Ch.17 - Acids and Bases

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Tro 6th Edition

Ch.17 - Acids and Bases

Problem 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.

Problem 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)?

Problem 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)

Problem 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)

Problem 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)

Problem 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)

Problem 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)

Problem 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)

Problem 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)

Problem 35c

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

Problem 36a

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

Problem 36b

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

Problem 36c

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

Problem 36d

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

Problem 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

Problem 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

Problem 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

Problem 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

Problem 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

Problem 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

Problem 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.

Problem 46c

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

Problem 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

Problem 53a

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

Problem 53b,c

Calculate [H₃O⁺] and [OH^–] for each solution at 25 °C. b. pH = 11.23 c. pH = 2.87

Problem 55

Complete the table. (All solutions are at 25 °C.)

Problem 57

Like all equilibrium constants, the value of K_w depends on temperature. At body temperature (37 °C), K_w = 2.4×10^–14. What are the [H₃O⁺] and pH of pure water at body temperature?

Problem 58

The value of K_w increases with increasing temperature. Is the autoionization of water endothermic or exothermic?

Problem 59

Calculate the pH of each acid solution. Explain how the resulting pH values demonstrate that the pH of an acid solution should carry as many digits to the right of the decimal place as the number of significant figures in the concentration of the solution. [H₃O⁺] = 0.044 M [H₃O⁺] = 0.045 M [H₃O⁺] = 0.046 M

Problem 60

Determine the concentration of H₃O⁺ to the correct number of significant figures in a solution with each pH. Describe how these calculations show the relationship between the number of digits to the right of the decimal place in pH and the number of significant figures in concentration. pH = 2.50 pH = 2.51 pH = 2.52