Question 1

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)   NaCNF) B) and E)
G) B) and D)

Question 2

The formula for the conjugate acid of H2PO4- is H3PO4.

Accepted Answer

A) True 
 B)False

Question 3

If the pH of pure water is 7.0, the hydroxide ion concentration in pure water is 1 * 10-7 M.

Accepted Answer

A) True 
 B)False

Question 4

The pH of a Ba(OH) 2 solution is 10.00. What is the H+ ion concentration of this solution

Accepted Answer

A)   4.0 * 10-11 M
B)   1.6 * 10-10 M
C)   1.3 * 10-5 M
D)   1.0 * 10-10 M
E)   10. MF) B) and E)
G) B) and C)

Question 5

The hydronium ion and the hydroxide ion, in that order, are:

Accepted Answer

A)   H3O+, OH+
B)   OH-, H3O-
C)   OH-, H+
D)   H3O+, OH-
E)   H3O-, OH-F) B) and C)
G) C) and D)

Question 6

In the reaction: CH3COOH(aq)  + NH2- (aq)   ⇋\leftrightharpoons⇋  CH3COO- (aq)  + NH3(aq) , the conjugate acid-base pairs are:

Accepted Answer

A)   pair 1: CH3COOH and CH3COO- ; pair 2: NH2- and NH3
B)   pair 1: CH3COOH and NH3; pair 2: NH2- and CH3COO-
C)   pair 1: CH3COOH and NH2- ; pair 2: NH3 and CH3OO-
D)   pair 1: CH3COOH and CH3COO- ; pair 2: NH4+ and NH3
E)   pair 1: CH3COOH and CH3COO- ; pair 2: NH2- and NH3+ F) C) and D)
G) None of the above

Question 7

The OH- concentration in a 7.5 * 10-3 M Ca(OH) 2 solution is

Accepted Answer

A)   7.5 * 10-3 M.
B)   1.5 * 10-2 M.
C)   1.3 * 10-12 M.
D)   1.0 * 10-7 M.
E)   1.0 * 10-14 M.F) A) and D)
G) All of the above

Question 8

Identify the conjugate acid of HCO3-.

Accepted Answer

A)   H2O
B)   CO32-
C)   H2CO3
D)   CO2
E)   H3O+F) C) and D)
G) B) and C)

Question 9

Determine the pH of a KOH solution made by mixing 0.251 g KOH with enough water to make 1.0 * 102 mL of solution.

Accepted Answer

A)   1.35
B)   2.35
C)   7.00
D)   11.65
E)   12.65F) A) and B)
G) A) and C)

Question 10

Calculate the pH of a 3.5 * 10-3 M HNO3 solution.

Accepted Answer

A)   -2.46
B)   0.54
C)   2.46
D)   3.00
E)   3.46F) A) and B)
G) All of the above

Question 11

Predict the direction in which the equilibrium will lie for the reaction H2SO3(aq)  + HCO3- (aq)   ⇋\leftrightharpoons⇋  HSO3-(aq)  + H2CO3(aq) .Ka1(H2SO3)  = 1* 10-2; Ka1(H2CO3)  = 4.2 * 10-7

Accepted Answer

A)   to the right
B)   to the left
C)   in the middle D) None of the above
E) A) and C)

Question 12

Calculate the pH of a 6.7 * 10-2 M NaOH solution.

Accepted Answer

A)   12.83
B)   2.17
C)   11.82
D)   6.71
E)   1.17F) A) and B)
G) B) and C)

Question 13

Which one of the following statements is true for a 0.1 M solution of a weak acid HA

Accepted Answer

A)   The concentration of H+ is slightly greater than the concentration of A-.
B)   The pH equals 1.0.
C)   The concentration of H+ is exactly equal to the concentration of A-.
D)   The pH is less than 1.0.
E)   The concentration of H+ is slightly less than the concentration of A-.F) None of the above
G) C) and D)

Question 14

Identify the conjugate acid of SO42-.

Accepted Answer

A)   H2SO4
B)   HSO4-
C)   H2SO3
D)   H3O+
E)   SO32-F) A) and B)
G) All of the above

Question 15

In aqueous solutions at 25$\circ$C, the sum of the ion concentrations ([H+] + [OH -]) equals 1 * 10 - 14.

Accepted Answer

A) True 
 B)False

Question 16

A 0.10 M HF solution is 8.4% ionized. Calculate the H+ ion concentration.

Accepted Answer

A)   0.84 M
B)   0.12 M
C)   0.10 M
D)   0.084 M
E)   8.4 * 10-3 MF) None of the above
G) D) and E)

Question 17

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

Accepted Answer

A)   NH3(aq)  + H2O(l)   ⇋\leftrightharpoons⇋  NH2+(aq)  + H3O+(aq) 
B)   NH3(aq)  + H2O(l)   ⇋\leftrightharpoons⇋  NH4+(aq)  + OH-(aq) 
C)   NH3(aq)  + H2O(l)   ⇋\leftrightharpoons⇋  NH4- (aq)  + OH+(aq) 
D)   NH3(aq)  + OH-(aq)   ⇋\leftrightharpoons⇋  NH2- (aq)  + H2O(l) 
E)   NH3(aq)  + H3O+(aq)   ⇋\leftrightharpoons⇋  NH 4+_4^+4+​ (aq)  + H 2_22​ O(l)  F) C) and D)
G) B) and D)

Question 18

Of the two acids HBr and H2Se, H2Se is the stronger acid.

Accepted Answer

A) True 
 B)False

Question 19

Which one of these equations represents the reaction of a weak 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)  E) C) and D)
F) None of the above

Question 20

Calculate the pH of a 0.18 M solution of KNO2. (Ka (HNO2)  = 4.5 x 10-4)

Accepted Answer

A)   5.70
B)   8.30
C)   2.05
D)   11.95
E)   9.91F) None of the above
G) B) and E)

Exam 15: Acids and Bases

The pH of a Ba(OH) 2 solution is 10.00. What is the H+ ion concentration of this solution

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In aqueous solutions at 25 ∘\circ∘ C, the sum of the ion concentrations ([H+] + [OH -]) equals 1 * 10 - 14.

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Determine the pH of a KOH solution made by mixing 0.251 g KOH with enough water to make 1.0 * 102 mL of solution.

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If the pH of pure water is 7.0, the hydroxide ion concentration in pure water is 1 * 10-7 M.

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

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Calculate the pH of a 6.7 * 10-2 M NaOH solution.

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

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Of the two acids HBr and H2Se, H2Se is the stronger acid.

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Calculate the pH of a 0.18 M solution of KNO2. (Ka (HNO2) = 4.5 x 10-4)

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

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A 0.10 M HF solution is 8.4% ionized. Calculate the H+ ion concentration.

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Which one of the following statements is true for a 0.1 M solution of a weak acid HA

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Calculate the pH of a 3.5 * 10-3 M HNO3 solution.

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Predict the direction in which the equilibrium will lie for the reaction H2SO3(aq) + HCO3- (aq) ⇋\leftrightharpoons⇋ HSO3-(aq) + H2CO3(aq) .Ka1(H2SO3) = 1* 10-2; Ka1(H2CO3) = 4.2 * 10-7

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The formula for the conjugate acid of H2PO4- is H3PO4.

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The hydronium ion and the hydroxide ion, in that order, are:

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Identify the conjugate acid of HCO3-.

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In the reaction: CH3COOH(aq) + NH2- (aq) ⇋\leftrightharpoons⇋ CH3COO- (aq) + NH3(aq) , the conjugate acid-base pairs are:

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The OH- concentration in a 7.5 * 10-3 M Ca(OH) 2 solution is

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Identify the conjugate acid of SO42-.

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The pH of a Ba(OH) ₂ solution is 10.00. What is the H⁺ ion concentration of this solution

Correct Answer
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In aqueous solutions at 25^$\circ$C, the sum of the ion concentrations ([H⁺] + [OH ^-]) equals 1 * 10 ^{- 14}.

Correct Answer
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Determine the pH of a KOH solution made by mixing 0.251 g KOH with enough water to make 1.0 * 10² mL of solution.

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If the pH of pure water is 7.0, the hydroxide ion concentration in pure water is 1 * 10^-7 M.

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Calculate the pH of a 6.7 * 10^-2 M NaOH solution.

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Of the two acids HBr and H₂Se, H₂Se is the stronger acid.

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Calculate the pH of a 0.18 M solution of KNO₂. (K_a (HNO₂) = 4.5 x 10^-4)

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A 0.10 M HF solution is 8.4% ionized. Calculate the H⁺ ion concentration.

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Calculate the pH of a 3.5 * 10^-3 M HNO₃ solution.

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Predict the direction in which the equilibrium will lie for the reaction H₂SO₃(aq) + HCO₃^- (aq) $\leftrightharpoons$ HSO₃^-(aq) + H₂CO₃(aq) .K_a1(H₂SO₃) = 1* 10^-2; K_a1(H₂CO₃) = 4.2 * 10^-7

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The formula for the conjugate acid of H₂PO₄^- is H₃PO_4.

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Identify the conjugate acid of HCO₃^-.

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In the reaction: CH₃COOH(aq) + NH₂^- (aq) $\leftrightharpoons$ CH₃COO^- (aq) + NH₃(aq) , the conjugate acid-base pairs are:

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The OH^- concentration in a 7.5 * 10^-3 M Ca(OH) ₂ solution is

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Identify the conjugate acid of SO₄^2-.

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