Ionic EquilibriumHard
Question
The solubility product Mg(OH)2 in water at 25oC is 2.56 × 10-13(mol/lt)3 while that of Al(OH)3 is 4.32 × 10-34 (mol/lt)4. If s1 and s2 are the solubilities of Mg(OH)2 and Al(OH)3 in water in mol/lt at 25oC, what is the ratio, s1/s2 ?
Options
A.2 × 105
B.2 × 104
C.3 × 106
D.3 × 103
Solution
Ksp of Mg (OH)2 = 2.56 × 10-13
4 s13 = 2.56 × 10-13 ⇒ s1 = 4 × 10-5 M
Ksp of Al (OH)3 = Ksp = 4.32 × 10-34
27 s24 = 4.32 × 10-34 ⇒ s2 = 2 × 10-9 M
= 
= 2 × 104
4 s13 = 2.56 × 10-13 ⇒ s1 = 4 × 10-5 M
Ksp of Al (OH)3 = Ksp = 4.32 × 10-34
27 s24 = 4.32 × 10-34 ⇒ s2 = 2 × 10-9 M
= = 2 × 104 Create a free account to view solution
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