A chemist uses a pipette to transfer 25.0 cm325.0\,\mathrm{cm^{3}}25.0cm3 of barium hydroxide solution into a conical flask. The solution is titrated with 0.100 mol/dm30.100\,\mathrm{mol/dm^{3}}0.100mol/dm3 hydrochloric acid.
Ba(OH)2+2HCl→BaCl2+2H2O \mathrm{Ba(OH)_{2} + 2HCl \rightarrow BaCl_{2} + 2H_{2}O} Ba(OH)2+2HCl→BaCl2+2H2OThe burette readings are shown in the table.
| Titration | Initial burette reading (cm3\mathrm{cm^{3}}cm3) | Final burette reading (cm3\mathrm{cm^{3}}cm3) |
|---|---|---|
| Rough | 0.10 | 25.50 |
| 1 | 0.50 | 25.40 |
| 2 | 1.15 | 26.10 |
| 3 | 0.25 | 25.25 |
The relative formula mass, MrM_rMr, of barium hydroxide is 171.3.
Calculate the concentration of the barium hydroxide solution in g/dm3\mathrm{g/dm^{3}}g/dm3.
152 exam-style questions on OCR GCSE Chemistry 5.1 Monitoring chemical reactions, covering 5.1.1 The technique of titration, 5.1.2 Theoretical mass, percentage yield and atom economy, 5.1.3 Concentration of a solution in mol/dm3, 5.1.4 Concentration calculations and titration results, 5.1.5 Molar gas volume and volumes of gases in reactions, and 5.1.6 Choosing a reaction pathway. Each one has a worked solution and a mark scheme showing where the marks go.