HCOO- 
C) CN- 
D) NO2- 
E) CH3COO-

Exam 15: Acids and Bases

What is the pH of 10.0 mL of 0.0020 M HCl?

The compound CH3NH2 reacts with water to form CH3NH3+ and OH-.What role does CH3NH2 play in this reaction?

Calculate the pH of a 0.025 M solution of NaNO2 (Ka(HNO2)= 4.5 x 10-4)

Identify the conjugate base of HPO42-

What mass of ammonium chloride must be added to 250.mL of water to give a solution with pH = 4.85? [Kb(NH3)= 1.8 × 10-5]

What is the pH of a solution prepared by mixing 10.0 mL of a strong acid solution with pH = 2.0 and 10.0 mL of a strong acid solution with pH = 6.0?

A 0.14 M HNO2 solution is 5.7% ionized.Calculate the H+ ion concentration.

The pH of a sample of river water is 6.0.A sample of effluent from a food processing plant has a pH of 4.0.What is the ratio of hydronium ion concentration in the effluent to the hydronium ion concentration in the river?

Which solution will have the lowest pH?

Which of the following is both a Lewis Base and a Brønsted Acid

Arrange the acids H2Se, H2Te, and H2S in order of increasing acid strength.

Predict the direction in which the equilibrium will lie for the reaction H2CO3 + F- HCO3- + HF.Ka1( H2CO3)= 4.2 × 10-7; Ka(HF)= 7.1 × 10-4

HCN is classified as a weak acid in water.What does this classification mean?

Calculate the concentration of chromate ion (CrO42-)in a 0.450 M solution of chromic acid (H2CrO4).[For chromic acid, Ka1 = 0.18, Ka2 = 3.2 × 10-7.]

The hydrolysis of NH4F will result in which of the following types of solutions given: (Ka(NH4+)= 5.6 x 10-10, Kb(F-)= 1.4 x 10-11)

The OH- concentration in a 2.5 × 10-3 M Ba(OH)2 solution is

Which one of the following salts will form an acidic solution on dissolving in water?

Which one of the following equations represents the ionization of a weak monoprotic acid in water?

Al(OH)3 is an amphoteric hydroxide.Write a balanced ionic equation to show its reaction with HNO3.

Given the following Ka values, which anion is the strongest base?

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The compound CH₃NH₂ reacts with water to form CH₃NH₃⁺ and OH^-.What role does CH₃NH₂ play in this reaction?

Calculate the pH of a 0.025 M solution of NaNO₂ (K_a(HNO₂)= 4.5 x 10^-4)

Identify the conjugate base of HPO₄^2-

What mass of ammonium chloride must be added to 250.mL of water to give a solution with pH = 4.85? [K_b(NH₃)= 1.8 × 10^-5]

A 0.14 M HNO₂ solution is 5.7% ionized.Calculate the H⁺ ion concentration.

Arrange the acids H₂Se, H₂Te, and H₂S in order of increasing acid strength.

Predict the direction in which the equilibrium will lie for the reaction H₂CO₃ + F^- HCO₃^- + HF.K_a1(H₂CO₃)= 4.2 × 10^-7; K_a(HF)= 7.1 × 10^-4

Calculate the concentration of chromate ion (CrO₄^2-)in a 0.450 M solution of chromic acid (H₂CrO₄).[For chromic acid, K_a1 = 0.18, K_a2 = 3.2 × 10^-7.]

The hydrolysis of NH₄F will result in which of the following types of solutions given: (K_a(NH₄⁺)= 5.6 x 10^-10, K_b(F^-)= 1.4 x 10^-11)

The OH^- concentration in a 2.5 × 10^-3 M Ba(OH)₂ solution is

Al(OH)₃ is an amphoteric hydroxide.Write a balanced ionic equation to show its reaction with HNO₃.

Given the following K_a values, which anion is the strongest base?