In the titration of 69.0 mL of 0.400 M HCOOH with 0.150 M LiOH, how many mL of LiOH are required to reach the equivalence point

184mL of LiOH are required

Explanation:

HCOOH, formic acid, reacts with lithium hydroxide, LiOH, as follows:

HCOOH + LiOH → LiCOOH + H₂O

Based on the equation, 1 mole of HCOOH reacts per mole of LiOH.

Thus, to know hoy many moles of LiOH you need to reach the equivalence pointy, you know the moles of HCOOH you have to neutralize.

Moles HCOOH you need to neutralize:

69.0mL = 0.069L * (0.400mol / L) = 0.0276 moles HCOOH

That means you need to add 0.0276 moles of LiOH to neutralize the formic acid. With molar concentration, we can determine the volume of LiOH, thus:

Volume 0.150M LiOH:

0.0276 moles LiOH * (1L / 0.150moles LiOH) = 0.184L of 0.150M LiOH =

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explanation:

i think option no d is the correct answer