Question 1

What does the term amphoteric mean?

Accepted Answer

A substance is ampho

Question 2

Match the following.

-Bronsted-Lowry acid

Accepted Answer

A) proton donor 
B) electron pair acceptor 
C) proton acceptor 
D) electron pair donor 
E) produces protons in aqueous solution
F)produces hydroxide ions in aqueous solution 
A) proton donor 
B) electron pair acceptor 
C) proton acceptor 
D) electron pair donor 
E) produces protons in aqueous solution
F)produces hydroxide ions in aqueous solution

Question 3

What is the selenide ion concentration [Se2-] for a 0.100 mol L-1 H2Se solution that has the stepwise dissociation constants of Ka1 = 1.3 × 10-4 and Ka2 = 1.0 × 10-11?

Accepted Answer

A) 3.6 × 10-3 mol L-1 
B) 1.3 × 10-4 mol L-1 
C) 1.3 × 10-5 mol L-1 
D) 1.0 × 10-11 mol L-1 
A) 3.6 × 10-3 mol L-1 
B) 1.3 × 10-4 mol L-1 
C) 1.3 × 10-5 mol L-1 
D) 1.0 × 10-11 mol L-1

Question 4

Determine the Ka for CH3NH3⁺ at 25 °C. The Kb for CH3NH2 is 4.4 × 10-4.

Accepted Answer

A) 3.1 × 10-10 
B) 6.8 × 10-11 
C) 5.6 × 10-10 
D) 2.3 × 10-3 
E) 2.3 × 10-11 
A) 3.1 × 10-10 
B) 6.8 × 10-11 
C) 5.6 × 10-10 
D) 2.3 × 10-3 
E) 2.3 × 10-11

Question 5

Which of the following is correct?

Accepted Answer

A) According to the Bronsted-Lowry theory, an acid is a proton donor while a base is a proton acceptor. 
B) According to the Bronsted-Lowry theory, an acid is a proton acceptor while a base is a proton donor. 
C) According to the Bronsted-Lowry theory, an acid is a proton donor while a base is a hydroxide ion acceptor. 
D) According to the Bronsted-Lowry theory, an acid is a hydroxide donor while a base is a proton acceptor. 
E) According to the Bronsted-Lowry theory, an acid is a hydroxide donor while a base is a hydroxide acceptor. 
A) According to the Bronsted-Lowry theory, an acid is a proton donor while a base is a proton acceptor. 
B) According to the Bronsted-Lowry theory, an acid is a proton acceptor while a base is a proton donor. 
C) According to the Bronsted-Lowry theory, an acid is a proton donor while a base is a hydroxide ion acceptor. 
D) According to the Bronsted-Lowry theory, an acid is a hydroxide donor while a base is a proton acceptor. 
E) According to the Bronsted-Lowry theory, an acid is a hydroxide donor while a base is a hydroxide acceptor.

Question 6

Determine the pH of a 0.188 mol L-1 NH3 solution at 25 °C. The Kb of NH3 is 1.76 × 10-5.

Accepted Answer

A) 5.480 
B) 2.740 
C) 8.520 
D) 11.260 
E) 12.656 
A) 5.480 
B) 2.740 
C) 8.520 
D) 11.260 
E) 12.656

Question 7

Identify the Lewis acid, Lewis base, and Lewis acid-base adduct in the following equation: (C2H5)2O + BF3 ⇌ (C2H5)2O:BF3

Accepted Answer

A) (C2H5)2O is a Lewis base, BF3 is a Lewis acid, and (C2H5)2O:BF3 is a Lewis acid-base adduct. 
B) (C2H5)2O is a Lewis acid, BF3 is a Lewis base, and (C2H5)2O:BF3 is a Lewis acid-base adduct. 
C) (C2H5)2O is a Lewis acid-base adduct, BF3 is a Lewis acid, and (C2H5)2O:BF3 is a Lewis base. 
D) (C2H5)2O is a Lewis base, BF3 is a Lewis acid-base adduct, and (C2H5)2O:BF3 is a Lewis acid adduct. 
E) (C2H5)2O and BF3 are both Lewis acid-base adducts and (C2H5)2O:BF3 is a Lewis acid. 
A) (C2H5)2O is a Lewis base, BF3 is a Lewis acid, and (C2H5)2O:BF3 is a Lewis acid-base adduct. 
B) (C2H5)2O is a Lewis acid, BF3 is a Lewis base, and (C2H5)2O:BF3 is a Lewis acid-base adduct. 
C) (C2H5)2O is a Lewis acid-base adduct, BF3 is a Lewis acid, and (C2H5)2O:BF3 is a Lewis base. 
D) (C2H5)2O is a Lewis base, BF3 is a Lewis acid-base adduct, and (C2H5)2O:BF3 is a Lewis acid adduct. 
E) (C2H5)2O and BF3 are both Lewis acid-base adducts and (C2H5)2O:BF3 is a Lewis acid.

Question 8

Which of the following bases is the strongest? The base is followed by its Kb.

Accepted Answer

A) (CH3CH2)2NH, 8.6 × 10-4 
B) CH3NH2, 4.4 × 10-4 
C) C6H5NH2, 4.0 × 10-10 
D) NH3, 1.76 × 10-5 
E) C5H5N, 1.7 × 10-9 
A) (CH3CH2)2NH, 8.6 × 10-4 
B) CH3NH2, 4.4 × 10-4 
C) C6H5NH2, 4.0 × 10-10 
D) NH3, 1.76 × 10-5 
E) C5H5N, 1.7 × 10-9

Question 9

The acid-dissociation constant at 25.0 °C for hypochlorous acid (HClO)is 3.0 × 10-8. At equilibrium, the molarity of H3O+ in a 0.010 mol L-1 solution of HClO is ________.

Accepted Answer

A) 1.7 × 10-5 
B) 0.010 
C) 5.8 × 10-10 
D) 4.76 
E) 2.00 
A) 1.7 × 10-5 
B) 0.010 
C) 5.8 × 10-10 
D) 4.76 
E) 2.00

Question 10

Determine the pH of a 0.00598 mol L-1 HClO4 solution.

Accepted Answer

A) 1.777 
B) 6.434 
C) 7.566 
D) 2.223 
E) 3.558 
A) 1.777 
B) 6.434 
C) 7.566 
D) 2.223 
E) 3.558

Question 11

Which of the following equilibria represents the second ionization step of H3PO4?

Accepted Answer

A) H3PO4(aq)+ H2O(l)⇌ H2PO4-(aq)+ H3O+(aq) 
B) H3PO4(aq)+ 2H2O(l)⇌ HPO42-(aq)+ 2H3O+(aq) 
C) H2PO4-(aq)+ H2O(l)⇌ HPO42-(aq)+ H3O+(aq) 
D) HPO42-(aq)+ H2O(aq)⇌ PO43-(aq)+ H3O+(aq) 
E) H3PO4(aq)+ 3H2O(l)⇌ PO43-(aq)+ 3H3O+(aq) 
A) H3PO4(aq)+ H2O(l)⇌ H2PO4-(aq)+ H3O+(aq) 
B) H3PO4(aq)+ 2H2O(l)⇌ HPO42-(aq)+ 2H3O+(aq) 
C) H2PO4-(aq)+ H2O(l)⇌ HPO42-(aq)+ H3O+(aq) 
D) HPO42-(aq)+ H2O(aq)⇌ PO43-(aq)+ H3O+(aq) 
E) H3PO4(aq)+ 3H2O(l)⇌ PO43-(aq)+ 3H3O+(aq)

Question 12

Determine the [OH⁻] concentration in a 0.169 mol L-1 Ca(OH)2 solution.

Accepted Answer

A) 0.338 mol L-1 
B) 0.169 mol L-1 
C) 5.92 × 10-14 mol L-1 
D) 2.96 × 10-14 mol L-1 
E) 0.298 mol L-1 
A) 0.338 mol L-1 
B) 0.169 mol L-1 
C) 5.92 × 10-14 mol L-1 
D) 2.96 × 10-14 mol L-1 
E) 0.298 mol L-1

Question 13

Calculate the pH of a 1.60 mol L-1 KBrO solution. Ka for hypobromous acid, HBrO, is 2.0 × 10-9.

Accepted Answer

A) 2.55 
B) 4.25 
C) 9.75 
D) 11.45 
A) 2.55 
B) 4.25 
C) 9.75 
D) 11.45

Question 14

Determine the [OH-] concentration of a 0.116 mol L-1 Ba(OH)2 solution at 25 °C.

Accepted Answer

A) 4.310 × 10-14 mol L-1 
B) 0.116 mol L-1 
C) 0.232 mol L-1 
D) 8.62 × 10-14 mol L-1 
E) 0.058 mol L-1 
A) 4.310 × 10-14 mol L-1 
B) 0.116 mol L-1 
C) 0.232 mol L-1 
D) 8.62 × 10-14 mol L-1 
E) 0.058 mol L-1

Question 15

A 7.0 × 10-3 mol L-1 aqueous solution of Ca(OH)2 at 25.0 °C has a pH of ________.

Accepted Answer

A) 12.15 
B) 1.85 
C) 1.4 × 10-2 
D) 7.1 × 10-13 
E) 11.85 
A) 12.15 
B) 1.85 
C) 1.4 × 10-2 
D) 7.1 × 10-13 
E) 11.85

Question 16

What is the hydronium ion concentration of a 0.500 mol L-1 acetic acid solution with Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is below:

Accepted Answer

A) 3.0 × 10-2 mol L-1 
B) 4.2 × 10-2 mol L-1 
C) 3.0 × 10-3 mol L-1 
D) 4.2 × 10-3 mol L-1 
A) 3.0 × 10-2 mol L-1 
B) 4.2 × 10-2 mol L-1 
C) 3.0 × 10-3 mol L-1 
D) 4.2 × 10-3 mol L-1

Question 17

Calculate the pH for an aqueous solution of acetic acid that contains 2.15 × 10-3 mol L-1 hydronium ion.

Accepted Answer

A) 4.65 × 10-12  
B) 2.15 × 10-3  
C) 2.67 
D) 11.33 
A) 4.65 × 10-12  
B) 2.15 × 10-3  
C) 2.67 
D) 11.33

Question 18

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 4.33 at 25 °C.

Accepted Answer

A) 2.1 × 10-10 mol L-1 
B) 9.7 × 10-10 mol L-1 
C) 4.7 × 10-5 mol L-1 
D) 3.8 × 10-5 mol L-1 
E) 6.3 × 10-6 mol L-1 
A) 2.1 × 10-10 mol L-1 
B) 9.7 × 10-10 mol L-1 
C) 4.7 × 10-5 mol L-1 
D) 3.8 × 10-5 mol L-1 
E) 6.3 × 10-6 mol L-1

Question 19

Which one of the following will form a basic solution in water?

Accepted Answer

A) NaBr 
B) LiCN 
C) KClO2 
D) KClO4 
E) NH4Cl 
A) NaBr 
B) LiCN 
C) KClO2 
D) KClO4 
E) NH4Cl

Question 20

Describe a molecule that can be a Lewis acid.

Accepted Answer

A molecule with an i

Exam 15: Acids and Bases

What does the term amphoteric mean?

Match the following. -Bronsted-Lowry acid

What is the selenide ion concentration [Se2-] for a 0.100 mol L-1 H2Se solution that has the stepwise dissociation constants of Ka1 = 1.3 × 10-4 and Ka2 = 1.0 × 10-11?

Determine the Ka for CH3NH3⁺ at 25 °C. The Kb for CH3NH2 is 4.4 × 10-4.

Which of the following is correct?

Determine the pH of a 0.188 mol L-1 NH3 solution at 25 °C. The Kb of NH3 is 1.76 × 10-5.

Identify the Lewis acid, Lewis base, and Lewis acid-base adduct in the following equation: (C2H5)2O + BF3 ⇌ (C2H5)2O:BF3

Which of the following bases is the strongest? The base is followed by its Kb.

The acid-dissociation constant at 25.0 °C for hypochlorous acid (HClO)is 3.0 × 10-8. At equilibrium, the molarity of H3O+ in a 0.010 mol L-1 solution of HClO is ________.

Determine the pH of a 0.00598 mol L-1 HClO4 solution.

Which of the following equilibria represents the second ionization step of H3PO4?

Determine the [OH⁻] concentration in a 0.169 mol L-1 Ca(OH)2 solution.

Calculate the pH of a 1.60 mol L-1 KBrO solution. Ka for hypobromous acid, HBrO, is 2.0 × 10-9.

Determine the [OH-] concentration of a 0.116 mol L-1 Ba(OH)2 solution at 25 °C.

A 7.0 × 10-3 mol L-1 aqueous solution of Ca(OH)2 at 25.0 °C has a pH of ________.

What is the hydronium ion concentration of a 0.500 mol L-1 acetic acid solution with Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is below:

Calculate the pH for an aqueous solution of acetic acid that contains 2.15 × 10-3 mol L-1 hydronium ion.

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 4.33 at 25 °C.

Which one of the following will form a basic solution in water?

Describe a molecule that can be a Lewis acid.

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Filters

What is the selenide ion concentration [Se^2-] for a 0.100 mol L^-1 H₂Se solution that has the stepwise dissociation constants of K_a1 = 1.3 × 10^-4 and K_a2 = 1.0 × 10^-11?

Determine the K_a for CH₃NH₃⁺ at 25 °C. The K_b for CH₃NH₂ is 4.4 × 10^-4.

Determine the pH of a 0.188 mol L^-1 NH₃ solution at 25 °C. The K_bof NH₃ is 1.76 × 10^-5.

Identify the Lewis acid, Lewis base, and Lewis acid-base adduct in the following equation: (C₂H₅)₂O + BF₃ ⇌ (C₂H₅)₂O:BF₃

Which of the following bases is the strongest? The base is followed by its K_b.

The acid-dissociation constant at 25.0 °C for hypochlorous acid (HClO)is 3.0 × 10^-8. At equilibrium, the molarity of H₃O⁺ in a 0.010 mol L^-1 solution of HClO is ________.

Determine the pH of a 0.00598 mol L^-1 HClO₄ solution.

Which of the following equilibria represents the second ionization step of H₃PO₄?

Determine the [OH⁻] concentration in a 0.169 mol L^-1 Ca(OH)₂ solution.

Calculate the pH of a 1.60 mol L^-1 KBrO solution. K_a for hypobromous acid, HBrO, is 2.0 × 10^-9.

Determine the [OH^-] concentration of a 0.116 mol L^-1 Ba(OH)₂ solution at 25 °C.

A 7.0 × 10^-3 mol L^-1 aqueous solution of Ca(OH)₂ at 25.0 °C has a pH of ________.

What is the hydronium ion concentration of a 0.500 mol L^-1 acetic acid solution with K_a = 1.8 × 10^-5? The equation for the dissociation of acetic acid is below:

Calculate the pH for an aqueous solution of acetic acid that contains 2.15 × 10^-3 mol L^-1 hydronium ion.