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- Which acid in each of the following pairs has the stronger conjugate base? See Table 16.1 to compare the relative strengths of conjugate acid-base pairs. (a) HCl or HF
Problem 58
Problem 60a
Arrange each group of compounds in order of increasing acid strength. Explain your reasoning. (a) HCl, H2S, PH3
- Calculate the percent dissociation of 0.10 M hydrazoic acid (HN3, Ka = 1.9 X 10^-5). Recalculate the percent dissociation of 0.10 M HN3 in the presence of 0.10 M HCl, and explain the change.
Problem 61
- Calculate the pH of 100.0 mL of 0.30 M NH3 before and after the addition of 4.0 g of NH4NO3, and account for the change. Assume that the volume remains constant.
Problem 62
Problem 63a
Identify the weakest acid in each of the following sets. Explain your reasoning. (a) H2SO3, HClO3, HClO4
Problem 63b
Identify the weakest acid in each of the following sets. Explain your reasoning. (b) NH3, H2O, H2S
Problem 63c
Identify the weakest acid in each of the following sets. Explain your reasoning. (c) B(OH)3, Al(OH)3, Ga(OH)3
- Identify the stronger acid in each of the following pairs. Explain your reasoning. (b) H3PO4 or H3AsO4
Problem 64
Problem 65a,b
Identify the stronger base in each of the following pairs.
Explain your reasoning.
(a) ClO2- or ClO3-
(b) HSO4- or HSeO4-
Problem 65c
Identify the stronger base in each of the following pairs.
Explain your reasoning.
(c) HS- or OH-
Problem 65d
Identify the stronger base in each of the following pairs.
Explain your reasoning.
(d) HS- or Br-
- Water at 500 °C and 250 atm is a supercritical fluid. Under these conditions, Kw is approximately 1.7 * 10^-19. Estimate [H3O+] and [OH-] at 500 °C. Is the water acidic, basic, or neutral?
Problem 73
Problem 76d
Calculate the H3O+ concentration to the correct number of significant figures for solutions with the following pH values. (d) 14.25
Problem 79b
Which of the indicators given in Figure 16.5, methyl violet, bromcresol green, phenol red, or thymolphthalein, would be most appropriate to detect a pH change from: (b) 8 to 10?
- Which of the following species behave as strong acids or as strong bases in aqueous solution? (a) HNO2 (b) HNO3(c) NH4+ (d) Cl-
Problem 80
- Which of the following species behave as strong acids or strong bases in aqueous solution? (a) H- (b) O2- (c) H2SO4 (d) CsOH
Problem 81
- Calculate the pH of the following solutions: (c) 0.075 M NaOH
Problem 83
Problem 84a
Calculate the pH of solutions prepared by: (a) Dissolving 4.8 g of lithium hydroxide in water to give 250 mL of solution.
Problem 84d
Calculate the pH of solutions prepared by: (d) Mixing 100.0 mL of 2.0 * 10-3 M HCl and 400.0 mL of 1.0 * 10-3 M HClO4. (Assume that volumes are additive.)
- Calculate the pH of solutions prepared by: (a) Dissolving 0.20 g of sodium oxide in water to give 100.0 mL of solution.
Problem 85
- How many grams of CaO should be dissolved in sufficient water to make 1.00 L of a solution with a pH of 10.50?
Problem 86
- How many grams of SrO should be dissolved in sufficient water to make 2.00 L of a solution with a pH of 10.0?
Problem 87
Problem 88b
Look up the values of Ka in Appendix C for C6H5OH, HNO3, CH3CO2H, and HOCl, and arrange these acids in order of: (b) Decreasing percent dissociation.
- A vitamin C tablet containing 250 mg of ascorbic acid 1C6H8O6; Ka = 8.0 * 10-52 is dissolved in a 250 mL glass of water. What is the pH of the solution?
Problem 94
- Acetic acid 1CH3COOH; Ka = 1.8 * 10-52 has a concentration in vinegar of 3.50% by mass. What is the pH of vinegar? (The density of vinegar is 1.02 g/mL.)
Problem 95
- A typical aspirin tablet contains 324 mg of aspirin (acetylsalicylic acid, C9H8O4), a monoprotic acid having Ka = 3.0 * 10-4. If you dissolve two aspirin tablets in a 300 mL glass of water, what is the pH of the solution and the percent dissociation?
Problem 99
- Write balanced net ionic equations and the corresponding equilibrium equations for the stepwise dissociation of the diprotic acid H2SeO4.
Problem 102
- Write balanced net ionic equations and the corresponding equilibrium equations for the stepwise dissociation of the triprotic acid H3PO4.
Problem 103
- Like sulfuric acid, selenic acid H2SeO4 is a diprotic acid that has a very large value of Ka1. Calculate the pH and the concentrations of all species present in 0.50 M H2SeO4 (Ka2 = 1.2 * 10^-22).
Problem 108
- Calculate the concentrations of H3O+ and SO4 2- in a solution prepared by mixing equal volumes of 0.2 M HCl and 0.6 M H2SO41Ka2 for H2SO4 is 1.2 * 10-22.
Problem 109