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How does part b differ from part a and how do I go about solving this?
Preparing for the lab: Exercise #3 Your TA asks you to make 100 mLof a benzoic acidbenzoate buffer solution of pH 4.40. The Ka of benzoic acid is 6.5 x 10 s. a) Determine the volumes of 0.50 M benzoic acid and 0.50 M sodium benzoate required to make 100.0 mL of a pH 4.40 buffer solution. b) Determine the volumes of0.50 M benzoic acid and 0.50 M sodium hydroxide required to make 100.0 mL of a pH 4.40 buffer solution. (Hint: these problems will require the Henderson-Hasselbalch Equation and algebra. In each part, there are 2 unknowns: the volume of the acid and the volume of the base. In order to solve for 2 unknowns, you will need 2 equations.)
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a) pH = pk, t log conjugate base weak Acid (moles of benzoate ion) moles of benzoic acid pH pk, + log ( pK,--log(ka) ) =-log(6.5x10-5 - 4.187 (0.1x 0.5) 4.187 + log ( .x 0.5 4.4 ml (0.1x 0.5) 4.187+log ( x 0.5 ml (0.1x 0.5) Xml X 0.5 (0.1x 0.5) (1.632x 0.5) Xml0.0612 L 10(0213) - 6.124 ml of benzoic acid needed

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