Brown - Chemistry: The Central Science 14th Edition

Ch.16 - Acid-Base Equilibria

Back

All textbooks

Brown 14th Edition

Ch.16 - Acid-Base Equilibria

Problem 23
Which of the following is the stronger Brønsted–Lowry acid, HBrO or HBr?
Problem 24
Which of the following is the stronger Brønsted–Lowry acid, HClO3 or HClO2?
Problem 25
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 26
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 27
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 28
If a solution is described as basic, which of the following is true: (i) 3H+ < 3OH-, (ii) 3H+ = 3OH-, or (iii) 3H+ > 3OH-?
Problem 28a
Write a chemical equation that illustrates the autoionization of water.
Problem 28b
Write the expression for the ion product constant for water, K_w.
Problem 29
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 30a
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 30b
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 30c
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 31
Which of the following solutions is the most acidic? (a) 0.2 M Ba(OH)2, (b) 0.2 M H2SO3, (c) 1.0 M glucose 1C6H12O6).
Problem 32
Which of the following solutions is the most basic? (a) 0.6 M NaCl, (b) 0.150 M CsOH, (c) 0.100 M Sr1OH22.
Problem 32
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 33
By what factor does [H⁺] change for a pH change of (a) 2.00 units? (b) 0.50 units?
Problem 34
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 35

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

Problem 36

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

Problem 37

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 38

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 39

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. (a) Is the solution acidic, neutral, or basic? (b) Is there another indicator you could use to narrow the range of possible pH values for the solution?

Problem 39b

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 40b

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 40c

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 43b

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

Problem 44

Calculate the pH of each of the following strong acid solutions: (a) 0.0167 M HNO3 (b) 15.00 mL of 1.00 M HCl diluted to 0.500 L (c) a mixture formed by adding 50.0 mL of 0.020 M HCl to 125 mL of 0.010 M HI.

Problem 23

Problem 24

Problem 25

Problem 26

Problem 27

Problem 28

Problem 28a

Problem 28b

Problem 29

Problem 30a

Problem 30b

Problem 30c

Problem 31

Problem 32

Problem 32

Problem 33

Problem 34