Answer the following questions about the solubility of AgCl(s). The value of K_sp for AgCl(s) is 1.8 — Equilibrium Chemistry Question

K_sp = [Ag⁺][Cl^-]
Let x = [Ag⁺] = [Cl^-]
Then 1.8 × 10^-10 = (x)(x) ⇒ x = √(1.8 × 10^-10)
x = [Ag⁺] = 1.3 × 10^-5 M

1 point is earned for the correct K_sp expression and indication that the two ions have equal concentrations.
1 point is earned for correct calculation of the value of [Ag⁺].

1.8 × 10^-10 = [Ag⁺] × (0.54) ⇒ [Ag⁺] = 3.3 × 10^-10 M

1 point is earned for the correct answer with supporting work. || An increased [Cl^-] will decrease the solubility of AgCl(s) since the K_sp is a product of the [Ag⁺] and [Cl^-]. (This is an example of the common ion effect.)

1 point is earned for a correct explanation.