Question 1

The pOH of a solution is 10.40. Calculate the hydrogen ion concentration in the solution.

Accepted Answer

A)   4.0 * 10-11 M
B)   3.6 M
C)   4.0 * 10-10 M
D)   2.5 * 10-4 M
E)   1.8 * 10-4 M

Question 2

What is the pH of a 0.20 M solution of NH4Cl? [Kb(NH3)  = 1.8 * 10-5]

Accepted Answer

A)   3.74
B)   4.98
C)   6.53
D)   9.02
E)   10.25

Question 3

Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH of 2.87.

Accepted Answer

A)   2.9 * 10-2 M
B)   5.7 * 10-2 M
C)   1.3 * 10-3 M
D)   2.9 * 10-3 M
E)   5.7 * 10-4 M

Question 4

Which of the following solutions is acidic

Accepted Answer

A)   [H3O+] = 7.0 x 10-7 M
B)   [H3O+] = 1.5 x 10-10 M
C)   [H3O+] -7 M
D)   [H3O+] > 7.0 x 10-7 M
E)   [H3O+] = 1.0 x 10-14 M

Question 5

Which of the following solutions is basic

Accepted Answer

A)   [OH-] = 1.0 x 10-14 M
B)   [OH-] = 1.0 x 10-7 M
C)   [H3O+] = 1.0 x 10-14 M
D)   [H3O+] > 1.0 x 10-7 M
E)   [OH-] -7 M

Question 6

Calculate the H+ ion concentration in lemon juice having a pH of 2.40.

Accepted Answer

A)   4.0 * 10-2 M
B)   250 M
C)   0.38 M
D)   4.0 * 10-3 M
E)   12 M

Question 7

When comparing acid strength of binary acids HX, as X varies within a particular group of the periodic table, which one of these factors dominates in affecting the acid strength

Accepted Answer

A)   bond strength
B)   electron withdrawing effects
C)   percent ionic character of the H-X bond
D)   solubility
E)   Le Châtelier's principle

Question 8

Kw = 1.0 x 10S1U1P1-14S1S1P0at all temperatures.

Accepted Answer

A) True 
 B)False

Question 9

Identify the conjugate base of HSO4-.

Accepted Answer

A)   OH-
B)   H2SO4
C)   H2O
D)   H2SO3
E)   SO42-

Question 10

Aspartic acid (C4H7NO4) , one of the 20 essential amino acids, has two ionizable hydrogens. At 25 ∘\circ∘ C, Ka1 = 1.38 * 10-4 and Ka2 = 1.51 * 10-10. What is the concentration of doubly ionized aspartate ions in a 0.125 M aqueous solution of aspartic acid

Accepted Answer

A)   3.33 * 10-2 M
B)   4.16 * 10-3 M
C)   4.15 * 10-3 M
D)   1.51 * 10-10 M
E)   2.08 * 10-14 M

Question 11

The formula for the conjugate base of HPO42- is H2PO4-.

Accepted Answer

A) True 
 B)False

Question 12

HCN is classified as a weak acid in water. This classification means that a relatively small fraction of the acid undergoes ionization.

Accepted Answer

A) True 
 B)False

Question 13

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

Question 14

What is the pH of a 0.30 M solution of HOCl (Ka = 3.5 x 10-8)

Accepted Answer

A)   7.45
B)   6.54
C)   7.98
D)   5.22
E)   3.99

Question 15

What is the concentration of H+ in a 2.5 M HCl solution

Accepted Answer

A)   0
B)   1.3 M
C)   2.5 M
D)   5.0 M
E)   10. M

Question 16

When 2.0 * 10-2 mole of nicotinic acid (a monoprotic acid)  is dissolved in 350. mL of water, the pH is 3.05. What is the Ka of nicotinic acid

Accepted Answer

A)   1.0 * 10-5
B)   1.2 * 10-5
C)   1.4 * 10-5
D)   1.6 * 10-5
E)   None of the above

Question 17

The equilibrium constant for the reaction C6H5COOH(aq)  + CH3COO-(aq)   ⇋\leftrightharpoons⇋  C6H5COO-(aq)  + CH3COOH(aq) 
Is 3.6 at 25 ∘\circ∘ C. If Ka for CH3COOH is 1.8 * 10-5, what is the acid dissociation constant for C6H5COOH

Accepted Answer

A)   5.0 * 10-6
B)   6.5 * 10-5
C)   2.3 * 10-4
D)   8.3 * 10-5
E)   5.6 * 10-6

Question 18

Which of the following solutions is basic

Accepted Answer

A)   [H3O+] = 1.0 x 10-10 M
B)   [OH-] = 1.0 x 10-10 M
C)   [H3O+] > 1.0 x 10-7 M
D)   [OH-] -10 M
E)   [OH-] = 1.0 x 10-7 M

Question 19

The pH of a 0.6 M solution of a weak acid is 4.0. What percent of the acid has ionized

Accepted Answer

A)   0.01 %
B)   0.02 %
C)   0.03 %
D)   0.04 %
E)   None of the above

Question 20

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

Exam 15: Acids and Bases

The pOH of a solution is 10.40. Calculate the hydrogen ion concentration in the solution.

Correct AnswerverifiedShow Answer

What is the pH of a 0.30 M solution of HOCl (Ka = 3.5 x 10-8)

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HCN is classified as a weak acid in water. This classification means that a relatively small fraction of the acid undergoes ionization.

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Calculate the H+ ion concentration in lemon juice having a pH of 2.40.

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The formula for the conjugate base of HPO42- is H2PO4-.

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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]

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The pH of a 0.6 M solution of a weak acid is 4.0. What percent of the acid has ionized

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Identify the conjugate base of HSO4-.

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Aspartic acid (C4H7NO4) , one of the 20 essential amino acids, has two ionizable hydrogens. At 25 ∘\circ∘ C, Ka1 = 1.38 * 10-4 and Ka2 = 1.51 * 10-10. What is the concentration of doubly ionized aspartate ions in a 0.125 M aqueous solution of aspartic acid

Correct AnswerverifiedShow Answer

What is the concentration of H+ in a 2.5 M HCl solution

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What is the pH of a 0.20 M solution of NH4Cl? [Kb(NH3) = 1.8 * 10-5]

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When comparing acid strength of binary acids HX, as X varies within a particular group of the periodic table, which one of these factors dominates in affecting the acid strength

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Which of the following solutions is acidic

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When 2.0 * 10-2 mole of nicotinic acid (a monoprotic acid) is dissolved in 350. mL of water, the pH is 3.05. What is the Ka of nicotinic acid

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Which of the following solutions is basic

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Which of the following solutions is basic

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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.]

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Kw = 1.0 x 10-14at all temperatures.

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The equilibrium constant for the reaction C6H5COOH(aq) + CH3COO-(aq) ⇋\leftrightharpoons⇋ C6H5COO-(aq) + CH3COOH(aq) Is 3.6 at 25 ∘\circ∘ C. If Ka for CH3COOH is 1.8 * 10-5, what is the acid dissociation constant for C6H5COOH

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Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH of 2.87.

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Correct Answer
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What is the pH of a 0.30 M solution of HOCl (K_a = 3.5 x 10^-8)

Correct Answer
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Correct Answer
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Calculate the H⁺ ion concentration in lemon juice having a pH of 2.40.

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The formula for the conjugate base of HPO₄^2- is H₂PO₄^-.

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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]

Correct Answer
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Correct Answer
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Identify the conjugate base of HSO₄^-.

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Aspartic acid (C₄H₇NO₄) , one of the 20 essential amino acids, has two ionizable hydrogens. At 25^$\circ$C, K_a1 = 1.38 * 10^-4 and K_a2 = 1.51 * 10^-10. What is the concentration of doubly ionized aspartate ions in a 0.125 M aqueous solution of aspartic acid

Correct Answer
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What is the concentration of H⁺ in a 2.5 M HCl solution

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What is the pH of a 0.20 M solution of NH₄Cl? [K_b(NH₃) = 1.8 * 10^-5]

Correct Answer
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Correct Answer
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Correct Answer
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When 2.0 * 10^-2 mole of nicotinic acid (a monoprotic acid) is dissolved in 350. mL of water, the pH is 3.05. What is the K_a of nicotinic acid

Correct Answer
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Correct Answer
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Correct Answer
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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.]

Correct Answer
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K_w = 1.0 x 10^-14at all temperatures.

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The equilibrium constant for the reaction C₆H₅COOH(aq) + CH₃COO^-(aq) $\leftrightharpoons$ C₆H₅COO^-(aq) + CH₃COOH(aq) Is 3.6 at 25^$\circ$C. If K_a for CH₃COOH is 1.8 * 10^-5, what is the acid dissociation constant for C₆H₅COOH

Correct Answer
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Correct Answer
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