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A weak acid HA (pKa = 5.00) was titrated with 1.10 M KOH. The acid solution...

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Chemistry

A weak acid HA (pKa = 5.00) was titrated with 1.10 M KOH. Theacid solution had a volume of 100.0 mL and a molarity of 0.107 M.Find the pH at the following volumes of base added: Vb = 0.00,1.00, 5.00, 9.00, 9.90, 10.00, 10.10, and 12.00 mL. (Assume Kw =1.01 ✕ 10−14.)

Answer & Explanation Solved by verified expert
4.2 Ratings (875 Votes)
1 Without any KOH added this weak acid undergoes self dissociation HA H A pKa 500 hence H A Ka 10500 HAHA H20100 pH logH 05logKa0100 300 2 I will just arbitrarily pick one case say 5ml base added and you SHOULD solve the rest base added 1 9 and 99    See Answer
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