Brown - Chemistry: The Central Science 15th Edition

Ch.16 - Acid-Base Equilibria

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Brown 15th Edition

Ch.16 - Acid-Base Equilibria

Problem 27
Which of the following is the stronger Brønsted–Lowry acid, HBrO or HBr?
Problem 28
Which of the following is the stronger Brønsted–Lowry acid, HClO3 or HClO2?
Problem 29
Predict the products of the following acid–base reactions, and predict whether the equilibrium lies to the left or to the right of the reaction arrow:
(a) O^2-(aq) + H₂O(l) ⇌
(b) CH₃COOH(aq) + HS^-(aq) ⇌
(c) NO₂^-(aq) + H₂O(l) ⇌
Problem 30
Predict the products of the following acid–base reactions, and predict whether the equilibrium lies to the left or to the right of the reaction arrow:
(a) NH₄⁺(aq) + OH^-(aq) ⇌
(b) CH₃COO^-(aq) + H₃O⁺(aq) ⇌
(c) HCO₃^-(aq) + F^-(aq) ⇌
Problem 31
If a neutral solution of water, with pH = 7.00, is cooled to 10 °C, the pH rises to 7.27. Which of the following three statements is correct for the cooled water: (i) [H+] > [OH-], (ii) [H+] = [OH-], or (iii) [H+] < [OH-]?
Problem 32a
Write a chemical equation that illustrates the autoionization of water.
Problem 32b
Write the expression for the ion product constant for water, K_w.
Problem 33
Calculate [H⁺] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) [OH^-] = 0.00045 M (b) [OH^-] = 8.8 × 10^-9 M (c) a solution in which [OH^-] is 100 times greater than [H⁺].
Problem 34a
Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) 3H+4 = 0.0505 M
Problem 34b
Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (b) 3H+4 = 2.5 * 10-10 M
Problem 34c
Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (c) a solution in which 3H+4 is 1000 times greater than 3OH-4.
Problem 36
Deuterium oxide 1D2O, where D is deuterium, the hydrogen-2 isotope) has an ion-product constant, Kw, of 8.9 * 10-16 at 20 °C. Calculate 3D+4 and 3OD-4 for pure (neutral) D2O at this temperature.
Problem 37
By what factor does [H⁺] change for a pH change of (a) 2.00 units? (b) 0.50 units?
Problem 38
Consider two solutions, solution A and solution B. The concentration of 3H+4 in solution A is 250 times greater than that in solution B. What is the difference in the pH values of the two solutions?

Problem 39

Complete the following table by calculating the missing entries and indicating whether the solution is acidic or basic.

Problem 40

Complete the following table by calculating the missing entries. In each case, indicate whether the solution is acidic or basic.

Problem 41

The average pH of normal arterial blood is 7.40. At normal body temperature 137 °C2, Kw = 2.4 * 10-14. Calculate 3H+4, 3OH-4, and pOH for blood at this temperature.

Problem 42

Carbon dioxide in the atmosphere dissolves in raindrops to produce carbonic acid (H2CO3), causing the pH of clean, unpolluted rain to range from about 5.2 to 5.6. What are the ranges of [H+] and [OH-] in the raindrops?

Problem 43b

Addition of the indicator methyl orange to an unknown solution leads to a yellow color. The addition of bromthymol blue to the same solution also leads to a yellow color. (b) What is the range (in whole numbers) of possible pH values for the solution?

Problem 44b

Addition of phenolphthalein to an unknown colorless solution does not cause a color change. The addition of bromthymol blue to the same solution leads to a yellow color. (b) Which of the following can you establish about the solution: (i) A minimum pH, (ii) A maximum pH, or (iii) A specific range of pH values?

Problem 44c

Addition of phenolphthalein to an unknown colorless solution does not cause a color change. The addition of bromthymol blue to the same solution leads to a yellow color. (c) What other indicator or indicators would you want to use to determine the pH of the solution more precisely?

Problem 45

Is each of the following statements true or false? (a) All strong acids contain one or more H atoms. (b) A strong acid is a strong electrolyte. (c) A 1.0-M solution of a strong acid will have pH = 1.0.

Problem 46

Determine whether each of the following is true or false: (a) All strong bases are salts of the hydroxide ion. (b) The addition of a strong base to water produces a solution of pH > 7.0. (c) Because Mg(OH)2 is not very soluble, it cannot be a strong base.

Problem 47b

Calculate the pH of each of the following strong acid solutions: (b) 1.52 g of HNO₃ in 575 mL of solution

Problem 48b

Calculate the pH of each of the following strong acid solutions: (b) 0.225 g of HClO₃ in 2.00 L of solution

Problem 49

Calculate [OH-] and pH for (a) 1.5 × 10^-3 M Sr(OH)_2 (b) 2.250 g of LiOH in 250.0 mL of solution (c) 1.00 mL of 0.175 M NaOH diluted to 2.00 L (d) a solution formed by adding 5.00 mL of 0.105 M KOH to 15.0 mL of 9.5 × 10^-2 M Ca(OH)_2.

Problem 50c

Calculate [OH^-] and pH for each of the following strong base solutions: (c) 10.0 mL of 0.0105 M Ca(OH)₂ diluted to 500.0 mL

Problem 51

Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.50.

Problem 52

Calculate the concentration of an aqueous solution of Ca1OH22 that has a pH of 10.05.

Problem 53

Write the chemical equation and the Ka expression for the ionization of each of the following acids in aqueous solution. First, show the reaction with H+(aq) as a product and then with the hydronium ion: (a) HBrO2 (b) C2H5COOH.

Problem 27

Problem 28

Problem 29

Problem 30

Problem 31

Problem 32a

Problem 32b

Problem 33

Problem 34a

Problem 34b

Problem 34c

Problem 36

Problem 37

Problem 38