Question

At a certain temperature, the solubility of strontium arsenate, Sr3(AsO4)2, is 0.0540 g/L. What is the Ksp of this salt at this temperature

Answer 1

 Get into moles first. .0590 grams over 540.8 grams per mole = 1.09 x l0^-4 moles 

Sr3(As04)2 = 3 Sr++(aq) plus 2 As04^-3(aq) 

Ksp = (Sr++)^3(As04^-3)^2 

(Sr++) = 3 X l.09 x l0^-4 = 3.27 x l0^-4 

(As04^-3) = 2 x l.09 x l0^-4 = 2.18 x l0^-4 

Ksp = (3.27 x l0^-4)^3 (2.18 x l0^-4)^2 which equals 1.66 x 10^-18th


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