Question

Aqueous sulfuric acid (H,SO) will react with solid sodium hydroxide (NaOH) to produce aqueous sodium sulfate (Na, So) and liquid water (HO). Suppose 44.1 g of sulfuric acid is mixed with 9.7 g of sodium hydroxide. Calculate the minimum mass of sulfuric acid that could be left over by the chemical reaction. Round your answer to 2 significant digits. X 6 ?

Answer 1

Balanced chemical reaction

$H_{2}SO_{4}(aq)+2NaOH(s)\rightarrow Na_{2}SO_{4}(aq)+2H_{2}O(I)$

$moles of H_{2}SO_{4}= \frac{given mass}{molar mass}= \frac{44.1}{98}= 0.45$

$moles of NaOH= \frac{given mass}{molar mass}= \frac{9.7}{40}= 0.24$

For 0.24 moles of NaOH 0.12 moles of H2SO4 is required it means 0.33 moles of H2SO4 left behind.

So Mass of H2SO4 left over= 0.33*98=32.34gm