Chemistry practicals can seem daunting, but these four core experiments...
Chemistry1,191 views·Updated 16 Jul 2026·4 pagesAQA GCSE Chemistry Practical Experiments for Paper 1
Lena@lena_ftpy
1 / 4
1
of 4
Making Salts
Ever wondered how table salt is actually made in a lab? This practical shows you how to create pure crystals from scratch using a simple acid-base reaction. You'll be combining sulphuric acid with copper oxide to produce beautiful blue copper sulphate crystals.
The process is quite straightforward: heat dilute sulphuric acid gently, then add copper oxide powder until no more fizzing occurs (this means all the acid has reacted). Filter out the leftover copper oxide, then evaporate your solution slowly using a water bath until crystals begin forming.
The key to success is patience during the crystallisation process. Leave your solution in a cool place for at least 24 hours to get proper crystal formation. Pat them dry carefully with filter paper, and you'll have created your first pure salt sample.
Top tip: Add the copper oxide in excess - you'll know you've added enough when the fizzing stops completely. This ensures all your acid has reacted.
2
of 4
Neutralisation
Titration might sound complex, but it's basically just finding out exactly how much acid you need to neutralise a base. You're playing detective to discover the unknown concentration of sulphuric acid using sodium hydroxide solution.
Your main tools are a burette (the tall tube with measurements) and a pipette for precise measuring. Add phenolphthalein indicator to your sodium hydroxide - it'll turn pink and act as your colour-change signal. Slowly drip acid from the burette whilst swirling your flask.
The magic moment is the end point - when the solution suddenly changes from pink to colourless. This tells you the acid and base have perfectly neutralised each other. Record your measurements and repeat until you get concordant results (within 0.1 cm³ of each other).
Remember: Always read the burette from the bottom of the meniscus and add acid drop-by-drop near the end point to avoid overshooting.
3
of 4
Electrolysis
Electrolysis is like using electricity to break apart compounds - think of it as chemical demolition! You'll investigate what happens when electric current passes through aqueous solutions using carbon electrodes.
Set up your circuit with carbon rods as inert electrodes in solutions of copper chloride and sodium chloride. When you switch on the 4V power supply, chemical magic happens. At the positive electrode (anode), chlorine gas bubbles off, whilst at the negative electrode (cathode), different products form depending on your solution.
With copper chloride, you'll see brown copper metal coating the negative electrode. Sodium chloride produces hydrogen gas instead. Use blue litmus paper held with forceps to test for the gases - chlorine will bleach it white.
Safety first: Ensure good ventilation because chlorine gas is toxic. Never let the electrodes touch each other or you'll short-circuit your setup.
4
of 4
Temperature Changes
This practical lets you explore exothermic reactions by measuring temperature changes when acids and alkalis react. You're investigating how the amount of reactants affects the heat energy released during neutralisation.
Use polystyrene cups as your reaction vessel - they're excellent insulators that prevent heat loss to surroundings. Start with 25 cm³ of hydrochloric acid, measure its temperature, then gradually add 5 cm³ portions of sodium hydroxide solution.
Stir gently with your thermometer through the lid hole and record the maximum temperature after each addition. You'll notice the temperature rises as more alkali neutralises the acid, reaching a peak before dropping again when excess alkali cools the mixture.
Key point: Record temperatures quickly after mixing and keep stirring gently for accurate readings. The polystyrene cup acts like a calorimeter to minimise heat loss.
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Chemistry1,191 views·Updated 16 Jul 2026·4 pagesAQA GCSE Chemistry Practical Experiments for Paper 1
Lena@lena_ftpy
Chemistry practicals can seem daunting, but these four core experiments are your gateway to understanding how chemical reactions work in real life. From making crystals to exploring electrolysis, these practicals give you hands-on experience with the fundamental processes that power...
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Making Salts
Ever wondered how table salt is actually made in a lab? This practical shows you how to create pure crystals from scratch using a simple acid-base reaction. You'll be combining sulphuric acid with copper oxide to produce beautiful blue copper sulphate crystals.
The process is quite straightforward: heat dilute sulphuric acid gently, then add copper oxide powder until no more fizzing occurs (this means all the acid has reacted). Filter out the leftover copper oxide, then evaporate your solution slowly using a water bath until crystals begin forming.
The key to success is patience during the crystallisation process. Leave your solution in a cool place for at least 24 hours to get proper crystal formation. Pat them dry carefully with filter paper, and you'll have created your first pure salt sample.
Top tip: Add the copper oxide in excess - you'll know you've added enough when the fizzing stops completely. This ensures all your acid has reacted.
2
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Neutralisation
Titration might sound complex, but it's basically just finding out exactly how much acid you need to neutralise a base. You're playing detective to discover the unknown concentration of sulphuric acid using sodium hydroxide solution.
Your main tools are a burette (the tall tube with measurements) and a pipette for precise measuring. Add phenolphthalein indicator to your sodium hydroxide - it'll turn pink and act as your colour-change signal. Slowly drip acid from the burette whilst swirling your flask.
The magic moment is the end point - when the solution suddenly changes from pink to colourless. This tells you the acid and base have perfectly neutralised each other. Record your measurements and repeat until you get concordant results (within 0.1 cm³ of each other).
Remember: Always read the burette from the bottom of the meniscus and add acid drop-by-drop near the end point to avoid overshooting.
3
of 4Sign up to see the content. It's free!
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Electrolysis
Electrolysis is like using electricity to break apart compounds - think of it as chemical demolition! You'll investigate what happens when electric current passes through aqueous solutions using carbon electrodes.
Set up your circuit with carbon rods as inert electrodes in solutions of copper chloride and sodium chloride. When you switch on the 4V power supply, chemical magic happens. At the positive electrode (anode), chlorine gas bubbles off, whilst at the negative electrode (cathode), different products form depending on your solution.
With copper chloride, you'll see brown copper metal coating the negative electrode. Sodium chloride produces hydrogen gas instead. Use blue litmus paper held with forceps to test for the gases - chlorine will bleach it white.
Safety first: Ensure good ventilation because chlorine gas is toxic. Never let the electrodes touch each other or you'll short-circuit your setup.
4
of 4Sign up to see the content. It's free!
- Access to all documents
- Improve your grades
- Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Temperature Changes
This practical lets you explore exothermic reactions by measuring temperature changes when acids and alkalis react. You're investigating how the amount of reactants affects the heat energy released during neutralisation.
Use polystyrene cups as your reaction vessel - they're excellent insulators that prevent heat loss to surroundings. Start with 25 cm³ of hydrochloric acid, measure its temperature, then gradually add 5 cm³ portions of sodium hydroxide solution.
Stir gently with your thermometer through the lid hole and record the maximum temperature after each addition. You'll notice the temperature rises as more alkali neutralises the acid, reaching a peak before dropping again when excess alkali cools the mixture.
Key point: Record temperatures quickly after mixing and keep stirring gently for accurate readings. The polystyrene cup acts like a calorimeter to minimise heat loss.
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The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.
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