(a(i))[1]
Write a chemical equation to show the thermal decomposition of barium carbonate.
(a(ii))[1]
Suggest the pH of the solution formed when barium oxide is added to water.
(a(iii))[2]
Name the two gaseous products made when barium nitrate is heated.
(b(i))[2]
Write a chemical equation for the reaction of aqueous sodium carbonate with aqueous barium nitrate.
(b(ii))[3]
Describe how a pure sample of barium carbonate could be obtained from the mixture formed.
(c(i))[2]
Calculate how many moles of barium carbonate were used in this experiment.
(c(ii))[1]
Deduce how many moles of carbon dioxide were produced when all the barium carbonate had reacted.
(c(iii))[1]
Calculate the volume of carbon dioxide formed in (c)(ii) at room temperature and pressure, in $\text{dm}^3$.
(c(iv))[2]
Calculate how many moles of hydrochloric acid were in excess.