Suppose you titrated your standard acid (KHP) with the base to be standardized, but addedseveral drops extra of the base (i.e. stopped the titration after the phenolphthalein indicator inthe solution turned very pink).

a. How would this affect your final determination of the molarity of the base? Wouldyou calculate the concentration to be greater or less than it really is?

b. If this calculated value was used to determine the molar mass of the unknown acid,what type of error would you have for the molar mass of the unknown acid? (i.e.would you overestimate or underestimate the molar mass value?) Support youranswer by, for every step in the calculation, determining whether the calculated valuewould be greater or less than it should be.

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