1. Reactions of chlorine with water and sodium hydroxide.

2. Reaction with water Chlorine reacts slowly with cold water to form a mixture of hydrochloric and chloric (i) acids. Cl 2 + H 2 O ↓ HCl + HOCl

3. Two reactions are going on; 1) ½Cl 2 + H 2 O → HCl + OH - Oxidation N o of chlorine in chlorine molecules is O. Oxidation N o of chlorine in the chloride ion is -1. As the oxidation N o has become less positive chlorine has been reduced. ½Cl 2 + e- → Cl -

4. 2) ½Cl 2 + H 2 O → HOCl + H + Oxidation N o of chlorine in chlorine molecules is O. Oxidation N o of chlorine in the chlorate ion is +1. As the oxidation number has become more positive chlorine has been oxidised. ½Cl 2 + OH - → HOCl + e - As chlorine has been both oxidised and reduced it is said to have disproportionated.

5. Chloric (i) acid decomposes on standing; 2HOCl → 2HCl + O 2 Oxidation N o of chlorine in chlorate ions is +1. Oxidation N o of chlorine in the chloride ion is -1. As the oxidation N o has become less positive chlorine has been reduced. Oxidation N o of oxygen in chlorate ion is -2. Oxidation N o of oxygen in oxygen molecules is 0. As the oxidation No becomes more positive oxygen has been oxidised.

6. Water purification Chloric (i) acid is the reason why chlorine is used in water purification. When it breaks down reactive oxygen atoms are produced that kill bacteria. HOCl → HCl + [O]

7. The potential to kill bacteria must last right up the point of delivery to the consumer. So ammonia is also added, producing chloroamines; Eg; NH 3 + HOCl → NH 2 Cl + H 2 O Chloroamines then slowly release chlorate (i) as they are hydrolysed. NH 2 Cl + H 2 O → NH 3 + HOCl

8. Pros and cons of water purification Chlorine also reacts with organic matter to produce chlorinated organic compounds which increase the risk of cancer. But this increased risk is insignificant when placed against that of consuming contaminated water.

9. Reaction with sodium hydroxide. Chlorine reacts with cold, dilute NaOH to form a mixture of hydrochloric and chloric (i) acids. Cl 2 + 2OH - → Cl - + OCl - + H 2 O Two reactions are involved;

10. Two reactions are going on; 1) ½Cl 2 + H 2 O → HCl + OH - Oxidation N o of chlorine in chlorine molecules is O. Oxidation N o of chlorine in the chloride ion is -1. As the oxidation N o has become less positive chlorine has been reduced. ½Cl 2 + e- → Cl -

11. 2) ½Cl 2 + H 2 O → HOCl + H + Oxidation N o of chlorine in chlorine molecules is O. Oxidation N o of chlorine in the chlorate ion is +1. As the oxidation number has become more positive chlorine has been oxidised. ½Cl 2 + OH - → HOCl + e - As chlorine has been both oxidised and reduced it is said to have disproportionated.

12. Bleach The reaction with sodium hydroxide is used commercially to manufacture household bleach. This is an equimolar solution of sodium chloride and sodium chlorate (i).

13. Action of bleach Chloric (i) acid is the reason why chlorine is used in bleach. When it breaks down reactive oxygen atoms are produced that react with, and bleach, coloured compounds. HOCl → HCl + [O]

14. Reaction with hot, concentrated NaOH. With hot, concentrated sodium hydroxide chlorate (v) ions are produced instead of chlorate (i). 3Cl 2 + 3OH - → ClO 3 - + 5Cl - + 3H + Again two reactions are going on at the same time; 1) Chlorine is reduced; ½Cl 2 + e- → Cl -

15. Oxidation N o of chlorine in chlorine molecules is O. Oxidation N o of chlorine in the chlorate ion is +5. As the oxidation number has become more positive chlorine has been oxidised. 2) ½Cl 2 + 3OH - → ClO 3 - + 3H + + 5e- As chlorine has been both oxidised and reduced in this reaction it is said to have disproportionated.

16. Chlorate (v) ions are also produced slowly when chlorate (i) ions are allowed to stand, or more rapidly when they are heated. 3OCl - → ClO 3 - + 2Cl - Again chlorine is being both oxidised and reduced, so it is disproportionated.