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?
2 Answers
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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.
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HCL is hydrochloric acid….Water dissolves all acids. Neutralizes them. Makes no sense.
