I don't know of any way to do this short of solving three problems. You can eliminate 1 of the Fe/Al hydroxides; i.e., Al(OH)3 is more soluble than Fe(OH)3 because Ksp is larger. However, you may not compare Ksp directly for purposes of determining solublility with salts that are not the same kind; i.e. 1:1 as in AgCN, 1:2 as in Sn(OH)2 and 1:3 as in Al(OH)3.
For AgCN, solublity is sqrt(Ksp)
Can you handle the other two?
what is the most soluble salt of the following set?
a) AgCN with Ksp=6.0 x 10^-17
b) Al(OH)3 with Ksp = 1.9x10^-33
c) Fe(OH)3 with Ksp = 2.6 x 10^-39
d) Sn(OH)2 with Ksp = 1.6 x 10^-19
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