How many milliliters of 1.00 KOH should be added to 100 mL of solution containin

Question

How many milliliters of 1.00 KOH should be added to 100 mL of solution containing 10.0 g of histidine hydrochloride (FM 191.62) to get a pH of 9.30? The answer is 78.9 mL but I don't know how to get there.

Explanation / Answer

His-HCl + KOH ----> His-HCl-K+ Molarity of His -HCl , M = ( mass/molarmass) / volume in L = ( 10.0 / 191.62 ) / 0.1 L = 0.522 M No.of moles , n = molarity x volume in L = 0.522 x 0.1 L = 0.522 moles According to the balanced equation , 1 mole of His-HCl reacts with 1 mole of KOH 0.522 moles of His -HCl reacts with 0.522 moles of KOH So volume of KOH required(in L) , V = no.of moles / molarity = 0.522 moles / 1.00 M = 0.522 L = 522 mL

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