Asolution has a pb2+  concentration of 1.9 x 10-3  m, and an f-1  concentration of 3.8 x 10-3  m. the value of ksp  for pbf2  at room temperature is 4 x 10-8. will this solution form a precipitate? the solubility equilibrium equation is as follows..yesno

We are going to get the value of Qsp and compare it with the Ksp value:

when Qsp is the concentration of the initial products:

Qsp = [Pb2+][F-]^2

when the [Pb2+] = 1.9 x 10^-3

and [F-] = 3.8 x 10^-3

by substitution:

∴Qsp = (1.9 x 10^-3) * (3.8 x 10^-3)^2

           = 2.7 x 10^-8 

when Ksp = 4 x 10^-8

so Qsp < Ksp

∴ precipitate will not be formed 

c. electrical charges of ionic bonds.

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