This document provides information about chemistry revision on acids, bases and salts. It discusses soluble and insoluble salts such as chlorides, sulphates and nitrates. It also describes methods for preparing soluble and insoluble salts, including the titration and solid acid methods. The document further discusses the preparation of copper(II) sulphate through the reaction of copper(II) oxide with sulphuric acid, and provides chemical tests to identify the copper and sulphate ions.

1. Chemistry revision form 5 - 2011 Topic acid base and salt

2. a) Soluble and Insoluble salts Chlorides salts Sulphates salts soluble salts All soluble except All soluble except Insoluble salts

3. a) Soluble and Insoluble salts Nitrate salts carbonate salts soluble salts All soluble Insoluble salts All insoluble except

4. SALT PREPARATION METHODS SOLUBLE SALTS ( must start with ) TITRATION METHOD ( reaction between and ) SOLID AND HOT ACID METHOD For soluble salts of salts For all soluble salts

5. SALT PREPARATION METHODS INSOLUBLE SALT ( the reactants must be in form) METHOD

6. Excess copper (II) oxide powder Acid xxxxxxxxxxxx Heat

7. State the colour of copper (II) oxide powder copper(II) sulphate solution Based on Diagram, name the acid used to prepare copper (II) sulphate.

8. Write the chemical equation for the preparation of copper (II) sulphate. State the reason why copper (II) oxide powder is added until in excess.

9. Describe how to obtain pure crystals from solution of copper (II) sulphate in the beaker above.

10. 0.1 mol of copper (II) sulphate is produced from the reaction between acid and excess copper (II) oxide. Calculate the mass of copper (II) sulphate formed.

11. Describe chemical tests to verify the present of cation in copper (II) sulphate solution.

12. Describe chemical tests to verify the present of anion in copper (II) sulphate solution.

13. Question 3 Preparation of salt Name of method: i.Titration 0.1 mol dm-3 hydrochloric acid method of preparation of salt Experiment 1 25.0 cm3 of 0.2 mol dm-3 sodium hydroxide + phenolphthalein

14. Experiment 11 10 cm3 of 1.0 mol dm-3 lead(II) nitrate solution Excess potassium iodide solution Name of method: Double decomposition (precipitation)

15. b.Experiment 1 i.Name reaction Neutralization ii.Chemical equation NaOH + HCl  NaCl +H 2 O

16. iii. Colour change of phenolpthalein Pink to colourless

17. iv. Calculate Volume of HC l needed Mole of NaOH= 25 x 0.1/1000 =0.005 From the equation, 0.005 mol NaOH  0.005 mol HCl But mole = MV/1000 So V = mole x 1000/M V = 0.005 x 1000/0.1 V = 50Cm 3

18. c. Experiment II i.Name of salt Lead(II) iodide Ii. Write Ionic equation P b 2+ + 2I -  PbI 2

19. Iii How pure salt is obtained from the reaction II? Filter the mixture Rinse residue with distilled water Dry between two filter papers

20. iv. Calculate maximum mass of precipitate X Mole of Pb(NO 3 ) 2 = 10x1 /1000 = 0.01 mol But 0.01 mole Pb 2+  0.01 mole PbI 2 So mass of PbI 2 = mole x mmass = 0.01x(207+ 2(127))g =4.61 g

21. Question 4 Action of heat on salts + Name gas Q CARBON DIOXIDE name of COMPOUND x Copper (ii) carbonate Compound X Copper (II) oxide Gas Q ∆

22. State the colour of COMPOUND X COPPER(II) OXIDE GREEN BLACK

23. (III) Chemical equation for decomposition of compound X CuCO 3  CuO + CO 2 (iv) If copper(II) nitrate is heated to replace compound X, write chemical equation 2Cu(NO 3 ) 2  2CuO+ 4NO 2 + O 2

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