Brown - Chemistry: The Central Science 14th Edition

Ch.16 - Acid-Base Equilibria

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Brown 14th Edition

Ch.16 - Acid-Base Equilibria

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 44b

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

Problem 45

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 46

Calculate [OH-] and pH for each of the following strong base solutions: (a) 0.182 M KOH, (b) 3.165 g of KOH in 500.0 mL of solution, (c) a solution formed by mixing 20.0 mL of 0.015 M Ba(OH)2 with 40.0 mL of 8.2 x 10^-3 M NaOH.

Problem 46c

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 47

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

Problem 48

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

Problem 49

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 50

Write the chemical equation and the K_a expression for the acid dissociation of each of the following acids in aqueous solution. First show the reaction with H⁺(a)q as a product and then with the hydronium ion: (a) C₆H₅COOH (b) HCO₃^-

Problem 51

Lactic acid CH3CH(OH)COOH has one acidic hydrogen. A 0.10 M solution of lactic acid has a pH of 2.44. Calculate Ka.

Problem 52

Phenylacetic acid 1C6H5CH2COOH2 is one of the substances that accumulates in the blood of people with phenylketonuria, an inherited disorder that can cause mental retardation or even death. A 0.085 M solution of C6H5CH2COOH has a pH of 2.68. Calculate the Ka value for this acid.

Problem 53

A 0.100 M solution of chloroacetic acid 1ClCH2COOH2 is 11.0% ionized. Using this information, calculate 3ClCH2COO-4, 3H+4, 3ClCH2COOH4, and Ka for chloroacetic acid.

Problem 54

A 0.100 M solution of bromoacetic acid 1BrCH2COOH2 is 13.2% ionized. Calculate 3H+4, 3BrCH2COO-4, 3BrCH2COOH4 and Ka for bromoacetic acid.

Problem 55

A particular sample of vinegar has a pH of 2.90. If acetic acid is the only acid that vinegar contains (Ka = 1.8 * 10^-5), calculate the concentration of acetic acid in the vinegar.

Problem 56

If a solution of HF 1Ka = 6.8 * 10-42 has a pH of 3.65, calculate the concentration of hydrofluoric acid.

Problem 32

Problem 33

Problem 34