Question

How would the molar solubility of barium sulfate be impacted if it were to be dissolved in 0.010 M CaSO4 (with no other change in conditions)?

A. It would increase

B. It would stay the same

C. It would decrease

D. There is not enough information to provide an answer

Answer 1

ksP FOR BaSO4= [Ba+2] [SO4-2] =

let x= [Ba+2]

then x²=1.1*10^-10, x= 1.0488*10-5 M/L

[SO4-]2 = 1.0488*10-5

when 0,01m CasO4 is dissolved

CaSO4-----> Ca+2 +SO4-2

KSp =2.4*10-5

y²= 2.4*10-5, where y= [Ca+2] =[SO4-]2

y= 0.004899M

[SO4-2] =0.004899

      BaSO4                                 Ba+2                SO4-2

initial                                            0                       0.004899

change                                                     x                                x

equilibrium                                                x                          0.004899+x

KSp = x*(x+0.004899)= 1.1*10^-10, where x= solubility of BaSO4

when solved using excel,. x = 2.2*10^{- 8} M. The solubility will decrease ( C is correct)