Question

2) How many milliliters of water have to be added to 264.2 mL of 0.27 M HCl to reduce the concentration to 0.10 M HCl?

Answer 1

ANSWER

The volume of water required to reduce the concentration is 713.34 mL

STEP-BY-STEP EXPLANATION

Given information

The inital concentration of HCl = 0.27 M

The initial volume of HCl = 264.2 mL

The final concentration of HCl = 0.10 M

Let the volume of water be V2

To calculate the volume of water required to reduce the concentration of HCl, we will need to apply the dilution formula

$C1V1\text{ = C2V2}$

$\begin{gathered} 0.27\text{ }\times\text{ 264.2 = 0.1 }\times\text{ V2} \\ 71.334\text{ = }0.1V2 \\ \text{Divide both sides by 0.1} \\ \frac{71.344}{0.1}\text{ = }\frac{\cancel{0.1}V2}{\cancel{0.1}} \\ V2\text{ = 713.34 mL} \end{gathered}$

Therefore, the volume of water required to reduce the concentration is 713.34 mL