Back
- Which of the following can behave both as a Brønsted–Lowry acid and as a Brønsted–Lowry base? (a) HCO3- (b) CN- (c) H2O (d) H2CO3
Problem 49
- Aqueous solutions of hydrogen sulfide contain H2S, HS-, S2-, H3O+ , OH-, and H2O in varying concentrations. Which of these species can act only as an acid? Which can act only as a base? Which can act both as an acid and as a base?
Problem 54
- The hydronium ion H3O+ is the strongest acid that can exist in aqueous solution because stronger acids dissociate by transferring a proton to water. What is the strongest base that can exist in aqueous solution?
Problem 55
- Choose from the conjugate acid–base pairs HSO4- >SO42-, HF>F-, and NH4+>NH3 to complete the following equation with the pair that gives an equilibrium constant Kc 7 1. _____ + NO2 - S _____ + HNO2
Problem 56
- Choose from the conjugate acid–base pairs F- > HF, NH3 > NH4+, and NO3- > HNO3, to complete the following equation with the pair that gives an equilibrium constant Kc > 1. _____ + H2CO3 ⇌ _____ + HCO3-
Problem 57
- 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
- Which base in each of the following pairs has the stronger conjugate acid? See Table 16.1 to compare the relative strengths of conjugate acid-base pairs. (a) Cl- or CO32-
Problem 59
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 76e
Calculate the H3O+ concentration to the correct number of significant figures for solutions with the following pH values. (e) -1.0
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?
Problem 79c
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: (c) 2 to 0?
- 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