In the titration of 50.0 mL of 0.400 M HCOOH with 0.150 M LiOH, how many...

Question

Question

In the titration of 50.0 mL of 0.400 M HCOOH with 0.150 M LiOH, how many mL of LiOH are required to reach the equivalence point?

Answer 1

Answer #1

The balanced equation is

HCOOH + LiOH ------> HCOOLi + H₂O

Number of moles of HCOOH = 0.400 * 0.05 L = 0.0200 mole

From the balanced equation we can say that

1 mole of HCOOH requires 1 mole of LiOH so

0.0200 mole of HCOOH will require

= 0.0200 mole of HCOOH *(1 mole of LiOH / 1 mole of HCOOH)

= 0.0200 mole of LiOH

Molarity of LiOH = number of moles of LiOH / volume of solution in L

volume of solution in L = 0.0200 mol / 0.150 = 0.133 L

1 L = 1000 mL

0.133 L = 133 mL

Therefore, the volume of LiOH required would be 133 mL

Answer 2

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