Chapter 16 Problems

A 0.110 M solution of a weak acid, represented as HA, has a pH of 4.35. Calculate the value of Ka for HA.

1.81 x 10^-8

Calculate the pH of 0.180 M NH3; Kb = 1.8 × 10−5.

11.3

Calculate the pH of 0.290 M NH4Cl. See Appendix A.3 for K values as needed.

11.4

Rank the acid strength of HClO, HClO2, and HBrO from weakest to strongest.

HBrO>HClO>HClO2

Use the following structure of formic acid to explain why it is monoprotic instead of diprotic.

Monoprotic - one ionizable hydrogen atom

Calculate [H3O+] and pH for a 0.317 M solution of HF; Ka = 6.8 × 10−4.

[H3O^+] = 0.0147 pH = 1.83

At some temperature other than 25°C, Kw = 1.14 × 10−14. What are the concentrations of [H3O^+] and [OH^−] in pure water at this temperature?

[H3O^+] and [OH^-] = 1.07 x 10^-7

Estimate the ascorbate ion concentration in 0.200 M ascorbic acid (vitamin C) solution. See Table 16.3 for Ka values.

[HC6H6O6^-] = .004 M

Determine [OH−] at 25°C for an aqueous solution with a) [H3O^+] = 4.68 × 10^−11 M. b) [H3O^+] = 3.15 × 10^−3 M. c) [H3O^+] = 6.05 × 10^−4 M.

a) 2.14 x 10^-4 b) 3.17 x 10^-12 c) 1.65 x 10^-11

Calculate the pH of each of the following solutions. a) 0.0010 M HCl b) 0.025 M NaOH c) 0.33 M Sr(OH)2

a) 3 b) 12.4 c) 13.5

Calculate the pOH of a solution having each of the following hydroxide ion concentrations. a) 6.2 × 10^−4 M b) 9.93 × 10^−8 M c) 4.55 × 10^−12 M

a) 3.2 b) 7.00 C) 11.3

Write the ionization reaction for each of these bases. a) Ba(OH)2 b) NH3

a) Ba(OH)2 + H2O --> Ba^2+ + 2OH^- b) NH3 + H2O --> NH4^+ + OH^-

Classify each solution in problem 23 as acidic, basic, or neutral. (The problems above)

a) Basic b) Acidic c) Acidic

Classify each species in each reaction as a Brønsted acid or Brønsted base, and identify the conjugate pairs. a) HCN(aq) + H2O(l) ⇌ CN^−(aq) + H3O^+(aq) b) NH4^+(aq) + OH^−(aq) ⇌ NH3(aq) + H2O(l)

a) Bronsted acid: HCN, conjugate base: CN^- Bronsted base: H2O, conjugate acid: H3O^+ b) Bronsted acid: NH4^+, conjugate base: NH3 Bronsted base: OH^-, conjugate acid: H2O

Oxalic acid, H2C2O4, is diprotic. a) Write the two ionization reactions for oxalic acid. b) Write the Ka1 and Ka2 expressions for oxalic acid.

a) H2C2O4 + H2O --> HC2O4^- + H2O^+ HC2O4^- + H2O --> C2O4^2- + H3O^+ b) idk

Write the formula for the conjugate acid of each of the following. a) CO3^2- b) ClO2^- c) NO3^- d) BrO^-

a) HCO3^- b) HClO2 c) HNO3 d) HBrO

Write the ionization reaction for each of these acids. a) HClO4 b) HClO2

a) HClO4 + H2O--> ClO4^- + H^+ b) HClO2 + H2O --> H^+ + ClO2^-

Which of the following 0.100 M solutions are acidic, which are basic, and which are neutral? a) BaCl2 b) NH4Br c) K2CO3 d) NH4NO3 e) CaSO3 f) LiNO3

a) Neutral b) Acidic c) Basic d) Acidic e) Basic f) Neutral

Classify the following solutions as acidic, basic, or neutral at 25°C. a) pH = 7.00 b) [H3O^+] = 1.0 × 10^−12 M c) pOH = 5.00 d) [OH^−] = 1.0 × 10^−9 M

a) Neutral b) Basic c) Basic d) Acidic