Question Description
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 organicmonoprotic 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, for2.0 x 10–5, you would type 2.0 in the first box and -5 into the second box.)
Hypochlorous acid, HOCl, is a weakermonoprotic 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 of0.35 M NaOH, what is the pH of the final solution?
Calculate the pH of a buffer solutioncontaining 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 abuffer solution containing 0.125 M potassium acetate and 0.10 M acetic acid,what is the change in pH of the solution?
Summative assignment questionsThe 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?
