(a)[1]
Write the ionic equation that shows an acid reacting with an alkali.
(b(i))[1]
Name one sodium compound and the acid that could be used to make sodium sulfate by this method.
(b(ii))[3]
Describe how titration is used to prepare a colourless solution of sodium sulfate.
(b(iii))[2]
Describe how pure sodium sulfate crystals can be prepared from aqueous sodium sulfate.
(c(i))[2]
Calculate the maximum mass of barium sulfate that could be produced. $\text{Ba}^{2+}(aq) + \text{SO}_4^{2-}(aq) \rightarrow \text{BaSO}_4(s)$ 20.0 cm$^3$ of 0.550 mol/dm$^3$ barium nitrate was added to excess aqueous sodium sulfate. [The relative formula mass of BaSO$_4$ is 233.]
(c(ii))[1]
A dry sample of barium sulfate with a mass of 1.92 g was obtained. Calculate the percentage yield of barium sulfate.