A student monitors the progress of the precipitation reaction between excess barium chloride, BaCl2(aq)\text{BaCl}_2(\text{aq})BaCl2(aq), and a 50.0 cm3 sample of sulfuric acid, H2SO4(aq)\text{H}_2\text{SO}_4(\text{aq})H2SO4(aq). At a specific time ttt, the dry precipitate of barium sulfate, BaSO4(s)\text{BaSO}_4(\text{s})BaSO4(s) (molar mass = 233.4 g mol-1), filtered from the mixture has a mass of 1.167 g.
What is the concentration, in mol dm−3\text{mol dm}^{-3}mol dm−3, of the remaining sulfate ions, SO42−\text{SO}_4^{2-}SO42−, in the solution at time t t\,t if the initial concentration of the sulfuric acid was 0.150 mol dm-3? (Assume the total volume of the solution remains constant at 50.0 cm3.)
0.0500 mol dm−30.0500\text{ mol dm}^{-3}0.0500 mol dm−3
0.100 mol dm−30.100\text{ mol dm}^{-3}0.100 mol dm−3
0.150 mol dm−30.150\text{ mol dm}^{-3}0.150 mol dm−3
0.0250 mol dm−30.0250\text{ mol dm}^{-3}0.0250 mol dm−3
91 exam-style questions on OCR GCSE Chemistry Monitoring chemical reactions. Each one has a worked solution and a mark scheme showing where the marks go.