Question

In a titration of 35.0 mL of 0.550 M H2SO4, ________ mL of a 0.323 M KOH solution is required for neutralization.

express your answer using 3 significant figures

Answer 1

For all acid base titrations

milliequivalents of acid = milliequivalents of base

H2SO4 being a dibasic acid ,

milliequivalents of H2SO4 = 2 x 35 x 0.550

and milliequivalents of base = 1x V x 0.323

Equating we get V = 119.19 mL

ALTERNATIVELY

H2SO4 + 2KOH ----------> K2SO4 + 2H2O is the balanced equation for the tiration

Then

M1V1/n1 = M2V2 /n2

where n1 and n2 are the storichiometric coefficients of acid and base repsectively.

Thus

35x0.550 /1 = V x 0.323 /2

Which gives V = 119.19 mL