Making insoluble salts
4 marks · NormalThree precipitation reactions are shown below. For each reaction, complete the table by writing a balanced ionic equation for the formation of the insoluble salt, including state symbols.
| Reaction | Insoluble Salt | Ionic Equation |
|---|---|---|
| Silver nitrate + sodium bromide | Silver bromide | |
| Lead(II) nitrate + potassium sulfate | Lead(II) sulfate | |
| Barium chloride + sodium carbonate | Barium carbonate |
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Common mistakes: Missing or incorrect charge on ions; Incorrect state symbols; Incorrect coefficients
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Marking points
M1 · 1 mark · Correct ionic equation for silver bromide, including state symbols: Ag+(aq) + Br-(aq) -> AgBr(s)
M2 · 1 mark · Correct ionic equation for lead(II) sulfate: Pb2+(aq) + SO4^2-(aq) -> PbSO4(s)
M3 · 1 mark · Correct ionic equation for barium carbonate: Ba2+(aq) + CO3^2-(aq) -> BaCO3(s)
A1 · 1 mark · All three equations include correct state symbols and balanced charges.
Worked solution
| Reaction | Insoluble Salt | Ionic Equation |
|---|---|---|
| Silver nitrate + sodium bromide | Silver bromide | Ag^+(aq) + Br^-(aq) → AgBr(s) |
| Lead(II) nitrate + potassium sulfate | Lead(II) sulfate | Pb^{2+}(aq) + SO_4^{2-}(aq) → PbSO_4(s) |
| Barium chloride + sodium carbonate | Barium carbonate | Ba^{2+}(aq) + CO_3^{2-}(aq) → BaCO_3(s) |