Which brings the titrated solution back to the equivalence

Reference no: EM13345966

You need to titrate 38.2 mL of an acetic acid solution (CH3COOH). (Acetic acid is a monoprotic acid.) You begin your titration with a 0.12 M solution of KOH. After you have added 48.5 mL of the KOH solution, however, you realize that you forgot to add an indicator and have overshot the equivalence point. To neutralize the excess base, you use a second buret to add 10.2 mL of a 0.25 M solution of HCl, which brings the titrated solution back to the equivalence point. What is the molar concentration of the original acetic acid solution?

Reference no: EM13345966

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