TEACHING LABORATORY Chemical Reactions Precipitation Reactions Thermal Decomposition Acid-base Reactions Redox Reactions/ Displacement Neutralisation reaction Displacement reaction VIRTUAL CHEMLAB Preliminary Lab Manual Cation Lab Manual Anion Lab Manual Gas Lab Manual Action of Heat Lab Manual Redox Lab Manual PERFORMANCE LABORATORY The Laboratory Challenge Lab Challenge 1 Lab Challenge 2 Lab Challenge 3 Lab Challenge 4 Lab Challenge 5 The MCQ Challenge Level 1 Level 2 Level 3 ChemQuest WebQuest   SOLUBILITY TABLE     Solid/Salt Solubility in Water Application in QA Nitrates All nitrates are soluble. This means that any ion, when combined with the nitrate ion in solution, will not precipitate. Sodium, potassium and ammonium salts All sodium, potassium and ammonium salts are soluble. This means that any ion, when combined with the sodium, potassium and ammonium ion in solution, will not precipitate. Sulphates All sulphates are soluble except for BaSO4, CaSO4 and PbSO4. When a solution containing barium, calcium, or lead(II) ions are mixed with sulphate ions, a precipitate will be formed. Chlorides All chlorides are soluble except for AgCl, PbCl2. When solutions containing silver or lead(II) ions are mixed with sulphate ions, a precipitate will be formed. Carbonates All carbonates are insoluble except for Na2CO3, K2CO3 and (NH4)2CO3. Any cation except NH4+ and Group I cations e.g. Na+, K+, and will combine with carbonate ions in solution to form a precipitate. Oxides and Hydroxides All oxides and hydroxides are insoluble except for Na2O, K2O, NaOH, KOH and Ca(OH)2 [sparingly soluble]. Most cations except NH4+ and Group I cations e.g. Na+, K+, and will combine with hydroxide ions in solution to form precipitates.

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