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 K_a is 4.5 x 10^-7. Calculate the K_b of its conjugate base.

A 0.115 M aqueous solution of an organic monoprotic acid HX has a pH of 3.42. Calculate K_a 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 K_a for hypochlorous acid.

Calculate the pK_a 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. (pK_a, 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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