Question #1b658
1 Answer
Apr 24, 2016
The solution is to select an ion that will form a precipitate or gas with one of the ions while leaving the other in solution.
Explanation:
A list of useful solubility rules follows:
- All compounds of the ammonium ion (NH4+), and of Alkali metal (Group IA) cations (sodium, potassium, etc.), are soluble.
- All nitrates, perchlorates and acetates (ethanoates) are soluble.
- All chlorides, bromides and iodides are soluble EXCEPT those of silver, lead and mercury(I).
- All sulphates are soluble EXCEPT those of silver, lead, mercury(I), barium, strontium and calcium.
- All carbonates, sulfites and phosphates are insoluble EXCEPT those of ammonium and Alkali metal (Group IA) cations.
- All hydroxides are insoluble EXCEPT those of ammonium, barium and alkali metal (Group I) cations.
- All sulfides are insoluble EXCEPT those of ammonium, Alkali metal (Group I) cations and Alkali earth metal (Group II) cations.
- All oxides are insoluble EXCEPT those of calcium, barium and Alkali metal (Group I) cations; these soluble ones actually react with the water to form hydroxides (hydrolyse).
