Question

Part A

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?

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?

20.0 mL

11.1 mL

72.4 mL

36.2 mL

SubmitRequest Answer

Part B

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. You add 20.00 mL of HCOOH to the beaker before titrating, and it requires 35.43 mL of NaOH to reach the end point. What is the concentration of the HCOOH solution?

You are given a solution of  (formic acid) with an approximate concentration of 0.20  and you will titrate this with a 0.1105  . You add 20.00  of  to the beaker before titrating, and it requires 35.43  of  to reach the end point. What is the concentration of the  solution?

0.1105 M

0.1958 M

0.0624 M

0.2000 M

Answer 1

Reaction is:

HCOOH + NaOH --> HCOONa + H₂O

Part A

Molarity of HCOOH (M₁) = 0.20 M

Volume of HCOOH (V₁) = 20.0 mL

Molarity of NaOH(M₂) = 0.1105 M

Let the volume of NaOH be V₂

From molarity equation

M₁V₁ = M₂V₂

0.20 M * 20.0 mL = 0.1105 M *V₂

V₂ = 36.2 mL

Part B

Let the Molarity of HCOOH beM₁

Volume of HCOOH (V₁) = 20.00 mL

Molarity of NaOH(M₂) = 0.1105 M

volume of NaOH (V₂) = 35.43 mL

From molarity equation

M₁V₁ = M₂V₂

M₁ * 20.00mL = 0.1105 M * 35.43 mL

M₁ = 0.1958 M