CCEA GCSE Chemistry
CCEA GCSE Chemistry 1.10 Solubility Exam Questions
Free CCEA GCSE Chemistry revision for 1.10 Solubility: what you need to know, common mistakes and exam-style questions with answers. Covers saturated solutions, solubility in g per 100 g of water, solubility curves and how temperature affects solids and gases.
Practise 1.10 Solubility with past papers
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About CCEA GCSE Chemistry 1.10 Solubility
Solubility is the final topic of Unit 1 in CCEA GCSE Chemistry. It defines the key terms solute, solvent, solution and saturated solution, and expresses solubility as the mass of solute that dissolves in 100 g of water at a stated temperature. You need to plot and read solubility curves, calculate solubility from experimental data and work out the mass of crystals that forms when a saturated solution is cooled. The topic also explains why most solids become more soluble as temperature rises while gases become less soluble. It links to crystallisation in salt preparation and chemical analysis. Examiners commonly set solubility curve calculations and expect correct units.
What you need to know
- Key terms A solute dissolves in a solvent to form a solution. A soluble substance dissolves; an insoluble one does not. A saturated solution contains the maximum mass of solute that can dissolve at that temperature.
- Solubility Solubility is the maximum mass of solute that dissolves in 100 g of water at a given temperature, measured in g per 100 g water. To scale: solubility = mass of solute / mass of water x 100.
- Solubility curves Plot solubility against temperature with a smooth curve. Read off the solubility at a temperature, or the temperature at which a solution becomes saturated. The steeper the curve, the more the solubility changes with temperature.
- Crystals on cooling When a saturated solution is cooled, the solute that can no longer stay dissolved forms crystals. Mass of crystals = solubility at higher temperature - solubility at lower temperature (for 100 g water), scaled for the actual mass of water.
- Gases Gases become less soluble as temperature increases, which is why fizzy drinks go flat faster when warm and why warm water holds less dissolved oxygen for fish.
- Measuring solubility Make a saturated solution at a known temperature, weigh a portion of it, evaporate the water and weigh the solid left. The mass of water is the mass of solution minus the mass of solid.
Common mistakes in 1.10 Solubility
- Giving solubility in grams only. Always include per 100 g of water and the temperature.
- Forgetting to scale when the mass of water is not 100 g.
- Saying all substances become more soluble when heated. Gases become less soluble at higher temperatures.
- Joining points on a solubility curve with straight lines. Draw a smooth curve of best fit.
- Using the mass of solution instead of the mass of water in calculations.
Try three 1.10 Solubility exam-style questions
1. Define the term saturated solution. (2 marks)
Show the mark scheme answer
A solution that contains the maximum mass of solute that can dissolve; at a particular temperature.
2. 22 g of a salt dissolved in 40 g of water to form a saturated solution at 30 °C. Calculate the solubility of the salt at 30 °C. (2 marks)
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22 / 40 x 100; = 55 g per 100 g water.
3. The solubility of potassium nitrate is 110 g per 100 g water at 60 °C and 32 g per 100 g water at 20 °C. Calculate the mass of crystals formed when a saturated solution in 50 g of water is cooled from 60 °C to 20 °C. (3 marks)
Show the mark scheme answer
Per 100 g water: 110 - 32 = 78 g; for 50 g of water: 78 / 2; = 39 g.
1.10 Solubility FAQs
What does CCEA GCSE Chemistry 1.10 Solubility cover?
It covers solutes, solvents and saturated solutions, solubility in g per 100 g of water, solubility curves and calculations, and how temperature affects the solubility of solids and gases.
Which unit is 1.10 Solubility examined in?
It is examined in the Unit 1 written paper, Structures, Trends, Chemical Reactions, Quantitative Chemistry and Analysis.
What calculations come up on solubility?
Expect to scale masses to 100 g of water, read values from solubility curves and work out the mass of crystals formed when a saturated solution cools. Always show the scaling step.
