Question 1

If the pH of seawater is 8.0, what is the hydroxide ion concentration in seawater

Accepted Answer

A)  1 * 10-5 M 
B)  1 * 10-6 M 
C)  1 * 10-7 M 
D)  1 * 10-8 M 
E)  None of the above 
A)  1 * 10-5 M 
B)  1 * 10-6 M 
C)  1 * 10-7 M 
D)  1 * 10-8 M 
E)  None of the above

Question 2

Consider the weak bases below and their Kb values: $\begin{array}{ll}
\mathrm{C}_{6} \mathrm{H}_{7} \mathrm{O} & \mathrm{~K}_{\mathrm{b}}=1.3 \times 10^{-10} \
\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{2} & \mathrm{~K}_{\mathrm{b}}=5.6 \times 10^{-4} \
\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N} & \mathrm{~K}_{\mathrm{b}}=1.7 \times 10^{-9}
\end{array}$ Arrange the conjugate acids of these weak bases in order of increasing acid strength.

Accepted Answer

A)  C5H5NH+ 6H7OH 2H5NH 
B)  C6H7OH 5H5NH+ 2H5NH 
C)  C5H5NH+ 2H5NH3+ 6H7OH 
D)  C6H7OH 2H5NH3+5H5NH+ 
E)  C2H5NH3+5H5NH+ 6H7OH 
A)  C5H5NH+ 6H7OH 2H5NH 
B)  C6H7OH 5H5NH+ 2H5NH 
C)  C5H5NH+ 2H5NH3+ 6H7OH 
D)  C6H7OH 2H5NH3+5H5NH+ 
E)  C2H5NH3+5H5NH+ 6H7OH

Question 3

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 4

What is the pH of a 0.0055 M HA (weak acid) solution that is 8.2% ionized

Accepted Answer

A)  2.26 
B)  3.35 
C)  4.52 
D)  8.21 
E)  10.65 
A)  2.26 
B)  3.35 
C)  4.52 
D)  8.21 
E)  10.65

Question 5

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

Accepted Answer

A)  BF3 
B)  NH3 
C)  CO2 
D)  HNO2 
E)  PCl3 
A)  BF3 
B)  NH3 
C)  CO2 
D)  HNO2 
E)  PCl3

Question 6

A 5.2 L sample of a 1.1 M KOH solution is mixed with 2.3 L of a 0.20 M Sc(OH)3 solution. What is the pH of the mixture

Accepted Answer

A)  13.67 
B)  13.89 
C)  14.11 
D)  14.23 
E)  13.98 
A)  13.67 
B)  13.89 
C)  14.11 
D)  14.23 
E)  13.98

Question 7

Identify the conjugate acid of CO32-.

Accepted Answer

A)  H2CO3 
B)  HCO3- 
C)  H2O 
D)  H3O+ 
E)  CO2 
A)  H2CO3 
B)  HCO3- 
C)  H2O 
D)  H3O+ 
E)  CO2

Question 8

What is the pH of a solution prepared by mixing 100. mL of 0.0500 M HCl with 300. mL of 0.500 M HF? [Ka(HF) = 7.1 * 10-4]

Accepted Answer

A)  1.47 
B)  1.90 
C)  1.30 
D)  1.63 
E)  2.82 
A)  1.47 
B)  1.90 
C)  1.30 
D)  1.63 
E)  2.82

Question 9

Which solution will have the lowest pH

Accepted Answer

A)  0.25 M HClO 
B)  0.25 M HClO2 
C)  0.25 M HClO3 
D)  0.25 M HClO4 
E)  0.25 M NaClO4 
A)  0.25 M HClO 
B)  0.25 M HClO2 
C)  0.25 M HClO3 
D)  0.25 M HClO4 
E)  0.25 M NaClO4

Question 10

The pH of tomato juice is about 4.5. Calculate the concentration of hydrogen ions in this juice.

Accepted Answer

A)  3 * 10-10 M 
B)  3 * 10-5 M 
C)  5 * 10-4 M 
D)  4 M 
E)  3 * 1010 M 
A)  3 * 10-10 M 
B)  3 * 10-5 M 
C)  5 * 10-4 M 
D)  4 M 
E)  3 * 1010 M

Question 11

For H3PO4, Ka1 = 7.3 * 10-3, Ka2 = 6.2 * 10-6, and Ka3 = 4.8 * 10-13. An aqueous solution of NaH2PO4 therefore would be

Accepted Answer

A)  neutral. 
B)  basic. 
C)  acidic. 
A)  neutral. 
B)  basic. 
C)  acidic.

Question 12

Calculate the pH of a 0.055 M solution of CH3COONa. (Ka(CH3COOH) = 1.8 x 10-5)

Accepted Answer

A)  12.74 
B)  4.74 
C)  8.74 
D)  9.26 
E)  5.26 
A)  12.74 
B)  4.74 
C)  8.74 
D)  9.26 
E)  5.26

Question 13

Calculate the pH of a 0.10 M HCN solution that is 0.0070% ionized.

Accepted Answer

A)  1.00 
B)  0.00070 
C)  3.15 
D)  5.15 
E)  7.00 
A)  1.00 
B)  0.00070 
C)  3.15 
D)  5.15 
E)  7.00

Question 14

In the reaction HNO3 + NH3 $\leftrightharpoons$ NH4+ + NO3-, NH4+ and NH3 are a conjugate acid-base pair.

Accepted Answer

A) True 
 B)False

Question 15

Calculate the pH of a 0.14 M HNO2 solution that is 5.7% ionized.

Accepted Answer

A)  0.85 
B)  1.70 
C)  2.10 
D)  11.90 
E)  13.10 
A)  0.85 
B)  1.70 
C)  2.10 
D)  11.90 
E)  13.10

Question 16

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

Accepted Answer

A)  HNO2(aq) + OH- (aq) $\leftrightharpoons$ H2O(l) + NO2-(aq) 
B)  HNO2(aq) + NH3(aq) $\leftrightharpoons$ NH4NO2(aq) 
C)  HNO2(aq) + H2O(l) $\leftrightharpoons$ H3O+(aq) + NO2-(aq) 
D)  HNO3(aq) + OH-(aq) $\leftrightharpoons$ H2O(l) + NO3-(aq) 
E)  NO2- (aq) + H2O(aq) $\leftrightharpoons$ HNO$_2$(aq) + OH$^-$(aq) 
A)  HNO2(aq) + OH- (aq) $\leftrightharpoons$ H2O(l) + NO2-(aq) 
B)  HNO2(aq) + NH3(aq) $\leftrightharpoons$ NH4NO2(aq) 
C)  HNO2(aq) + H2O(l) $\leftrightharpoons$ H3O+(aq) + NO2-(aq) 
D)  HNO3(aq) + OH-(aq) $\leftrightharpoons$ H2O(l) + NO3-(aq) 
E)  NO2- (aq) + H2O(aq) $\leftrightharpoons$ HNO$_2$(aq) + OH$^-$(aq)

Question 17

Which one of these net ionic equations represents the reaction of a strong acid with a strong base

Accepted Answer

A) H+(aq) + OH-(aq) $\rarr$ H2O(aq) 
B) H+(aq) + CH3NH2(aq) $\rarr$CH3NH3+(aq) 
C) OH-(aq) + HCN(aq) $\rarr$ H2O(aq) + CN-(aq) 
D) HCN(aq) + CH3NH2(aq) $\rarr$ CH3NH3+(aq) + CN-(aq) 
A) H+(aq) + OH-(aq) $\rarr$ H2O(aq) 
B) H+(aq) + CH3NH2(aq) $\rarr$CH3NH3+(aq) 
C) OH-(aq) + HCN(aq) $\rarr$ H2O(aq) + CN-(aq) 
D) HCN(aq) + CH3NH2(aq) $\rarr$ CH3NH3+(aq) + CN-(aq)

Question 18

When carbon dioxide dissolves in rain water carbonic acid forms which raises the pH of rain water above 7.

Accepted Answer

A) True 
 B)False

Question 19

Calculate the pH of a solution containing 0.20 g of NaOH in 2,000. mL of solution.

Accepted Answer

A)  9.40 
B)  10.40 
C)  11.40 
D)  12.40 
E)  None of the above 
A)  9.40 
B)  10.40 
C)  11.40 
D)  12.40 
E)  None of the above

Question 20

What is the pH of a 0.15 M solution of the weak base aniline (C6H5NH2; Kb = 3.8 x 10-10)

Accepted Answer

A)  5.12 
B)  8.88 
C)  13.18 
D)  9.42 
E)  10.24 
A)  5.12 
B)  8.88 
C)  13.18 
D)  9.42 
E)  10.24

Exam 15: Acids and Bases

If the pH of seawater is 8.0, what is the hydroxide ion concentration in seawater

Consider the weak bases below and their Kb values: =1.3\times1 =5.6\times1 =1.7\times1 Arrange the conjugate acids of these weak bases in order of increasing acid strength.

Which solution will have the lowest pH

What is the pH of a 0.0055 M HA (weak acid) solution that is 8.2% ionized

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

A 5.2 L sample of a 1.1 M KOH solution is mixed with 2.3 L of a 0.20 M Sc(OH)3 solution. What is the pH of the mixture

Identify the conjugate acid of CO32-.

What is the pH of a solution prepared by mixing 100. mL of 0.0500 M HCl with 300. mL of 0.500 M HF? [Ka(HF) = 7.1 * 10-4]

Which solution will have the lowest pH

The pH of tomato juice is about 4.5. Calculate the concentration of hydrogen ions in this juice.

For H3PO4, Ka1 = 7.3 * 10-3, Ka2 = 6.2 * 10-6, and Ka3 = 4.8 * 10-13. An aqueous solution of NaH2PO4 therefore would be

Calculate the pH of a 0.055 M solution of CH3COONa. (Ka(CH3COOH) = 1.8 x 10-5)

Calculate the pH of a 0.10 M HCN solution that is 0.0070% ionized.

In the reaction HNO3 + NH3 ⇋\leftrightharpoons⇋ NH4+ + NO3-, NH4+ and NH3 are a conjugate acid-base pair.

Calculate the pH of a 0.14 M HNO2 solution that is 5.7% ionized.

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

Which one of these net ionic equations represents the reaction of a strong acid with a strong base

When carbon dioxide dissolves in rain water carbonic acid forms which raises the pH of rain water above 7.

Calculate the pH of a solution containing 0.20 g of NaOH in 2,000. mL of solution.

What is the pH of a 0.15 M solution of the weak base aniline (C6H5NH2; Kb = 3.8 x 10-10)

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Consider the weak bases below and their K_b values: =1.3\times1 =5.6\times1 =1.7\times1 Arrange the conjugate acids of these weak bases in order of increasing acid strength.

A 5.2 L sample of a 1.1 M KOH solution is mixed with 2.3 L of a 0.20 M Sc(OH)₃ solution. What is the pH of the mixture

Identify the conjugate acid of CO₃^2-.

What is the pH of a solution prepared by mixing 100. mL of 0.0500 M HCl with 300. mL of 0.500 M HF? [K_a(HF) = 7.1 * 10^-4]

For H₃PO₄, K_a1 = 7.3 * 10^-3, K_a2 = 6.2 * 10^-6, and K_a3 = 4.8 * 10^-13. An aqueous solution of NaH₂PO₄ therefore would be

Calculate the pH of a 0.055 M solution of CH₃COONa. (K_a(CH₃COOH) = 1.8 x 10^-5)

In the reaction HNO₃ + NH₃ $\leftrightharpoons$ NH₄⁺ + NO₃^-, NH₄⁺ and NH₃ are a conjugate acid-base pair.

Calculate the pH of a 0.14 M HNO₂ solution that is 5.7% ionized.

What is the pH of a 0.15 M solution of the weak base aniline (C₆H₅NH₂; K_b = 3.8 x 10^-10)