Concentration of Solutions — GCSE Chemistry Revision
Revise Concentration of Solutions for GCSE Chemistry. Step-by-step explanation, worked examples, common mistakes and exam-style practice aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP.
At a glance
- What StudyVector is
- An exam-practice platform with board-aligned questions, explanations, and adaptive next steps.
- This topic
- Concentration of Solutions in GCSE Chemistry: explanation, examples, and practice links on this page.
- Who it’s for
- Students revising GCSE Chemistry for UK exams.
- Exam boards
- Practice is aligned to major specifications (AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP).
- Free plan
- Sign up free to use tutor paths and feedback on your answers. Free access is 3 days uncapped, then 30 min practice/day. Pricing
- What makes it different
- Syllabus-shaped practice and progress tracking—not generic AI answers.
Topic has curated content entry with explanation, mistakes, and worked example. [auto-gate:promote; score=70.6]
Next in this topic area
Next step: Percentage Yield
Continue in the same course — structured practice and explanations on StudyVector.
Go to Percentage YieldWhat is Concentration of Solutions?
Concentration tells us how much of a substance (solute) is dissolved in a certain volume of a solvent. It is usually measured in grams per decimetre cubed (g/dm³) or moles per decimetre cubed (mol/dm³). A concentrated solution has a large amount of solute in a small amount of solvent.
Board notes: Concentration calculations are a higher-tier topic for all exam boards. You must be comfortable with both g/dm³ and mol/dm³ and be able to convert between them. Titration calculations also rely heavily on this knowledge.
Step-by-step explanationWorked example
To find the concentration in mol/dm³ of a solution made by dissolving 4g of NaOH (Mr = 40) in 250 cm³ of water: 1. Moles of NaOH = 4g / 40 = 0.1 mol. 2. Volume in dm³ = 250 cm³ / 1000 = 0.25 dm³. 3. Concentration = 0.1 mol / 0.25 dm³ = 0.4 mol/dm³.
Practise this topic
Jump into adaptive, exam-style questions for Concentration of Solutions. Free to start; sign in to save progress.
Common mistakes
- 1Forgetting to convert volumes from cm³ to dm³. Remember that 1 dm³ = 1000 cm³, so you must divide cm³ by 1000.
- 2Confusing the terms solute, solvent, and solution. The solute is what dissolves, the solvent does the dissolving, and the solution is the final mixture.
- 3Using the wrong formula. For concentration in g/dm³, use Mass / Volume. For mol/dm³, use Moles / Volume.
Concentration of Solutions exam questions
Exam-style questions for Concentration of Solutions with mark-scheme style solutions and timing practice. Aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP specifications.
Concentration of Solutions exam questionsGet help with Concentration of Solutions
Get a personalised explanation for Concentration of Solutions from the StudyVector tutor. Ask follow-up questions and work through problems with step-by-step support.
Open tutorFree full access to Concentration of Solutions
Sign up in 30 seconds to unlock step-by-step explanations, exam-style practice, instant feedback and on-demand coaching — completely free, no card required.
Try a practice question
Unlock Concentration of Solutions practice questions
Get instant feedback, step-by-step help and exam-style practice — free, no card needed.
Start Free — No Card NeededAlready have an account? Log in
Step-by-step method
Step-by-step explanation
4 steps · Worked method for Concentration of Solutions
Core concept
Concentration tells us how much of a substance (solute) is dissolved in a certain volume of a solvent. It is usually measured in grams per decimetre cubed (g/dm³) or moles per decimetre cubed (mol/dm³…
Frequently asked questions
What is a saturated solution?
A saturated solution is one in which the maximum amount of solute has been dissolved in a solvent at a given temperature. No more solute can be dissolved.
How does temperature affect concentration?
For most solid solutes, increasing the temperature of the solvent increases the amount of solute that can dissolve, allowing for a more concentrated solution to be made.