Describe how to write the Ksp.
2 answers:
b2+ + 2 NO3- + 2 Na+ + 2 I- >> PbI2 (s) + 2 Na+ + 2 NO3-
net ionic
Pb2+ + 2 I- >> PbI2
Ksp = [Pb2+] [I-]^2
Ksp = 7.1 x 10^-9
molar solubility
let x = mol/L of Pb2+ that dissolve . This will give x mol/L Pb2+ and 2x mol/L I-
7.1 x 10^-9 = (x) (2x)^2 = 4x^3
molar solubility = 0.0012 M
~~thanks to google research~~
Answer: Well, for a start Ksp=Ksolubility product, and we use an equilibrium expression. Explanation: For the sparingly soluble salt, MX, we write the equation that represents its dissolution: MX(s)H2O⇌M++X− Ksp=[M+][X−][MX(s)], but MX(s) as A SOLID cannot express a concentration, and thus the expression simplifies to... Ksp=[M+][X−] Usually standard conditions are specified, because a hot solution can generally hold more solute than a cold one. For salts of the form MX2, Ksp=[M2+][X−]2. Ksp have been measured for a host of insoluble, and semi-soluble ionic salts.
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