1. Chromatograph C2 3.7
Put a pencil line on the paper (it’s pencil because ink would run)
Put dots of the substance on the line.
Dip the tip of the paper in the water.
Put lid on beaker (so that the solvent won’t evaporate)
If dots of different inks are at the same level, they have the same substances in them.
Remove paper from the solvent.
Leave for the solvent to evaporate.

2. Weigh the mas of the acid and the conical flask and cotton wool
Measuring rates C2 4
Weigh the mas of the acid and the conical flask and cotton wool
Weigh the mass of the calcium carbonate.
Put the calcium carbonate in the acid and plug it with cotton wool.
Measure the mass lost in a certain amount of time.
This experiment can be used to tell the effect of surface area (using powdered or lumps of calcium carbonate)
This can also be used to tell the effect of concentration of acid.
This can also be used to tell the effect of a catalyst (by adding the catalyst to the experiment)

3. Measure the gas produced in a certain amount of time.
Measuring rates C2 4
Put the calcium carbonate in the acid and plug it with the delivery tube.
Measure the gas produced in a certain amount of time.
This experiment can be used to tell the effect of surface area (using powdered or lumps of calcium carbonate)
This can also be used to tell the effect of concentration of acid.
This can also be used to tell the effect of a catalyst (by adding the catalyst to the experiment)

4. Measuring rates C2 4
Draw an X on a piece of paper.
Heat up hydrochloric acid and sodium thiosulphate to the temperature you need in a water bath.
Add them together.
Measure the time taken for the precipitate to obscure the cross.
You can use this experiment to determine the effect of temperature on rate.

5. Measuring energy changes C2 4.7
Add copper sulphate to a styrofoam cup (it’s an insulator)
Add the lid (to prevent heat loss)
Take the start temperature.
Add zinc powder.
Measure the temperature change.
This is used to measure energy changed in reactions.

6. Reversible reactions C2 4.8
Heat up blue (hydrated) copper sulphate. It will turn white (the water has been removed). This is an endothermic reaction because it has to be continuously heated.
Add water to the white (Anhydrous) copper sulphate. It will turn blue. This is an exothermic reaction because it is the opposite to the forward reaction.
CuSO4.5H2O CuSO4 + 5H2O
Blue hydrated copper sulphate
White anhydrous copper sulphate.

7. C2 5.2 Copper oxide + sulphuric acid  copper sulphate + water

8. Pb(NO3)2(aq) + 2KI(aq)  PbI2(s) + 2KNO3(aq)
C2 5.3 Making insoluble salts
Pb(NO3)2(aq) + 2KI(aq)  PbI2(s) + 2KNO3(aq)
The solid forms a precipitate, which can be separated from the solution by filtration.

9. C2 5.4 Electrolysis of lead bromide
Bromine gas is formed at the positive electrode (the reaction needs to be done in a fume cupboard for this reason) because bromide ions are negative.
Lead metal is formed at the negative electrode because lead ions are positive.
This circuit could make a lightbulb turn on because the ions moving allow electricity to be conducted.

10. C2 5.8 Electroplating
The positive electrode is silver metal. It turns into silver ions and goes into the solution.
The positive electrode will get smaller.
Any impurities will fall to the bottom of the beaker.
The negative electrode is the spoon (made of steel) silver ions will attach to the spoon and become silver metal.
The spoon will be covered in silver.