Ionic EquilibriumHard
Question
The concentration of hydroxyl ion in a solution left after mixing 100 mL of 0.1 M MgCI2 and 100 mL of 0.2 M NaOH (KSP of Mg(OH)2 = 1.2 × 10-11):
Options
A.2.88 × 10-3
B.2.88 × 10-2
C.2.88 × 10-4
D.2.88 × 10-5
Solution
MgCl2 + 2NaOH → Mg(OH)2 + 2NaCl
mm before 10 20 0 0
reaction 0 0 10 20
Thus, 10 m mole of Mg(OH)2 are formed. The product of [Mg2+][OH-]2 is therefore
= 5 √ 10-4 which is more than KSP of Mg(OH)2. Now solubility(s) of Mg(OH)2 can be derived by
KSP = 4s3
∴ s =
= 1.4 × 10-4 M
∴ [OH-] = 2s = 2.88 × 10-4 M
mm before 10 20 0 0
reaction 0 0 10 20
Thus, 10 m mole of Mg(OH)2 are formed. The product of [Mg2+][OH-]2 is therefore
= 5 √ 10-4 which is more than KSP of Mg(OH)2. Now solubility(s) of Mg(OH)2 can be derived byKSP = 4s3
∴ s =
= 1.4 × 10-4 M∴ [OH-] = 2s = 2.88 × 10-4 M
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