Ionic EquilibriumHard
Question
Let the solubilities of AgCl in pure water, 0.01 M CaCl2, 0.01 M NaCl & 0.05 M AgNO3 be s1, s2, s3 & s4 respectively what is the correct order of these quantities. Neglect any complexation.
Options
A.s1 > s2 > s3 > s4
B.s1 > s2 = s3 > s4
C.s1 > s3 > s2 > s4
D.s4 > s2 > s3 > s1
Solution
Let Ksp of AgCI = x
(a) solubility of AgCl in pure water = s1 = √x (b) solubility of AgCl in 0.01 M CaCl2 = s2 =
(c) solubility of AgCl in 0.01 M NaCl = s3 =
(d) solubility of AgCl in 0.05 M AgNO3 = s4 = 
So s1 > s3 > s2 > s4
(a) solubility of AgCl in pure water = s1 = √x (b) solubility of AgCl in 0.01 M CaCl2 = s2 =
(c) solubility of AgCl in 0.01 M NaCl = s3 =
(d) solubility of AgCl in 0.05 M AgNO3 = s4 = So s1 > s3 > s2 > s4
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