1. Preparation of a pure, dry sample of a soluble salt from an insoluble oxide or carbonate.
What type of reaction is this?
Draw and explain the 3 main steps to this procedure – highlighting what you would observe at each stage.
Describe one safety concern in this practical procedure and how we control the risk.
Write a balanced symbol and word equation for the reaction to produce copper sulfate from an acid and a carbonate.
What does adding the base or carbonate to excess mean? And why do we do it?
What is the purpose of heating the salt solution that is produced?
The purity of the crystals could be tested by finding the melting point. How do impurities affect the melting point?

2. Finding the reacting volumes of solutions of acid and alkali by titration.
Name the type of reaction that takes place between an acid and the alkali.
Using 3 main steps, describe and explain what you would do at each step and why that step is important. You may include diagrams.
Why is a burette used to measure the volume of one of the solutions instead of a measuring cylinder?
What safety precautions should you take when carrying out this experiment and why?
Why do we do a trial run before we do a more precise titration?
Write a balanced symbol and word equation for the reaction that is occurring here.
Explain why an indicator is necessary but why universal indicator is not suitable to use in a titration?
Why is it important to swirl the conical flask during the titration?
Why is it important to repeat the titration?
Chemistry only

3. Investigate what happens when aqueous solutions are electrolysed using inert electrodes.
Draw a diagram of the set up and label the equipment used.
Predict the products of the electrolysis of aqueous sodium chloride.
Describe what you would expect to see at each electrode How could you test for the products?
Explain why the sodium chloride must be dissolved or molten for this to work.
Name one hazard associated with this practical and describe how you would control it.
Write the half equations for the reactions at each electrode.
Describe how you could extend this investigation to investigate the hypothesis that the reactivity series is linked to the ability of a metal ion in solution to deposit on an inert electrode.

4. Investigate the variables that affect temperature changes in reacting solutions.
If we were to investigate the reaction between an alkali an acid and an alkali state 4 variables that could affect the temperature change.
Explain why it is important to just change one variable at a time.
List the equipment that you would need for this experiment and explain why each piece is needed.
What is the main limitation in this experiment.
Suggest an improvement to the method to reduce this problem.
State 3 other reactions that could be used for this experiment.
Describe how you would measure the amount of energy released by a chemical reaction.

5. Investigate how changes in concentration affect the rates of reactions by a method involving measuring the volume of a gas produced and a method involving a change in colour or turbidity.
Suggest three ways of measuring the rate of a reaction.
In a reaction investigating the rate of reaction between magnesium ribbon and hydrochloric acid identify the independent variable, dependent variable and suggest two control variables.
Explain why a gas syringe would be used in the experiment?
Why is it important that the bung is inserted quickly after the magnesium is added to the flask.
Explain how the rate of reaction can be calculated from a graph.
In this experiment the reaction is followed by observing a mark through a solution and noting when it disappears. Give two things about the mark that must be kept the same.

6. Investigate how paper chromatography can be used to separate and tell the difference between
coloured substances.
Why is it important to draw the start line in pencil?
Explain why the level of solvent should be below the ink spots.
Which is the mobile phase? Which is the stationary phase?
What is meant by the term ‘solvent front’?
How is a Rf value calculated and how can it be used?
Suggest why Rf values change when a different solvent is used.
How could you improve the reliability of the results?

7. Using chemical tests to identify ions.
Chemistry only
Using chemical tests to identify ions.
Describe the tests to distinguish hydrogen, oxygen, carbon dioxide and chlorine.
Describe how to carry out a flame test. What type of ions are identified with this method?
Dilute solutions of iron (III) chloride and iron (III) sulfate are both pale brown. Explain how you could distinguish between them.
Three ions in solution all give a white precipitate when sodium hydroxide is added. Identify the ions and explain how you could distinguish between them.
Give an example of an instrumental method and suggest why this method has an advantage over chemical tests.
Identify some safety precautions you should take when carrying out chemical tests to identify ions.

8. Analysis and purification of water samples from different sources, including pH, dissolved solids and
distillation.
How could you test a water sample for the presence of sodium and chloride ions?
Write an equipment list for the distillation of water and explain what each piece of equipment is for.
Describe how you could use distillation to purify a sample of a water.
When you distil a water sample it is essential that the delivery tube is above the level of the filtrate. Explain why.
Suggest two ways of testing the purity of water.
What safety precautions are used in the practical?