Consider the following data on some weak acids and weak bases: acid base K. K, name formula name formula hypochlorous acid HCIO 3.0 × 108 hydroxylamine HONH, 1.1 × 10-8 HCH;CO, 1.8 × 10 5 pyridine C3H;N 1.7x 109 olo acetic acid Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M NaCH3CO2 choose one v 0.1 M NaBr choose one v 0.1 M C5H5NHCI choose one v 0.1 M HONH3B v choose one 1 (lowest) 2 3 4 (highest)

Consider the following data on some weak acids and weak bases: acid base K. K, name formula name formula hypochlorous acid HCIO 3.0 × 108 hydroxylamine HONH, 1.1 × 10-8 HCH;CO, 1.8 × 10 5 pyridine C3H;N 1.7x 109 olo acetic acid Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M NaCH3CO2 choose one v 0.1 M NaBr choose one v 0.1 M C5H5NHCI choose one v 0.1 M HONH3B v choose one 1 (lowest) 2 3 4 (highest)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.55QE

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Consider 0.10 M solutions of the following compound: AlCl3, NaCN, KOH, CsClO4, and NaF. Place these solutions in order of increasing pH.
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Tartaric acid is a weak diprotic fruit acid with Ka1 = 1.0 103 and Ka2 = 4.6 105. a Letting the symbol H2A represent tartaric acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 Ka2. b Qualitatively describe the relative concentrations of H2A, HA, A2, and H3O+ in a solution that is about 0.5 M in tartaric acid. c Calculate the pH of a 0 0250 M tartaric acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentration in solutions b and c?
Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus 30.0 mL of 0.100 M sodium hydroxide (b) 100.0 mL of 0.250 M ammonia plus 50.0 mL of 0.100 M hydrochloric acid (c) 25.0 mL of 0.200 M sulfuric acid plus 50.0 mL of 0.400 M sodium hydroxide
A solution has a pH of 4.5. What would be the color of the solution if each of the following indicators were added? (See Fig. 14-8.) a. methyl orange b. alizarin c. bromcresol green d. phenolphthalein
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Write the acid ionization constant expression for the ionization of each of the following monoprotic acids. a. HCN (hydrocyanic acid) b. HC6H7O6 (ascorbic acid)
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