  An aqueous solution contains Ag+, Pb2+, Cu+, and Tl+ with each ion at a concentration of 0.15M. The chloride ion is slowly added to the solution. Using the Ksp information below, determine the order in which the ions would precipitate.AgCl = 1.8 x 10−10TiCl = 1.8 x 10−4PbCl2 = 1.7 x 10−5CuCl = 6.73 x 10−7TlCl = 3.7 x 10−4HgCl2 = 17.91 x 10−18

Question

An aqueous solution contains Ag+, Pb2+, Cu+, and Tl+ with each ion at a concentration of 0.15M. The chloride ion is slowly added to the solution. Using the Ksp information below, determine the order in which the ions would precipitate.

AgCl = 1.8 x 10−10
TiCl = 1.8 x 10−4
PbCl2 = 1.7 x 10−5
CuCl = 6.73 x 10−7
TlCl = 3.7 x 10−4
HgCl2 = 17.91 x 10−18

Step 1

Solubility product may be defined as the product of concentration of products each raised to the power equals to their respective stoichiometric coefficient.

Let’s take an example of AgCl

Dissociation of AgCl will be:

Step 2

Here we have Ag+, Pb+2, Cu+ and Tl+ ions

and solubilty of compounds are given as:

Step 3

Greater the solubility product, more soluble will be the compound.

When chloride ions are added to the beaker containing Ag+, Pb+2, Cu+ and Tl+, reaction starts occur...

Want to see the full answer?

See Solution

Want to see this answer and more?

Our solutions are written by experts, many with advanced degrees, and available 24/7

See Solution
Tagged in

Chemistry 