Shared flowchart

Chemistry · L4 · Solubility equilibrium: dissolution and the common ion effect

Sign in to clone

How a sparingly-soluble salt's dissolution equilibrium responds to pure water versus a solution already containing a common ion.

by @openstemUpdated Chemistry
Solid MX(s)MX(s) ⇌ M⁺(aq) + X⁻(aq)Ksp = [M⁺][X⁻]Dissolved in pure water[M⁺] = [X⁻] = sDissolved in solution withcommon ion X⁻ already presentEquilibrium shifts LEFT(Le Chatelier)Molar solubility s decreasesbelow the pure-water values = √Ksp(baseline solubility)

We use privacy-friendly product analytics (no session recording, PII masked) to improve OpenStem. Load analytics? Privacy Policy