1. Salts L.O. State that a salt is produced when the H + ion of an acid is replaced by a metal ion or NH 4 + Describe the reactions of an acid with carbonates, bases and alkalis to form a salt. Understand that a base readily accepts H + ions from an acid

2. Salts Definition: A salt is any chemical compound formed from an acid when a H + ion from the acid has been replaced by a metal ion or another positive ion. Cation is a positively charge ion Anion is a negatively charged ion

3. Examples Sulfuric acid  sulfate salts H 2 SO 4  K 2 SO 4 Hydrochloric acid  chloride salts HCl  NaCl Nitric acid  nitrate salts HNO 3  Ca(NO 3 ) 2

4. Acid Salts Sulfuric acid has two replaceable H + ions and is called a diprotic acid If one H + ion is replaced, an acid salt is formed e.g. H 2 SO 4  NaHSO 4 The acid salt itself can behave like an aicd, because the other H + ion can be replaced to form a conventional salt e.g. NaHSO 4  Na 2 SO 4

5. Formation of salts These are also know as neutralisation reactions The salts are produced by neutralising acids

6. Acid + Carbonate General Equation: acid + carbonate  salt + carbon dioxide + water Example: 2HCl(aq) + CaCO 3 (s)  CaCl 2 (aq) + H 2 O(l) + CO 2 (g) 2H + (aq) + CaCO 3 (s)  Ca 2+ (aq) + H 2 O(l) + CO 2 (g)

7. Acid + Base General Equation: acid + base  salt + water Example: 2HCl(aq) + CaO(s)  CaCl 2 (aq) + H 2 O(l) 2H + (aq) + CaO (s)  Ca 2+ (aq) + H 2 O(l)

8. Acid + Alkalis General Equation: acid + alkali  salt + water Example: HCl(aq) + NaOH(aq)  NaCl(aq) + H 2 O(l) H + (aq) + OH - (s)  H 2 O(l)

9. Ammonium salts + fertilisers Ammonium salts are used as artifical fertilisers They are formed when acids are neutralised by aqeous ammonia NH 3 (aq) + HNO 3 (aq)  NH 4 NO 3 (aq) Ammonium salts contain the ammonium ion, NH 4 +, in place of the metal ions found in most common salts Ammonium nitrate is present in solutions as two ions, NH 4 + (aq) and NO 3 - (aq).

10. Finding the % of ammonia