Question

$150$ mL of $6.0M$ $H_{2}S{O}_4$ solution is mixed with $250$ mL of $3.0M$ $H_{2}S{O}_4$. Resulting molarity is :

• A. $4.125M$
• B. $8.250M$
• C. $4.500M$
• D. $1.650M$

Answer 1

The correct option is A $4.125M$

The expression for the molarity of the mixture is $M\left(mixture\right)=\frac{M_1{V}_1+M_2{V}_2}{V_1+V_2}$
Substituting values in the above expression, we get
$M\left(mixture\right)=\frac{150\times 6.00+250\times 3.00}{150+250}=4.125M$