Consider the following reactions: Reaction 1: HC1O, + KOH → KC1O, + H;O Reaction 2: HC;H;O2 + KOH → KC;H;O2 +H;O In both reactions, 15.00 mL of 0.8116 M acid is titrated with 0.4217 M KOH. A volume of 28.87 mL of KOH is required to reach the equivalence point in both reactions. a) What is the pH of the HC1O, solution before the titration has started? (No KOH has been added.) b) What is the initial pH of HC;H;O2 solution before the titration has started? K.= 6.46 x 10-5 (Ok to use x is small.) c) What is the pH of Reaction 1 at the equivalence point? d) What is the pH of Reaction 2 at the equivalence point? e) What is the pH of Reaction 1 after 32.00 mL of KOH has been added? f) What is the pH of Reaction 2 after 18.00 mL of KOH has been added?

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.