The concentration of KI and KCl in a certain solution containing both is 0 .001 M each. If 20 mL of this solution is added to 20 mL of a saturated solution of AgI in water. What will happen ? K sp of AgCl = 10 − 10 ; K sp of AgI = 10 − 16

Step-by-step solution

I - solution I = 1 0 - 3 M Cl - solution I = 1 0 - 3 M Ag + solution II = K sp = 1 0 - 8 M I − solution II = K sp = 1 0 - 8 M . on mixing the equal volume of two solutions. I - = 1 0 - 3 + 1 0 - 8 2 = 1 0 - 3 1 + 1 0 - 5 2 ≈ 5 × 10 - 4 M Cl - = 1 0 - 3 2 M Ag + = 10 - 16 5 × 10 - 4 = 2 × 10 - 13 K IP AgI = 1 0 - 8 2 × 1 0 - 3 1 + 1 0 - 5 2 ≈ 1 0 - 1 1 4 > K sp AgI K IP AgCl = 1 0 - 8 2 × 1 0 - 3 2 ≈ 1 0 - 1 1 4 < K sp AgCl Hence AgI will ppt, but AgCl will not ppt.