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Katherine Wu 1H
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Joined: Fri Aug 30, 2019 12:15 am
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Postby Katherine Wu 1H » Wed Jan 15, 2020 5:53 pm

How do you use equilibrium constants to predict solubility?

Asha Agarwal 1E
Posts: 51
Joined: Fri Aug 30, 2019 12:16 am

Re: solubility

Postby Asha Agarwal 1E » Wed Jan 15, 2020 6:24 pm

If you have an equilibrium constant and initial concentrations, you can find the equilibrium concentrations using ICE tables and the quadratic equation. Knowing the equilibrium concentrations, you can see how much of the solute(reactants) dissociated or reacted to form the products.

Angela Patel 2J
Posts: 110
Joined: Sat Aug 24, 2019 12:17 am

Re: solubility

Postby Angela Patel 2J » Wed Jan 15, 2020 10:52 pm

For example for an acid, we can find how much will dissociate in water by making the ICE table and finding the equilibrium concentration of the hydronium ion

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Joined: Fri Aug 09, 2019 12:17 am

Re: solubility

Postby 805307623 » Thu Jan 16, 2020 3:22 pm

Solubility equilibrium is based on solids dissolving in water to produce the basic particles that form them.
Molecular solids dissolve into individual aqueous molecules, and Ionic solids dissociate into their respective cations and anions. The solubility equilibrium constant (Ksp) is the product of the concentrations of ions in a saturated solution at equilibrium. Each concentration is raised to the power of the coefficient of its ion, however, the solubility product equilibrium constant has no denominator because the reactant is a solid.

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