Given that at 298K Ksp for AgCNS and AgBr are 1.0 × 10−12 and 5.0 × 10−13 respectively. This data alone is sufficient to calculate the simultaneous solubility of AgCNS and AgBr - True or False?
True
First, let us write down the reactions:
AgCNS (s) ⇌ Ag+ (aq) + CNS− (aq)
It is a binary salt - AgCNS (s). The same can be said about AgBr (s)
AgBr (s) ⇌ Ag+ (aq) + Br− (aq)
It is given that these two, otherwise separate equilibria are existing simultaneously. We see that there is a common ion. But here the common ion effect will not be applicable. Why? Technically, there are just three ions and two solid in solution. That s a better approach to take.
If the solubility of AgCNS (s) is x and the solubility of AgCNS (s) is y, we have
Net [Ag+] = x + y
[CNS−] = x and [Br−] = y
Ksp (AgSCN) = [Ag+][CNS−] = (x+y)x ---------- (1)
& Ksp (AgBr) = [Ag+][Br−] = (x+y)y ------------(2)
We have been given the values of Ksp (AgSCN) and Ksp (AgBr)
So we have two equations and two variables. But it would be simpler to divide (1) by (2) and eliminate (x+y) here to expedite calculation.
Dividing equation (1) by equation (2), we get
xy = 2
Now we can eliminate x in equation (1) and get a quadratic in y
(2y + y)2y = 10−12
Solving y = 4.08 × 10−7 M
Thus Solubility of AgBr = 4.08 × 10−7 M {y > 0}
Substituting the value of y = 4.08 × 10−7 M in (1), and solving the quadratic in x,
We get x = solubility of AgSCN = 8.16 × 10−7 M { only positive value} So the answer is true. But we don't need to calculate the solubilities .