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A volume of 70.0 mL of a 0.860 M HNO3 solution is titrated with 0.450 M...

A volume of 70.0 mL of a 0.860 M HNO3 solution is titrated with 0.450 M KOH. Calculate the volume of KOH required to reach the equivalence point.

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Answer #1

Hi use formula

M1V1 = M2V2 when both reactants have equal number of moles in balanced chemical reaction equation.

HNO3 + KOH --> H2O + KNO3

M1 = concentration of HNO3 = 0.860 M; V1 = volume of HNO3 at equivalence point = 70.0 mL

M2 = concentration of KOH = 0.450 M;   V2 = volume of KOH at equivalence point = to be calculated

V2 = (M1V1) / M2 = [0.860 M x 70.0 mL) / 0.450 M = 134 mL

Volume of KOH required to reach the equivalence point = 134 mL

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