Equilibrium

Chemistry · Class 11

Simulation · Chemistry · Class 11

Which salt dissolves more?

"Which salt dissolves more?" is a free, interactive Class 11 Chemistry simulation for NEET and JEE, built on the NCERT section "Solubility equilibria of sparingly soluble salts" in Equilibrium. A beaker of a sparingly soluble salt dissolves until the ionic product reaches Ksp; formula type sets Ksp = xˣyʸS^(x+y), and a common-ion slider pushes solid back out. NEET has asked about this idea 5 times in 10 years of papers. JEE Main asked 52 questions from this chapter across the 42 shifts Lumi has analysed (2017–2026).

From the lesson Solubility equilibria of sparingly soluble salts in Equilibrium. Change the values and watch what happens.

Which salt dissolves more?Chemistry · Class 11

What it shows

NCERT § "Solubility Equilibria of Sparingly Soluble Salts"

A beaker of a sparingly soluble salt dissolves until the ionic product reaches Ksp; formula type sets Ksp = xˣyʸS^(x+y), and a common-ion slider pushes solid back out.

Controls

4 to try

  • Segmentedsalt type MX / MX2 / M2X / M3X
  • Sliderlog Ksp −20 to −4
  • Slidercommon ion added 0–0.1 M
  • SliderpH 2–12 (hydroxide salts)

Try this

Show that AgCl (Ksp 1.8×10⁻¹⁰) is less soluble than Ag2CrO4 (Ksp 1.1×10⁻¹²) by reading S for both; goal checks S values.

Common mistake

Ksp = S² for every salt; comparing solubility by Ksp across different formula types.

In NEET

10 years of papers

Asked 5 times in 10 years of NEET.

See the past questions: pH and Buffer Solutions, Equilibrium (chapter)

In JEE Main

42 shifts analysed

52 questions from Equilibrium across the 42 JEE Main shifts Lumi has analysed (2017–2026).

See the past questions

The idea behind it

NCERT § "Solubility Equilibria of Sparingly Soluble Salts"

  • For a sparingly soluble salt in contact with its saturated solution, the product of ion concentrations, each raised to its stoichiometric power, is the solubility product Ksp.
  • For BaSO₄ ⇌ Ba²⁺ + SO₄²⁻, Ksp = S² where S is the molar solubility.
  • For a general salt MₓXᵧ, Ksp = xˣ yʸ S^(x+y); for M₂X, Ksp = 4S³, and for MX₂ (like CaF₂), also 4S³.
  • If the ionic product in a solution exceeds Ksp, precipitation occurs; if it is less, the solution is unsaturated and more solid can dissolve.
  • A common ion lowers the solubility of a sparingly soluble salt; this is used to purify common salt by passing HCl gas through its saturated solution, which precipitates NaCl.
  • Salts of weak acids become more soluble at lower pH, because the anion is removed by protonation.
  • Compare the solubility of salts by comparing S, not Ksp directly, unless they have the same formula type.

Questions

5 answers

What does the "Which salt dissolves more?" simulation show?
A beaker of a sparingly soluble salt dissolves until the ionic product reaches Ksp; formula type sets Ksp = xˣyʸS^(x+y), and a common-ion slider pushes solid back out.
What mistake does the "Which salt dissolves more?" simulation fix?
A common mistake it clears up: ksp = S² for every salt; comparing solubility by Ksp across different formula types.
Has NEET asked about this idea?
Yes. NEET has asked about this idea 5 times in 10 years of papers.
Does JEE Main ask questions from Equilibrium?
Yes. JEE Main asked 52 questions from this chapter across the 42 shifts Lumi has analysed (2017–2026).
Is this simulation free?
Yes. It is free and runs in the browser on a phone or a laptop. It belongs to the lesson "Solubility equilibria of sparingly soluble salts" in Equilibrium (Class 11 Chemistry).

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