Ch.17 - Acids and Bases

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Tro 6th Edition

Ch.17 - Acids and Bases

Problema 8

A 0.085 M solution of a monoprotic acid has a percent ionization of 0.59%. Determine the acid ionization constant (Ka) for the acid.

Problema 11

Determine the pH of each solution. a. 0.20 M KCHO₂ b. 0.20 M CH₃NH₃I c. 0.20 M KI

Problema 15

A solution of 0.23 mol of the chloride salt of protonated quinine (QH+), a weak organic base, in 1.0 L of solution has a pH of 4.58. What is the Kb of quinine (Q)?

Problema 31a,b,d

Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base according to the Arrhenius definition. a. HNO₃(aq) b. NH₄⁺(aq) d. HC₂H₃O₂(aq)

Problema 31c

Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base according to the Arrhenius definition. c. KOH(aq)

Problema 32

Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base in aqueous solution according to the Arrhenius definition. a. NaOH(aq) b. H2SO4(aq) c. HBr(aq) d. Sr(OH)2(aq)

Problema 33a,c

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. a. H₂CO₃(aq) + H₂O(l) ⇌ H₃O⁺(aq) + HCO₃^–(aq) c. HNO₃(aq) + H₂O(l) → H₃O⁺(aq) + NO₃^–(aq)

Problema 33b

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. b. NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH^–(aq)

Problema 33d

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. d. C₅H₅N(aq) + H₂O(l) ⇌ C₅H₅NH⁺(aq) + OH^–(aq)

Problema 34b

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. b. CH₃NH₂(aq) + H₂O(l) ⇌ CH₃NH₃⁺(aq) + OH^–(aq)

Problema 34c

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. c. CO₃^2–(aq) + H₂O(l) ⇌ HCO₃^–(aq) + OH^–(aq)

Problema 35c

Write the formula for the conjugate acid of each base. c. HCO3–

Problema 36a

Write the formula for the conjugate base of each acid. a. H2SO4

Problema 36b

Write the formula for the conjugate base of each acid. b. HBr

Problema 36c

Write the formula for the conjugate base of each acid. c. HI

Problema 36d

Write the formula for the conjugate base of each acid. d. HCHO2

Problema 37

Both H₂O and H₂PO₄^– are amphoteric. Write an equation to show how each substance can act as an acid and another equation to show how each can act as a base.

Problema 39a

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). a. HNO₃

Problema 39b

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). b. HCl

Problema 39c

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). c. HBr

Problema 39d

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). d. H₂SO₃

Problema 40a

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). a. HF

Problema 40b

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). b. HCHO₂

Problema 40c

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). c. H₂SO₄

Problema 40d

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (K_a). d. H₂CO₃

Problema 41

The three diagrams represent three different solutions of the binary acid HA. Water molecules have been omitted for clarity, and hydronium ions (H3O+) are represented by hydrogen ions (H+). Rank the acids in order of decreasing strength.

Problema 43

Rank the solutions in order of decreasing [H₃O⁺]: 0.10 M HCl; 0.10 M HF; 0.10 M HClO; 0.10 M HC₆H₅O.

Problema 46c

Pick the stronger base from each pair. c. NO2– or NO3–

Problema 51

Calculate the pH and pOH of each solution at 25 °C. a. [H3O+] = 1.7 × 10^-8 M b. [H3O+] = 1.0 × 10^-7 M c. [H3O+] = 2.2 × 10^-6 M

Problema 53a

Calculate [H₃O⁺] and [OH^–] for each solution at 25 °C. a. pH = 8.55