You are given a solution of hcooh (formic acid) with an approximate concentration of 0.20 m and you will titrate this with a 0.1105 m naoh. if you add 20.00 ml of hcooh to the beaker before titrating, approximately what volume of naoh will be required to reach the end point? view available hint(s) you are given a solution of (formic acid) with an approximate concentration of 0.20 and you will titrate this with a 0.1105 . if you add 20.00 of to the beaker before titrating, approximately what volume of will be required to reach the end point? 11.1 ml 20.0 ml 72.4 ml 36.2 ml

The volume of NaOH required to reach the end point is 36.2 mL

We'll begin by writing the balanced equation for the reaction.

HCOOH + NaOH —> HCOONa + H₂O

From the balanced equation above,

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

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

From the question given above,

Molarity of base, NaOH (Mb) = 0.1105 M

Volume of acid, HCOOH (Va) = 20 mL

Molarity of acid, HCOOH (Ma) = 0.2 M

MaVa / MbVb = nA/nB

(0.2 × 20) / (0.1105 × Vb) = 1

4 / (0.1105 × Vb) = 1

Cross multiply

0.1105 × Vb = 4

Divide both side by 0.1105

Vb = 4 / 0.1105

Thus, the volume of the base, NaOH is 36.2 mL

Learn more: link

Explanation:

1. Write the balanced chemical equation.

2. Calculate the moles of HCOOH

3. Calculate the moles of NaOH.

4. Calculate the volume of NaOH