University of Adelaide Hypochlorous Acid and Monoprotic Acid Problems Paper
Summative assignment questions
The molarity of an aqueous solution of Ba(OH)2 is 0.0024 M.
(a) What is the concentration of H3O+ in this solution?
(b) What is the pH of the solution?
(c) What is the OH– concentration in the solution?
Carbonic acid, H2CO3 is a weak acid. Its first Ka is 4.5 x 10-7. Calculate the Kb of its conjugate base.
A 0.115 M aqueous solution of an organic monoprotic acid HX has a pH of 3.42. Calculate Ka for HX.
(Type the exponent part of your answer in the second box. For example, for 2.0 x 10–5, you would type 2.0 in the first box and -5 into the second box.)
Hypochlorous acid, HOCl, is a weaker monoprotic acid than acetic acid. In a 0.11 M solution, the pH is 4.24.
Calculate the Ka for hypochlorous acid.
Calculate the pKa for hypochlorous acid.
If 25 mL of 0.45 M HCl is added to 30 mL of 0.35 M NaOH, what is the pH of the final solution?
Calculate the pH of a buffer solution containing 0.125 M potassium acetate and 0.100 M acetic acid. (pKa, CH3COOH = 4.74)
If 0.050 mol of HCl is added to 1.0 L of a buffer solution containing 0.125 M potassium acetate and 0.10 M acetic acid, what is the change in pH of the solution?
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