Question 1

Order the following acids in order of increasing strength: HBrO HBrO3 HBrO4 HBrO2

Accepted Answer

A)  HBrO 3 4 2 
B)  HBrO4 3 2 3 2 4 
D)  HBrO 2 3 4 
E)  HBrO2 4 2 
A)  HBrO 3 4 2 
B)  HBrO4 3 2 3 2 4 
D)  HBrO 2 3 4 
E)  HBrO2 4 2

Question 2

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 3

What is the hydroxide ion concentration of a lye solution that has a pH of 9.20?

Accepted Answer

A)  6.3 × 10-10 mol L-1 
B)  1.6 × 10-5 mol L-1 
C)  4.8 mol L-1 
D)  9.2 mol L-1 
A)  6.3 × 10-10 mol L-1 
B)  1.6 × 10-5 mol L-1 
C)  4.8 mol L-1 
D)  9.2 mol L-1

Question 4

Calculate the pH of a 0. 60 mol L-1 H2SO3 solution that has the stepwise dissociation constants Ka1 = 1.5 × 10-2 and  Ka2=6.3 x 10-8

Accepted Answer

A)  1.02 
B)  1.06 
C)  1.82 
D)  2.04 
A)  1.02 
B)  1.06 
C)  1.82 
D)  2.04

Question 5

Find the percent ionization of a 0.265 mol L-1 HClO solution. The Ka of HClO is 2.9 × 10-8.

Accepted Answer

A)  0.0331% 
B)  0.0551% 
C)  1.12% 
D)  3.65% 
E)  3.32% 
A)  0.0331% 
B)  0.0551% 
C)  1.12% 
D)  3.65% 
E)  3.32%

Question 6

Find the percent ionization of a 0.400 mol L-1 solution of formic acid. The Ka of formic acid is 1.8 × 10-4.

Accepted Answer

A)  3.4% 
B)  2.1% 
C)  1.1% 
D)  3.5% 
E)  4.6% 
A)  3.4% 
B)  2.1% 
C)  1.1% 
D)  3.5% 
E)  4.6%

Question 7

Describe the relationship between molecular structure and acid strength.

Accepted Answer

1. The stronger the bond between a hydro

Question 8

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 9

Determine the pH of a 0.461 mol L-1 C6H5CO2H solution if the Ka of C6H5CO2H is 6.5 × 10-5.

Accepted Answer

A)  2.26 
B)  4.52 
C)  11.74 
D)  9.48 
E)  5.48 
A)  2.26 
B)  4.52 
C)  11.74 
D)  9.48 
E)  5.48

Question 10

Match the following.
-Lewis acid

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

What is the pH of a 0.30 mol L-1 pyridine solution that has Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is below: C5H5N(aq)+H2O(l) ⇌ C5H5NH+(aq)+OH-(aq)

Accepted Answer

A)  4. 62 
B)  8.72 
C)  9. 38 
D)  10. 38 
A)  4. 62 
B)  8.72 
C)  9. 38 
D)  10. 38

Question 12

Calculate the pH of a solution that contains 7.8 × 10-6 mol L-1 OH⁻ at 25 °C.

Accepted Answer

A)  1.28 
B)  5.11 
C)  12.72 
D)  8.89 
E)  9.64 
A)  1.28 
B)  5.11 
C)  12.72 
D)  8.89 
E)  9.64

Question 13

Identify the monoprotic acid.

Accepted Answer

A)  H2CO3 
B)  NH3 
C)  H3PO4 
D)  H2SO4 
E)  HBr 
A)  H2CO3 
B)  NH3 
C)  H3PO4 
D)  H2SO4 
E)  HBr

Question 14

Calculate the pH of a 0. 080 mol L-1 carbonic acid solution, H2CO3(aq), that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A)  1.10 
B)  3.73 
C)  6.37 
D)  10.25 
A)  1.10 
B)  3.73 
C)  6.37 
D)  10.25

Question 15

What is the difference between a strong and weak acid?

Accepted Answer

A strong acid ionizes/dissocia

Question 16

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of  1.50 x 10-2 mol L-1

Accepted Answer

A)  6.67 × 10-12 mol L-1, 2.82 
B)  6.67 × 10-12 mol L-1, 11.18 
C)  6.67 × 10-13 mol L-1, 1.82 
D)  6.67 × 10-13 mol L-1, 12.17 
A)  6.67 × 10-12 mol L-1, 2.82 
B)  6.67 × 10-12 mol L-1, 11.18 
C)  6.67 × 10-13 mol L-1, 1.82 
D)  6.67 × 10-13 mol L-1, 12.17

Exam 15: Acids and Bases

Order the following acids in order of increasing strength: HBrO HBrO3 HBrO4 HBrO2

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

What is the hydroxide ion concentration of a lye solution that has a pH of 9.20?

Calculate the pH of a 0. 60 mol L-1 H2SO3 solution that has the stepwise dissociation constants Ka1 = 1.5 × 10-2 and Ka2=6.3 x 10-8

Find the percent ionization of a 0.265 mol L-1 HClO solution. The Ka of HClO is 2.9 × 10-8.

Find the percent ionization of a 0.400 mol L-1 solution of formic acid. The Ka of formic acid is 1.8 × 10-4.

Describe the relationship between molecular structure and acid strength.

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

Determine the pH of a 0.461 mol L-1 C6H5CO2H solution if the Ka of C6H5CO2H is 6.5 × 10-5.

Match the following. -Lewis acid

What is the pH of a 0.30 mol L-1 pyridine solution that has Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is below: C5H5N(aq)+H2O(l) ⇌ C5H5NH+(aq)+OH-(aq)

Calculate the pH of a solution that contains 7.8 × 10-6 mol L-1 OH⁻ at 25 °C.

Identify the monoprotic acid.

Calculate the pH of a 0. 080 mol L-1 carbonic acid solution, H2CO3(aq), that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

What is the difference between a strong and weak acid?

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 x 10-2 mol L-1

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Filters

Order the following acids in order of increasing strength: HBrO HBrO₃ HBrO₄ HBrO₂

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

Calculate the pH of a 0. 60 mol L^-1 H₂SO₃ solution that has the stepwise dissociation constants K_a1 = 1.5 × 10^-2 and K_a2=6.3 x 10-8

Find the percent ionization of a 0.265 mol L^-1 HClO solution. The K_a of HClO is 2.9 × 10^-8.

Find the percent ionization of a 0.400 mol L^-1 solution of formic acid. The K_a of formic acid is 1.8 × 10^-4.

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

Determine the pH of a 0.461 mol L^-1 C₆H₅CO₂H solution if the K_a of C₆H₅CO₂H is 6.5 × 10^-5.

What is the pH of a 0.30 mol L^-1 pyridine solution that has K_b = 1.9 × 10^-9? The equation for the dissociation of pyridine is below: C₅H₅N(aq)+H₂O(l) ⇌ C₅H₅NH+(aq)+OH-(aq)

Calculate the pH of a solution that contains 7.8 × 10^-6 mol L^-1 OH⁻ at 25 °C.

Calculate the pH of a 0. 080 mol L^-1 carbonic acid solution, H₂CO₃₍_aq_),that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 x 10^-2 mol L^-1