Question

What volume of water is needed to dissolve 0.010 moles of AgCl entirely?

The K for AgCl is 1.7x10-10

Answer 1

The volume of water = 766.87 L

Further explanation

Given

The K for AgCl is 1.7x10⁻¹⁰

Required

the volume of water

Solution

AgCl dissolves in water to form ions(s=solubility)

AgCl ⇒ Ag⁺ + Cl⁻

s s s

K AgCl = [Ag⁺] [Cl⁻]

K AgCl = (s) (s) = s²

1.7x10⁻¹⁰ = s²

s=1.304 x 10⁻⁵ mol/L

The solubility of AgCl in water = 1.304 x 10⁻⁵ mol/L

So for 0.01 moles of AgCl, water needed :

`\tt (0.01)/(1.304* 10^(-5))=766.87~L`