QuestionQ2. ( $10 \%$ ) Calculated the volume of concentrated sulfuric acid $\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right) 98 \mathrm{wt} \%$ needed to prepare a 250 mL of 0.1 M diluted sulfuric acid solution. (Density of $\mathrm{H}_{2} \mathrm{SO}_{4}=$ $1.818 \mathrm{~g} / \mathrm{mL}$ ) and (Molar mass of $\mathrm{H}_{2} \mathrm{SO}_{4}$ ).

Studdy Solution
Calculate the volume of the concentrated solution required:
First, calculate the mass of the concentrated solution that contains $2.452 \, \text{g}$ of $\mathrm{H}_{2}\mathrm{SO}_{4}$:
$$\text{Mass of concentrated solution} = \frac{\text{Mass of } \mathrm{H}_{2}\mathrm{SO}_{4}}{\text{Weight percent}}$$ $$= \frac{2.452 \, \text{g}}{0.98}$$ $$= 2.502 \, \text{g}$$
Next, calculate the volume of the concentrated solution using its density:
$$\text{Volume of concentrated solution} = \frac{\text{Mass of concentrated solution}}{\text{Density}}$$ $$= \frac{2.502 \, \text{g}}{1.818 \, \text{g/mL}}$$ $$\approx 1.376 \, \text{mL}$$
The volume of concentrated sulfuric acid needed is approximately:
$$\boxed{1.376 \, \text{mL}}$$