URGENT: Write the Ksp for the following equilibria: a.) FeS (s) <====> Fe^2+ (aq

Question

URGENT:

Write the Ksp for the following equilibria:

a.) FeS (s) <====> Fe^2+ (aq) + S^2- (aq)

b.) Al(O3)3 (s) <===> Al^3+ (aq) + 3IO3^-

c.) Ba3(PO4)2 (s) <===> 3Ba^2+ (aq) + 2PO4^3- (aq)

d.) Mg(OH2 (s) <====> Mg^2+ (aq) + 2OH^- (aq)

Part II:

Taking into consideration the magnesium hydroxide equilibrium in part D, the amount of solid magnesium hydroxide that dissolves in pure water is going to be _____________ (greater or less) than the amount of solid magnesium hydroxide that dissolves in a 0.01 M Mg(NO3)2 solution.

The amount of solid magnesium hydroxide that dissolves in pure water is going to be _____________ (greater or less) than the amount of solid magnesium hydroxide that dissolves in a 0.01 M NaOH solution.

Explanation / Answer

Assuming you want only the expression for the Ksp values , and if smol/L is the solubility of salt

a)Ksp of FeS = [Fe+2][S-2] = s2

b) Ksp of Al(OH)3 =[Al+3][OH-]3 =sx(3s)3 =27 s4

c) Ksp of barium phosphate = [Ba+2 ]3[PO4-3]2= (3s)3 (2s)2 =108 s5

d) ksp of magesium hydroxide = [Mg+2][OH-1]2 = sx(2s)2 =4s3

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