Question

10 g of $NaOH$ required a certain amount of $H_{2}S{O}_4$ for complete neutralization. Calculate the number of moles of $H_{2}S{O}_4$ used.

• A. 1 mol
• B. 0.1 mol
• C. 0.5 mol
• D. 0.125 mol

Answer 1

The correct option is D 0.125 mol

The balanced equation for the reaction can be written as:

$2NaOH+H_{2}S{O}_4\to N{a}_{2}S{O}_4+2H_{2}O$

Number of moles in 10g of NaOH $=\frac{MassofNaOH}{MolarmassofNaOH}=$ $\frac{10}{40}=$ 0.25 moles

2 moles of NaOH requires = 1 mole of $H_{2}S{O}_4$

0.25 moles of NaOH forms = $\frac{1}{2}\times 0.25$ = 0.125 moles of $H_{2}S{O}_4$