In the titration of 86.0 mL of 0.400 M HCOOH with 0.150 M LiOH, how many...

Question

Question

In the titration of 86.0 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

HCOOH + LiOH ---> Li(HCOO) + H2O

No of moles of HCOOH = Molarity x Volume in L

= 0.4 M x (86 / 1000) L

= 0.0344 mole

1 mole HCOOH require 1 mole LiOH

0.0344 mole HCOOH requite 0.0344 mole LiOH

Volume of LiOH in L = No of moles of LiOH / Molarity

= 0.0344 mole / 0.150 M

= 0.229 L = (0.2293 x 1000) ml

= 229.3 ml

Answer 2

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