Acid-Base Equilibria


The following problems are taken from T. L. Brown, H. E. Lemay, B. E. Bursten, & J. R. Burdge, Chemistry: The Central Science, Ninth Edition, Chapter 16. To see the solution to a problem or to return from the solution, click on the number of the problem.


24) Consider two solutions, solution A and solution B. [H+] in solution A is 500 times greater than that in solution B. What is the difference in the pH values of the two solutions?


34) Calculate the pH of each of the following strong acid solutions:

      (a) 0.0575 M HNO3

      (b) 0.723 g HClO4 in 2.00 L of solution

      (c) 5.00 mL of 1.00 M HCl diluted to 0.750 L

      (d) a mixture formed by adding 50.0 mL of 0.020 M HCl to 125 mL of 0.010 HI


38) Calculate the concentration of an aqueous solution of Ca(OH)2 that has a pH of 12.00.

46) A 0.100 M solution of chloroacetic acid (ClCH2COOH) is 11.0% ionized. Using this information calculate, [ClCH2COO-], [H+], [ClCH2COOH], and Ka for chloroacetic acid.   


54) The active ingredient in aspirin is acetylsalicylic acid (HC9H7O4), a monoprotic acid with a Ka = 3.3 x 10-4 at 25°C. What is the pH of a solution obtained by dissolving two extra-strength aspirin tablets, containing 500 mg of acetylsalicylic acid each, in 250 mL of water?


66) Calculate the molar concentration of OH- ions in a 1.15 M solution of hypobromite ion (BrO-; Kb = 4.0 x 10-6). What is the pH of the solution?


80) Trisodium phosphate (Na3PO4) is available in hardware stores as TSP and is used as a cleaning agent. The label on a box of TSP warns that the substance is very basic (caustic or alkaline). What is the pH of a solution containing 50.0 g of TSP in a liter of solution?

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