Answer to Question #309426 in Inorganic Chemistry for Qataria

Question

. If the Ksp for the given reaction is 1.8 x 10 ^-10  at 25⁰ C, what is the equilibrium concentration of chloride ions, [Cl-]_eq, expressed in 10^-5 M? 

AgCl_(s)      Ag⁺_(aq) + Cl^-_(aq)

Answer 1

Solution:

AgCl(s) ⇌ Ag⁺(aq) + Cl^–(aq)

__S________S________S____

Thus,

[Ag⁺] = [Cl^–] = S

The K_sp expression for AgCl(s) is:

K_sp = [Ag⁺] × [Cl^–]

Therefore,

1.8×10^–10 = [S] × [S] = S²

[Cl^–] = S = (1.8×10^–10)^1/2 = 0.0000134 M = 1.34×10^–5 M

[Cl^–] = 1.34×10^–5 M

Answer: The equilibrium concentration of chloride ions (Cl^–) is 1.34×10^–5 M