Question

You titrate 5.0 mL of HCl with 0.010 M NaOH. You find the end point of your titration occurs when 12.0 mL of NaOH has been added. What is the total volume of the solution at the end point of the titration

Answer 1

Answer:

The total volume of the solution at the end point of the titration is 17.0 mL

Explanation:

First we will write a balanced chemical equation for the reaction between HCl and NaOH.

HCl + NaOH    →    NaCl + H₂O

This means 1 mole of HCl will react with 1 mole of NaOH to give 1 mole of NaCl and 1 mole of H₂O

From the question,

Concentration of acid (HCl), $C_{A}$ = ??

Volume of acid (HCl), $V_{A}$ = 5.0 mL

Concentration pf base (NaOH), $C_{B}$ = 0.010 M

Volume of base (NaOH), $V_{B}$ = 12.0 mL

To determine the Concentration of acid, $C_{A}$

From,

$\frac{C_{A}V_{A} }{C_{B}V_{B} } = \frac{n_{A} }{n_{B} }$

Where $n_{A}$ is the mole ratio of acid

and $n_{B}$ is the mole ratio of base.

The concentration of the acid used can be determined from the above formula.

But, we are asked to find the total volume of the solution at the end point of the titration

The total volume of the solution will be the sum of the volume of HCl that reacted and volume of NaOH that reacted.

Hence, The total volume of the solution = $V_{A} + V_{B}$

= 5.0 mL + 12.0 mL

= 17.0 mL

Hence, the total volume of the solution at the end point of the titration is 17.0 mL