1. The problem statement, all variables and given/known data A certain volume of a solution of 0.800M sulfuric acid was added to solid magnesium carbonate, and the carbon dioxide evolved was passed through concentrated sodium hydoxide solution. When the reaction had ceased, the mass of this solution was found to have increased by 15.0g What volume of sulfuric acid must have been added? 2. Relevant equations Basic stoichiometry 3. The attempt at a solution H2SO4 + MgCO3 -> MgSO4 + H2O + CO2 CO2 + NaOH -> NaHCO3 Hence H2SO4 + MgCO3 -> MgSO4 + H2O + NaHCO3 The extra weight comes from NaOH. Since the weight of the products had increased by 15g it must be due to NaOH. It comes out to .375 moles of NaOH. Since the mole ratio for every molecule is 1, there should be .375 moles of H2SO4 added. There are 0.8 moles of H2SO4 per litre so .375/.8=.47L or 470ml of H2SO4 but the answer at the back of the book suggest something else. I don’t know where I could have made my mistake.