Question

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

Answer 1

Answer:

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 =

184mL of LiOH are required

Answer 2

the volume of the base, LiOH required to reach the equivalence point is 184 mL

We'll begin by writing the balanced equation for the reaction. This is given below

HCOOH + LiOH —> HCOOLi + H₂O

From the balanced equequationation above,

The mole ratio of the acid, HCOOH (nA) = 1

The mole ratio of the base, LiOH (nB) = 1

From the question given above, the following data were:

Volume of acid, HCOOH (Va) = 69.0 mL

Molarity of acid, HCOOH (Ma) = 0.4 M

Molarity of base, LiOH (Mb) = 0.150 M

Volume of base, LiOH (Vb) =?

The volume of the base, LiOH required to reach the equivalence point can be obtained as follow:

MaVa / MbVb = nA / nB

(0.4 × 69) / (0.150 × Vb) = 1

27.6 / (0.150 × Vb) = 1

Cross multiply

0.150 × Vb = 27.6

Divide both side by 0.150

Vb = 27.6 / 0.150

Vb = 184 mL

Therefore, the volume of the base, LiOH required to reach the equivalence point is 184 mL

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