what is the molar solubility of lead sulfate in 1.0 X 10^-3 M Na2SO4?
The Solubility Product Constant PbSO4
Ksp= 1.8 x 10^-8
The Ksp expression is:
Na2SO4 = [2Na][SO4^-2]
[2Na]=2x
[SO4^-2]=x
Ksp= 1.8 x 10^-8 = (x)(2x)
Ksp= 1.8 x 10^-8 /4x^3
1.8 x 10^-8/4 = x^3
4.5 x 10^-9 = x^3
is this right so far... what do i do next please
No, you have made some wrong assumptions. First, PbSO4 is the insoluble material. Na2SO4 is soluble in water. Second, this is a common ion problem in which the presence of the sulfate ion from Na2SO4 will decrease the solubility of PbSO4.
So what do i do then to solve for the ksp
The problem doesn't ask for you to solve for Ksp. It asks for the solubility of PbSO4 in 1 x 10^-3 M Na2SO4.
PbSO4 ==> Pb^+2 + SO4^=
Ksp = (Pb^+2)(SO4^=) = 1.8 x 10^-8
If solubility of PbSO4 = S (or x if you wish), then (Pb^+) = S and (SO4^=) = S
The Na2SO4 in solution is
Na2SO4 ==> 2Na^+ + SO4^=
Since it is 1 x 10^-3 M in Na2SO4, then (SO4^=) = 1 x 10^-3.
Now set those up in the Ksp expression and solve for S. Remember that the total sulfate is that from the PbSO4 + that form the Na2SO4.
So im solving for two expressions... is that it.
ok I got x^2 = 1.8 x 10^-8 = 1.34 x 10^-4 for PbSO4 is this right
You are solving for the only unknown in the equation, which is S.
Ksp = (Pb^+2)(SO4^-2) = 1.8 x 10^-8
(S)(S + 1E-3)= 1.8 x 10^-8
S =
i subtracted 1E-3 from the 1.8E-8 and it got me a -9.999E-4 then i took the sqrt cause (X)(X) is x^2 and then the calculator told me an error
Ksp = (Pb^+2)(SO4^=) = 1,8 x 10^-8
(Pb^+2) = x
(SO4^=) = x+0.001
(x)(x+0.001) = 1.8 x 10^-8
You can see that this is a quadratic equation and we could solve it as a quadratic. The exact solution is (and I'm switching to y so as not to confuse the x with the times sign),
y^2 + 0.001y = 1.8 x 10^-8
There are two ways to do this.
1. Simplify the equation so there is no quadratic. You do that by making the assumption that y + 0.001 = 0.001; that is, that y is such a small number that a small number + 0.001 is still 0.001. If we do that then we have
y = 1.8 x 10^-8/0.001 = 1.8 x 10^-5 M. We need to test to see if our assumption is ok. 0.001 + 1.8 x 10^-5 = 0.00102 and there is just a small difference so we let it go and work it the easy way.
2. we can solve the quadratic by equating
y^2 + 0.001 -1.8 x 10^-8 = 0
I solved this by the quadratic formula and obtained 1.77 x 10^-5 so you see we don't make a bad assumption by solving it the easy way.
Yes, you have correctly set up the Ksp expression and solved for x in terms of the concentration of the sulfate ion. Next, you need to solve for x by taking the cubic root of both sides of the equation:
x^3 = 4.5 x 10^-9
Taking the cubic root of both sides:
x = (4.5 x 10^-9)^(1/3)
Now, you can calculate the value of x using a calculator or by hand. After finding the value of x, it represents the molar solubility of lead sulfate (PbSO4) in the given solution of 1.0 x 10^-3 M Na2SO4.