Ch.17 - Acids and Bases

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Tro 5th Edition

Ch.17 - Acids and Bases

Problem 33a,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 33c

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 34

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 35a,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 35b

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 36b

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 36c

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 37a

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

Problem 37b

Write the formula for the conjugate base of each acid. b. H₂SO₃

Problem 37c

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

Problem 37d

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

Problem 38

Write the formula for the conjugate acid of each base. a. NH₃ b. ClO₄^– c. HSO₄^– d. CO₃^2–

Problem 41b

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 41c

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 41d

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 42a

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 42c

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 42d

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 44

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 45c

Pick the stronger base from each pair. c. F^– or ClO^–

Problem 49

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 50a

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

Problem 50b,c

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

Problem 51

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

Problem 53

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 54

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

Problem 54e

Determine whether or not the mixing of each pair of solutions results in a buffer. e. 105.0 mL of 0.15 M CH₃NH₂; 95.0 mL of 0.10 M HCl

Problem 55

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 56

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

Problem 57a

For each strong acid solution, determine [H₃O⁺], [OH^–], and pH. a. 0.25 M HCl