The ksp of agcl is 1.8 × 10–10. how do you know that mixing equal amounts of 0.04m solution of agno3 and 0.002m solution of nacl will lead to the formation of a precipitate?
a. [ag+]×[cl–] = ksp agcl
b. [ag+]×[cl–] < ksp agcl
c. [ag+]×[cl–] > ksp agcl

Explanation:

Ksp is the product solubility constant.

The solubility equation for AgCl is:

The Ksp expression is:

Since Ksp = 1.8 ×  10⁻¹⁰, at equilibrium  [Ag⁺] [Cl⁻] = 1.8 ×  10⁻¹⁰.

When AgNO₃ dissolves in water it completely ionizes into Ag⁺ and NO₃⁻.

When NaCl dissolves in water it completely inoizes into Na⁺ and Cl⁻.

Uisng the molarity formula, M = n / V, you get n = M × V.

So, a volume V of a 0.04 M solution of AgNO₃ will yield 0.04V moles of Ag⁺ and the same volume V of a 0.002 M solution of NaCl will yield 0.02V moles of Cl⁻⁻

So the concentrations will be:

And the product of the two concentrations will be:

That product is much greater than 1.8 ×  10⁻¹⁰ meaning that the concentrations are higher than the equilibrium concentrations and the mixture will lead to the formation of a precipitate.

The option c., [Ag⁺] × [Cl⁻] > Ksp AgCl, describes that situation.