Aqueous sulfuric acid h2so4 will react with solid sodium hydroxide naoh to produce aqueous sodium sulfate na2so4 and liquid water h2o. suppose 89.3 g of sulfuric acid is mixed with 96. g of sodium hydroxide. calculate the minimum mass of sulfuric acid that could be left over by the chemical reaction. be sure your answer has the correct number of significant digits.

1) Balanced chemical equation

H2SO4 + 2NaOH - - - > Na2 SO4 + 2H2O

=> 1 mol H2SO4 : 2 moles NaOH

2) Convert 89.3 g of H2SO4 and 96.0 g of NaOH to moles

Molar mass of H2SO4 = 98.1 g/mol

Molar mass of NaOH = 40.0 g/mol

moles = mass in grams / molar mass

moles H2SO4 = 89.3 g / 98.1 g/mol = 0.910 mol

moles NaOH = 96.0 g / 40.0 g/mol = 2.40 mol

3) Theoretical molar ratio = 2 moles NaOH / 1 mol H2SO4

So, all the 0.91 mol of H2SO4 will be consumed along with 1.820 (2*0.91) moles of NaOH, and 0.580 moles (2.40 - 1.82) of NaOH will be left over by the chemical reaction.

4) Convert 0.580 moles NaOH to mass

0.580 moles * 40.0 g/mol = 23.2 g of NaOH will be left over