Question 1

H2SO4 is a stronger acid than HSO4-.

Accepted Answer

A) True 
 B)False

Question 2

If the pH of tomato juice is 4.0, what is the hydroxide ion concentration in this solution

Accepted Answer

A)  4 * 10-10 M 
B)  3 * 10-10 M 
C)  2 * 10-10 M 
D)  1 * 10-10 M 
E)  None of the above 
A)  4 * 10-10 M 
B)  3 * 10-10 M 
C)  2 * 10-10 M 
D)  1 * 10-10 M 
E)  None of the above

Question 3

Calculate the pH of a 1.6 M KOH solution.

Accepted Answer

A)  1.60 
B)  -0.20 
C)  0.20 
D)  14.20 
E)  13.80 
A)  1.60 
B)  -0.20 
C)  0.20 
D)  14.20 
E)  13.80

Question 4

Calculate the pOH for a solution with [H3O+] = 2.5 x 10-5 M

Accepted Answer

A)  4.60 
B)  9.40 
C)  4.0 x 10-10 
D)  2.50 
E)  11.50 
A)  4.60 
B)  9.40 
C)  4.0 x 10-10 
D)  2.50 
E)  11.50

Question 5

What is the pH of a 0.023 M solution of HCN (Ka = 4.9 x 10-10)

Accepted Answer

A)  1.64 
B)  10.95 
C)  3.05 
D)  5.47 
E)  4.97 
A)  1.64 
B)  10.95 
C)  3.05 
D)  5.47 
E)  4.97

Question 6

What is the OH- ion concentration in a 5.2 * 10-4 M HNO3 solution

Accepted Answer

A)  1.9 * 10-11 M 
B)  1.0 * 10-7 M 
C)  5.2 * 10-4 M 
D)  0 
E)  1.0 * 10-4 M 
A)  1.9 * 10-11 M 
B)  1.0 * 10-7 M 
C)  5.2 * 10-4 M 
D)  0 
E)  1.0 * 10-4 M

Question 7

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 8

Calculate the pH of a 0.15 M solution of HOI. (Ka = 2.3 x 10-11)

Accepted Answer

A)  5.73 
B)  5.53 
C)  5.33 
D)  5.13 
E)  None of the above 
A)  5.73 
B)  5.53 
C)  5.33 
D)  5.13 
E)  None of the above

Question 9

The pH of coffee is approximately 5.0. How many times greater is the [H+] in coffee than in neutral water

Accepted Answer

A)  200 
B)  100 
C)  5.0 
D)  1.4 
E)  0.01 
A)  200 
B)  100 
C)  5.0 
D)  1.4 
E)  0.01

Question 10

What mass of sodium nitrite must be added to 350. mL of water to give a solution with pH = 8.40? [Ka(HNO2) = 5.6 * 10-4]

Accepted Answer

A)  68 g 
B)  1.7 * 10-4 g 
C)  0.039 g 
D)  8.3 g 
E)  24 g 
A)  68 g 
B)  1.7 * 10-4 g 
C)  0.039 g 
D)  8.3 g 
E)  24 g

Question 11

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 12

Consider the weak acid CH3COOH (acetic acid). If a 0.048 M CH3COOH solution is 5.2% ionized, determine the [H3O+] concentration at equilibrium.

Accepted Answer

A)  0.25 M 
B)  9.2 * 10-3 M 
C)  0.048 M 
D)  0.052 M 
E)  2.5 * 10-3 M 
A)  0.25 M 
B)  9.2 * 10-3 M 
C)  0.048 M 
D)  0.052 M 
E)  2.5 * 10-3 M

Question 13

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 14

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 15

A 0.1 M solution of NH4NO2(aq) will be acidic.

Accepted Answer

A) True 
 B)False

Question 16

Al(OH)3 is an amphoteric hydroxide. The balanced ionic equation for its reaction with HNO3 is: Al(OH)3 + 3HNO3 $\rarr$Al(NO3)3 + 3H2O

Accepted Answer

A) True 
 B)False

Question 17

The salt hydrolysis reaction for CH3COONa that represents the acidic or basic nature of the solution is:

Accepted Answer

A)  Na+(aq) + H2O(l) $\leftrightharpoons$ NaH(s) + OH-(aq) 
B)  CH3COO-(aq) + H2O(l) $\leftrightharpoons$ CH2COO2-(aq) + H3O+(aq) 
C)  CH3COO-(aq) + H2O(l) $\leftrightharpoons$ CH3COOH(aq) + OH-(aq) 
D)  Na2O(s) + H2O(l) $\leftrightharpoons$ 2NaOH(aq) 
E)  CH3COO-(aq) + Na+(aq) $\leftrightharpoons$ CH$_3$COONa 
A)  Na+(aq) + H2O(l) $\leftrightharpoons$ NaH(s) + OH-(aq) 
B)  CH3COO-(aq) + H2O(l) $\leftrightharpoons$ CH2COO2-(aq) + H3O+(aq) 
C)  CH3COO-(aq) + H2O(l) $\leftrightharpoons$ CH3COOH(aq) + OH-(aq) 
D)  Na2O(s) + H2O(l) $\leftrightharpoons$ 2NaOH(aq) 
E)  CH3COO-(aq) + Na+(aq) $\leftrightharpoons$ CH$_3$COONa

Question 18

Arrange the acids HOBr, HBrO3, and HBrO2 in order of increasing acid strength.

Accepted Answer

A)  HOBr 3 2 
B)  HOBr 2 3 
C)  HBrO2 3 
D)  HBrO3 2 
E)  HBrO3 2 < HOBr 
A)  HOBr 3 2 
B)  HOBr 2 3 
C)  HBrO2 3 
D)  HBrO3 2 
E)  HBrO3 2 < HOBr

Question 19

For maleic acid, HOOCCH=CHCOOH, Ka1 = 1.42 * 10-2 and Ka2 = 8.57 * 10-7.What is the concentration of maleate ion (-OOCCH=CHCOO-) in a 0.150 M aqueous solution of maleic acid

Accepted Answer

A)  8.57 * 10-7 M 
B)  2.79 * 10-6 M 
C)  1.86 * 10-5 M 
D)  4.60 * 10-2 M 
E)  1.19 * 10-1 M 
A)  8.57 * 10-7 M 
B)  2.79 * 10-6 M 
C)  1.86 * 10-5 M 
D)  4.60 * 10-2 M 
E)  1.19 * 10-1 M

Question 20

The formula for the conjugate base of H2PO4- is PO43-.

Accepted Answer

A) True 
 B)False

Exam 15: Acids and Bases

H2SO4 is a stronger acid than HSO4-.

If the pH of tomato juice is 4.0, what is the hydroxide ion concentration in this solution

Calculate the pH of a 1.6 M KOH solution.

Calculate the pOH for a solution with [H3O+] = 2.5 x 10-5 M

What is the pH of a 0.023 M solution of HCN (Ka = 4.9 x 10-10)

What is the OH- ion concentration in a 5.2 * 10-4 M HNO3 solution

What is the pH of 10.0 mL of 0.0020 M HCl

Calculate the pH of a 0.15 M solution of HOI. (Ka = 2.3 x 10-11)

The pH of coffee is approximately 5.0. How many times greater is the [H+] in coffee than in neutral water

What mass of sodium nitrite must be added to 350. mL of water to give a solution with pH = 8.40? [Ka(HNO2) = 5.6 * 10-4]

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)

Consider the weak acid CH3COOH (acetic acid). If a 0.048 M CH3COOH solution is 5.2% ionized, determine the [H3O+] concentration at equilibrium.

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

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

A 0.1 M solution of NH4NO2(aq) will be acidic.

Al(OH)3 is an amphoteric hydroxide. The balanced ionic equation for its reaction with HNO3 is: Al(OH)3 + 3HNO3 →\rarr→ Al(NO3)3 + 3H2O

The salt hydrolysis reaction for CH3COONa that represents the acidic or basic nature of the solution is:

Arrange the acids HOBr, HBrO3, and HBrO2 in order of increasing acid strength.

For maleic acid, HOOCCH=CHCOOH, Ka1 = 1.42 * 10-2 and Ka2 = 8.57 * 10-7.What is the concentration of maleate ion (-OOCCH=CHCOO-) in a 0.150 M aqueous solution of maleic acid

The formula for the conjugate base of H2PO4- is PO43-.

Chemistry: The Study of Change

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Filters

H₂SO₄ is a stronger acid than HSO₄^-.

Calculate the pOH for a solution with [H₃O⁺] = 2.5 x 10^-5 M

What is the pH of a 0.023 M solution of HCN (K_a = 4.9 x 10^-10)

What is the OH^- ion concentration in a 5.2 * 10^-4 M HNO₃ solution

Calculate the pH of a 0.15 M solution of HOI. (K_a = 2.3 x 10^-11)

The pH of coffee is approximately 5.0. How many times greater is the [H⁺] in coffee than in neutral water

What mass of sodium nitrite must be added to 350. mL of water to give a solution with pH = 8.40? [K_a(HNO₂) = 5.6 * 10^-4]

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)

Consider the weak acid CH₃COOH (acetic acid). If a 0.048 M CH₃COOH solution is 5.2% ionized, determine the [H₃O⁺] concentration at equilibrium.

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

A 0.1 M solution of NH₄NO₂(aq) will be acidic.

Al(OH)₃ is an amphoteric hydroxide. The balanced ionic equation for its reaction with HNO₃ is: Al(OH)₃ + 3HNO₃ $\rarr$ Al(NO₃)₃ + 3H₂O

The salt hydrolysis reaction for CH₃COONa that represents the acidic or basic nature of the solution is:

Arrange the acids HOBr, HBrO₃, and HBrO₂ in order of increasing acid strength.

For maleic acid, HOOCCH=CHCOOH, K_a1 = 1.42 * 10^-2 and K_a2 = 8.57 * 10^-7.What is the concentration of maleate ion (^-OOCCH=CHCOO^-) in a 0.150 M aqueous solution of maleic acid

The formula for the conjugate base of H₂PO₄^- is PO₄^3-.