Question 1

Determine the [H3O⁺] in a 0.265 mol L-1 HClO solution. The Ka of HClO is 2.9 × 10-8.

Accepted Answer

A)  1.1 × 10-10 mol L-1 
B)  7.7 × 10-9 mol L-1 
C)  1.3 × 10-6 mol L-1 
D)  4.9 × 10-4 mol L-1 
E)  8.8 × 10-5 mol L-1 
A)  1.1 × 10-10 mol L-1 
B)  7.7 × 10-9 mol L-1 
C)  1.3 × 10-6 mol L-1 
D)  4.9 × 10-4 mol L-1 
E)  8.8 × 10-5 mol L-1

Question 2

Which of the following is a general property of an acid?

Accepted Answer

A)  Acids have sour taste. 
B)  Acids are not able to dissolve metals. 
C)  Acids turn red litmus paper blue. 
D)  Acids leave blue litmus paper unchanged. 
E)  All acids are dense liquids. 
A)  Acids have sour taste. 
B)  Acids are not able to dissolve metals. 
C)  Acids turn red litmus paper blue. 
D)  Acids leave blue litmus paper unchanged. 
E)  All acids are dense liquids.

Question 3

Calculate the pH for an aqueous solution of acetic acid that contains  2.15 x10-3 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 4

Match the following.
-Bronsted-Lowry base

Accepted Answer

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

Question 5

What is the concentration of hydroxide ions in pure water at 30.0 °C if Kw at this temperature is 1.47 × 10-14?

Accepted Answer

A)  1.00 × 10-7 mol L-1 
B)  1.30 × 10-7 mol L-1 
C)  1.47 × 10-7 mol L-1 
D)  8.93 × 10-8 mol L-1 
E)  1.21 × 10-7 mol L-1 
A)  1.00 × 10-7 mol L-1 
B)  1.30 × 10-7 mol L-1 
C)  1.47 × 10-7 mol L-1 
D)  8.93 × 10-8 mol L-1 
E)  1.21 × 10-7 mol L-1

Question 6

Which one of the following will form an acidic solution in water?

Accepted Answer

A)  NH4Cl 
B)  NaF 
C)  LiI 
D)  KNO3 
E)  NaCH3COO 
A)  NH4Cl 
B)  NaF 
C)  LiI 
D)  KNO3 
E)  NaCH3COO

Question 7

Which of the following acids is the strongest? The acid is followed by its Ka value.

Accepted Answer

A)  HF, 3.5 × 10-4 
B)  HCN, 4.9 × 10-10 
C)  HNO2, 4.6 × 10-4 
D)  HCHO2, 1.8 × 10-4 
E)  HClO2, 1.1 × 10-2 
A)  HF, 3.5 × 10-4 
B)  HCN, 4.9 × 10-10 
C)  HNO2, 4.6 × 10-4 
D)  HCHO2, 1.8 × 10-4 
E)  HClO2, 1.1 × 10-2

Question 8

Determine the Kb for CN⁻ at 25 °C. The Ka for HCN is 4.9 × 10-10.

Accepted Answer

A)  4.9 × 10-14 
B)  2.3 × 10-9 
C)  1.4 × 10-5 
D)  2.0 × 10-5 
E)  3.7 × 10-7 
A)  4.9 × 10-14 
B)  2.3 × 10-9 
C)  1.4 × 10-5 
D)  2.0 × 10-5 
E)  3.7 × 10-7

Question 9

Which of the following acids is the weakest? The acid is followed by its Ka value.

Accepted Answer

A)  CH3COOH, 1.8 × 10-5 
B)  HIO, 2.3 × 10-11 
C)  HBrO, 2.3 × 10-9 
D)  HClO, 2.9 × 10-8 
E)  C6H5COOH, 6.3 × 10-5 
A)  CH3COOH, 1.8 × 10-5 
B)  HIO, 2.3 × 10-11 
C)  HBrO, 2.3 × 10-9 
D)  HClO, 2.9 × 10-8 
E)  C6H5COOH, 6.3 × 10-5

Question 10

Match the following.
-Lewis base

Accepted Answer

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

Question 11

Determine the pOH in a 0.235 mol L-1 NaOH solution.

Accepted Answer

A)  13.76 
B)  0.24 
C)  13.37 
D)  0.63 
E)  12 
A)  13.76 
B)  0.24 
C)  13.37 
D)  0.63 
E)  12

Question 12

What is the pH of a 0. 500 mol L-1 NH3 solution that has Kb = 1.8 × 10-5? The equation for the dissociation of NH3 is below: NH3(aq)+H2O(l) ⇌NH4+(aq)+OH-(aq)

Accepted Answer

A)  2.22 
B)  2. 52 
C)  11. 48 
D)  10.48 
A)  2.22 
B)  2. 52 
C)  11. 48 
D)  10.48

Question 13

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 14

Determine the pH of a 0.741 mol L-1 KOH solution at 25 °C.

Accepted Answer

A)  0.13 
B)  13.87 
C)  0.17 
D)  12.65 
E)  11.88 
A)  0.13 
B)  13.87 
C)  0.17 
D)  12.65 
E)  11.88

Question 15

Calculate the pH of a 1.60 mol L-1 KBrO solution. Ka for hypobromous acid, HBrO, is  2.0 x10-9

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 16

Do both protons ionize instantaneously from a diprotic acid such as H2CO3? Explain your answer.

Accepted Answer

No. Polyprotic acids ionize in stages. A

Question 17

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 3.00.

Accepted Answer

A)  11.00 mol L-1 
B)  1.00 × 10-11 mol L-1 
C)  1.00 × 10-3 mol L-1 
D)  3.00 × 10-14 mol L-1 
E)  1.1 × 10-13 mol L-1 
A)  11.00 mol L-1 
B)  1.00 × 10-11 mol L-1 
C)  1.00 × 10-3 mol L-1 
D)  3.00 × 10-14 mol L-1 
E)  1.1 × 10-13 mol L-1

Question 18

Which of the following is the acid found in our stomachs?

Accepted Answer

A)  H2SO4 
B)  HI 
C)  HCl 
D)  HF 
E)  HBr 
A)  H2SO4 
B)  HI 
C)  HCl 
D)  HF 
E)  HBr

Question 19

Determine the pH of a 0.22 mol L-1 NaF solution at 25 °C. The Ka of HF is 3.5 × 10-5.

Accepted Answer

A)  10.20 
B)  5.10 
C)  8.90 
D)  11.44 
E)  2.56 
A)  10.20 
B)  5.10 
C)  8.90 
D)  11.44 
E)  2.56

Question 20

An aqueous solution at 25.0 °C contains [ H+] = 0.085 mol L-1. What is the pH of the solution?

Accepted Answer

A)  1.07 
B)  -1.07 
C)  13.0 
D)  0.0850 
E)  1.20 ×  10-13 
A)  1.07 
B)  -1.07 
C)  13.0 
D)  0.0850 
E)  1.20 ×  10-13

Exam 15: Acids and Bases

Determine the [H3O⁺] in a 0.265 mol L-1 HClO solution. The Ka of HClO is 2.9 × 10-8.

Which of the following is a general property of an acid?

Calculate the pH for an aqueous solution of acetic acid that contains 2.15 x10-3 mol L-1 hydronium ion.

Match the following. -Bronsted-Lowry base

What is the concentration of hydroxide ions in pure water at 30.0 °C if Kw at this temperature is 1.47 × 10-14?

Which one of the following will form an acidic solution in water?

Which of the following acids is the strongest? The acid is followed by its Ka value.

Determine the Kb for CN⁻ at 25 °C. The Ka for HCN is 4.9 × 10-10.

Which of the following acids is the weakest? The acid is followed by its Ka value.

Match the following. -Lewis base

Determine the pOH in a 0.235 mol L-1 NaOH solution.

What is the pH of a 0. 500 mol L-1 NH3 solution that has Kb = 1.8 × 10-5? The equation for the dissociation of NH3 is below: NH3(aq)+H2O(l) ⇌NH4+(aq)+OH-(aq)

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

Determine the pH of a 0.741 mol L-1 KOH solution at 25 °C.

Calculate the pH of a 1.60 mol L-1 KBrO solution. Ka for hypobromous acid, HBrO, is 2.0 x10-9

Do both protons ionize instantaneously from a diprotic acid such as H2CO3? Explain your answer.

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 3.00.

Which of the following is the acid found in our stomachs?

Determine the pH of a 0.22 mol L-1 NaF solution at 25 °C. The Ka of HF is 3.5 × 10-5.

An aqueous solution at 25.0 °C contains [ H+] = 0.085 mol L-1. What is the pH of the solution?

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Filters

Determine the [H₃O⁺] in a 0.265 mol L^-1 HClO solution. The K_a of HClO is 2.9 × 10^-8.

Calculate the pH for an aqueous solution of acetic acid that contains 2.15 x10^-3 mol L^-1 hydronium ion.

What is the concentration of hydroxide ions in pure water at 30.0 °C if K_w at this temperature is 1.47 × 10^-14?

Which of the following acids is the strongest? The acid is followed by its K_a value.

Determine the K_b for CN⁻ at 25 °C. The K_a for HCN is 4.9 × 10^-10.

Which of the following acids is the weakest? The acid is followed by its K_a value.

Determine the pOH in a 0.235 mol L^-1 NaOH solution.

What is the pH of a 0. 500 mol L^-1 NH₃ solution that has K_b = 1.8 × 10^-5? The equation for the dissociation of NH₃ is below: NH₃(aq)+H₂O(l) ⇌NH₄+(aq)+OH-(aq)

Determine the pH of a 0.741 mol L^-1 KOH solution at 25 °C.

Calculate the pH of a 1.60 mol L^-1 KBrO solution. K_a for hypobromous acid, HBrO, is 2.0 x10^-9

Do both protons ionize instantaneously from a diprotic acid such as H₂CO₃? Explain your answer.

Determine the pH of a 0.22 mol L^-1 NaF solution at 25 °C. The K_a of HF is 3.5 × 10^-5.

An aqueous solution at 25.0 °C contains [ H+] = 0.085 mol L^-1. What is the pH of the solution?