Question

A chemist wants to dilute 50 mL of a 3.5 M $H_{2}S{O}_4$ solution to a 2 M $H_{2}S{O}_4$ solution. To what volume must it be diluted?

• A. 87.5 mL
• B. 79.2 mL
• C. 75.5 mL
• D. 87.0 mL

Answer 1

The correct option is A 87.5 mL

$M_1{V}_1=M_2{V}_2$
Where,
$M_1\Rightarrow$ Molarity of the initial solution = 3.5 M
$V_1\Rightarrow$ Volume of the initial solution = 50 mL
$M_2\Rightarrow$ Molarity of the resultant solution i.e. after dilution = 2 M
$V_2\Rightarrow$ Volume of the resultant solution
$3.5\times 50=2\times V_2$
$V_2=\frac{3.5\times 50}{2}=87.5$ mL
Therefore, the initial solution must be diluted to 87.5 mL.