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How many milliliters of 1.00 M KOH should be added to 100 mL of solution containing 10.0 g of histidine hydrochloride (His HCl,
FM 191.62) to get a pH of 9.30?

First, divide 10.0g by 191.62g/mol to get 0.052187 mols of histidine HCl, pKa of 6.5.

Then, using pH = pKa + logx/.052187-x, the x is found to be 0.0521 mols of OH-.

From this point, should I multiply 0.0521 by 1.0M or by the molecular weight of KOH? I think I should multiply by 1.0M which would yield 52.1mL of KOH. If anyone can verify the accuracy of this answer, please respond.

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