What volume of water is needed to dissolve 0.010 moles of AgCl entirely? The K for AgCl is 1.7x10-10

The volume of water = 766.87 L

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 :

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