Question 1

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-. 
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-.

Question 2

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. 
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.

Question 3

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

Question 4

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) 
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 5

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

Question 6

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)  12.65 
A)  1.35 
B)  2.35 
C)  7.00 
D)  11.65 
E)  12.65

Question 7

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 8

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)  3.46 
A)  -2.46 
B)  0.54 
C)  2.46 
D)  3.00 
E)  3.46

Question 9

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)  1.17 
A)  12.83 
B)  2.17 
C)  11.82 
D)  6.71 
E)  1.17

Question 10

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 11

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)  9.91 
A)  5.70 
B)  8.30 
C)  2.05 
D)  11.95 
E)  9.91

Question 12

Identify the conjugate acid of SO42-.

Accepted Answer

A)  H2SO4 
B)  HSO4- 
C)  H2SO3 
D)  H3O+ 
E)  SO32- 
A)  H2SO4 
B)  HSO4- 
C)  H2SO3 
D)  H3O+ 
E)  SO32-

Question 13

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$_4^+$(aq) + H$_2$O(l) 
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$_4^+$(aq) + H$_2$O(l)

Question 14

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 M 
A)  0.84 M 
B)  0.12 M 
C)  0.10 M 
D)  0.084 M 
E)  8.4 * 10-3 M

Question 15

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. M 
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. M

Question 16

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+ 
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+

Question 17

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

Accepted Answer

A) True 
 B)False

Question 18

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

Accepted Answer

A) True 
 B)False

Question 19

Identify the conjugate acid of HCO3-.

Accepted Answer

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

Question 20

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

Exam 15: Acids and Bases

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

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

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

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

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

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.

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

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

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

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

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

Identify the conjugate acid of SO42-.

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

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

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

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

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

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

Identify the conjugate acid of HCO3-.

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

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

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

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.

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

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

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

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

Identify the conjugate acid of SO₄^2-.

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

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

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

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

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

Identify the conjugate acid of HCO₃^-.

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