titration of 25.00 mL of a 0.0800 M acetic acid solution with 0.0700 M KOH. assume temperature is 25 ^{o}C.

What is the analytical concentration of acetate ions at the equivalence point?

What volume of KOH has been added at the half-equivalence point?

CH3COOH + KOH ==== CH3COOK + H2O

25.00 mL of a 0.0800 M CH3COOH = 25.00x10^(-3)x0.0800=0.0020 moles of CH3COOH

So at equivalence point 0.0020 moles of KOH will be added.

Then the volume of KOH added = 0.0020/0.0700=0.02857 L=28.57 ml

So the analytical concentration of CH3COOH = 0.0020 / (25.00+28.57)x10^(-3)=0.0373 M

At half-equivalence point, 0.0010 moles of CH3COOH is neutralized.

So 0.0010 moles of KOH is used at the point.

The volume of KOH = 0.0010/0.0700=0.01429 L=14.29 ml

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