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10 Nov 2019
Question 3-4 Identify the strongest acid species and the strongest base species that can exist in aqueous solution by their names and formulas. Explain why the deionized water in the laboratory typically has a pH below 7. Calculate the pH of each of the following solutions. a. 0.500 M HCl b. 9.5 times 10^-2 M AI(OH)_3 c. 0.088 M CH_3CH_2COOH, Ka = 1.3 times 10^-5 d. 0.120 M C_5H_5N, Kb = 1.7 times 10^-9 Calculate the Ka for chloroacetic acid if a 0.100 M solution has a pH of 1.95. Calculate the molarity of an aqueous solution of HCN (Ka = 4.9 times 10^-10) whose pH is 5.00. Bromoacetic acid, BrCH_2CO_2H, is a monoprotic acid for which a 0.100 M solution is 13.2 % dissociated at equilibrium. Calculate Ka for this acid.
Question 3-4
Identify the strongest acid species and the strongest base species that can exist in aqueous solution by their names and formulas. Explain why the deionized water in the laboratory typically has a pH below 7. Calculate the pH of each of the following solutions. a. 0.500 M HCl b. 9.5 times 10^-2 M AI(OH)_3 c. 0.088 M CH_3CH_2COOH, Ka = 1.3 times 10^-5 d. 0.120 M C_5H_5N, Kb = 1.7 times 10^-9 Calculate the Ka for chloroacetic acid if a 0.100 M solution has a pH of 1.95. Calculate the molarity of an aqueous solution of HCN (Ka = 4.9 times 10^-10) whose pH is 5.00. Bromoacetic acid, BrCH_2CO_2H, is a monoprotic acid for which a 0.100 M solution is 13.2 % dissociated at equilibrium. Calculate Ka for this acid.
Keith LeannonLv2
26 Jul 2019