Ionic equilibrium and solubility laboratory
Compare Qsp with Ksp, add a common ion and predict when a precipitate forms.
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Explanation mode
supersaturated
Description of this simulation
Qsp = 1.000e-6, Ksp = 1.800e-10; the solution is supersaturated.
Quick test · 3 questions
- Qsp
- 1.0000e-6
- Ksp
- 1.8000e-10
- Saturation state
- supersaturated
- Precipitate predicted?
- Yes
Learning guide
- Learning objective
- Predict dissolution or precipitation from Qsp, Ksp and a common-ion change.
- Core equation
- Qsp = [Mᵐ⁺]^a[Aⁿ⁻]^b; precipitation when Qsp > Ksp
- Why the result changes
- Adding an ion already present raises the ion product and can push a saturated solution toward solid formation.
- Try this challenge
- Start below Ksp and add only enough chloride to cross the precipitation boundary.
- Sources
- IUPAC Solubility Data Series; CRC Handbook
What this model shows — and what it simplifies
Educational ModelThe ion product is compared directly with Ksp using the balanced dissolution stoichiometry.
Where do we see this in real life?
Solubility equilibria explain scale, kidney stones, water softening and selective precipitation analysis.
Explain this result
Scientific review record
Building- Module version
- v1 bundled
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- Last reviewed
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- Academic level
- School
- Reviewer
- Not publicly assigned
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