(a(i))[2]
Identify two soluble salts that can be mixed to make lead(II) chloride.
(a(ii))[3]
Write the ionic equation for the reaction that forms lead(II) chloride when aqueous solutions are mixed. Include state symbols.
(a(iii))[3]
List the steps the student should follow to obtain a pure sample of lead(II) chloride from the mixture in the beaker.
(b(i))[1]
Explain why lead(II) chloride has to be molten before it can conduct electricity.
(b(ii))[2]
Write the ionic half-equation for the reaction taking place at the anode.
(b(iii))[2]
State the test for chlorine gas and the observations.
(b(iv))[1]
Describe what is observed at the cathode.