20.0 mL of 0.075 M aqueous solution of lactic acid CH3CH(OH)COOH, a monoprotic acid, is titrated with aqueous 0.12M NaOH solution. For lactic acid, Ka = 1.4 x 10^-4 a) How many mL of the NaOh solution are needed to reach the equivalence point in the titration? b) What is the pH of the titration solution at the equivalence point in the titration c) What is the pH of the titration solution after the addition of only 5.0mL if the NaOH solution? The answers were attached as, but I can't seem to figure out the work for b and c. a. 12.5 b. pH=8.26 c. pH=3.68

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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.