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

 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

I hope my answer has come to your help. Thank you for posting your question here in .

Icant see the pictures