How to Calculate the Solubility Product of a Salt – Part 1

Solubility equilibrium is a type of dynamic equilibrium that exists when a solid chemical compound is in chemical equilibrium with a solution of that compound.


The solid may dissolve unchanged, with dissociation, or with chemical reaction with another component of the solution, viz., acid, base or salt. Each solubility equilibrium is characterized by a temperature-dependent solubility product which functions like an equilibrium constant.

Question:

Ksp(Ag2C2O4) = 1.29 x 10-11 mol3/L3 at 250C. A solution of K2C2O4 containing 0.152 mol in 500 mL water is shaken at 250C with excess Ag2CO3 till the following equilibrium is reached:

Ag2CO3 + K2C2O4 ⇌ Ag2C2O4 + K2CO3

At equilibrium, the solution contains 0.0358 mol of K2CO3. Assuming the degree of dissociation of K2C2O4 & K2CO3 to be equal, calculate the Ksp(Ag2CO3).

Solution:



Click to enlarge the image

Stirred up by the solubility product❓ Let Chemaficionado know at mychemistryhomework@gmail.com❗

References:

(1)    Wikipedia Contributors. Solubility equilibrium. Wikipedia. https://en.wikipedia.org/wiki/Solubility_equilibrium.

‌(2)    Ncert. Chemistry : Textbook for Class XI - Part.I; National Council Of Educational Research And Training: New Delhi.

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