consider the equilibrium reaction: pbcro4(s) <--> pb^2+ (aq) +cro4^2- (aq). A saturated solution of lead chromate, pbcro4 has a lead ion concentration of 1.4 x 10^-7 m. what is the value of the solubility product ksp for lead chromate?
See your post above.
.......PbCrO4(s) ==> Pb^2+ + CrO4^2-
E.......solid.......1.4E-7...1.4E-7
Substitute into the Ksp expression and solve for Ksp.
To find the solubility product constant (Ksp) for lead chromate (PbCrO4), we need to use the concentration of lead ions in the saturated solution.
The balanced equation for the equilibrium reaction is:
PbCrO4(s) ⇌ Pb2+(aq) + CrO42-(aq)
From the equation, we can see that the stoichiometric coefficient of PbCrO4 is 1, meaning that 1 mole of PbCrO4 produces 1 mole of Pb2+ ions.
Therefore, if the concentration of Pb2+ ions is 1.4 x 10^-7 M, then the concentration of PbCrO4 is also 1.4 x 10^-7 M.
Using the equation for the solubility product expression (Ksp), we have:
Ksp = [Pb2+][CrO42-]
Since the stoichiometric coefficient for both Pb2+ and CrO42- is 1, the concentrations can be directly substituted into the Ksp expression.
Thus, Ksp = (1.4 x 10^-7) x (1.4 x 10^-7)
Calculating this:
Ksp = 1.96 x 10^-14
Therefore, the value of the solubility product (Ksp) for lead chromate (PbCrO4) is 1.96 x 10^-14.
To calculate the solubility product constant (Ksp) for lead chromate (PbCrO4), we need to first write the balanced chemical equation for the dissolution of PbCrO4:
PbCrO4(s) ⇌ Pb2+(aq) + CrO42-(aq)
The solubility product constant (Ksp) expression for this reaction is:
Ksp = [Pb2+][CrO42-]
Given that the concentration of Pb2+ is 1.4 x 10^-7 M, we can substitute this value into the Ksp expression:
Ksp = (1.4 x 10^-7)([CrO42-])
Now, we need to find the concentration of CrO42-. To do this, we utilize the stoichiometry of the balanced equation. Since the stoichiometric coefficient of PbCrO4 is 1, it dissociates to give 1 mol of Pb2+ and 1 mol of CrO42-, so their concentrations are the same:
[CrO42-] = 1.4 x 10^-7 M
Substituting this concentration back into the Ksp expression:
Ksp = (1.4 x 10^-7)(1.4 x 10^-7)
Ksp = 1.96 x 10^-14
Therefore, the value of the solubility product constant (Ksp) for lead chromate is 1.96 x 10^-14.