What conditions must be met by [Pb+2] and [Cl- ] for PbCl2 to form? I had to shake it to get it to precipitate. Also, why does PbCl2 dissolve after adding extra water if it is insoluble in water?
PbCl2 is not insoluble. It is slightly soluble in water
Ksp for PbCl2 equals 1.0×10^-4
1.0×10^-4 = [Pb+2][Cl-]^2
PbCl2 solubility is 0.0292 moles/L at 25 C in H2O
The product of the Pb+2 concentration and the square of the Cl^-1 concentration must exceed 1×10^-4 for a precipitate of PbCl2 to form.
[Pb+2][Cl-]^2 must exceed 1.00×10^-4 befiore a precipitate can form.
HCL is hydrochloric acid….Water dissolves all acids. Neutralizes them. Makes no sense.