Tro - Chemistry: A Molecular Approach 6th Edition - Chapter 17

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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 11
Determine the pH of each solution. a. 0.20 M KCHO₂ b. 0.20 M CH₃NH₃I c. 0.20 M KI
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 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)
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 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.
Problem 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
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 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
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 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.
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