Question

Aqueous sulfuric acid H2SO4 will react with solid sodium hydroxide NaOH to produce aqueous sodium sulfate Na2SO4 and liquid water H2O. Suppose 5.88 g of sulfuric acid is mixed with 6.2 g of sodium hydroxide. Calculate the maximum mass of sodium sulfate that could be produced by the chemical reaction. Be sure your answer has the correct number of significant digits.

Answer 1

Reaction between them is given by-

$2NaOH\ \ +H_2SO_4\ \to\ Na_2SO_4\ \ +2H_2O$

Molar mass of $H_2SO_4=98\ g\ mole^{-1}$

Moles of sulphuric acid taken = $\frac{5.88}{98}=0.06\ mole$

Moles of sodium hydroxide taken = $\frac{6.2}{40}=0.155\ mole$

here sulphuric acid is limiting agent so

reaction will proceed according to sulphuric acid

$0.06\ mole\ H_SO_4\ will \ produce\ same\ amount\ of \ \ Na_2SO_4\\$

Maas of sodium sulphate produced = $moles\times molar\ mass=0.06\times 142=8.52\ g$