if BaSo4 was precipitated in solution contain 0.012 M NaCl and 0.002 M BaCl2 .calculate the sulfate concentration which is sufficient for saturate the solution with BaSo4 , if you now that the Ksp for BaSo4 equal to 1*10^-10 .

BaSO4 ==> Ba^+2 + SO4^-2

Ksp = (Ba^+2)(SO4^-2) = 1E-10
Plug in 0.002M for (Ba^+2) [from the BaCl2] and solve for sulfate ion. This assumes you are not to make a correction for the activity coefficients and work with straight molarity. Otherwise you must calculate the activity coefficients and correct for molarities and Ksp.

ha ha doing the same problem right now

To calculate the sulfate concentration required to saturate the solution with BaSO4, we need to find the maximum amount of BaSO4 that can dissolve in the solution.

The equation for the dissociation of BaSO4 is:
BaSO4 ⇌ Ba2+ + SO42-

The Ksp expression for BaSO4 is:
Ksp = [Ba2+][SO42-]

Given that the Ksp for BaSO4 is 1*10^-10, we can use this value to find the maximum amount of BaSO4 that can dissolve in the solution.

Let's assume 'x' is the concentration of SO42- that will dissolve.

At equilibrium, the concentration of Ba2+ and SO42- will be equal to 'x', so we can write:
[Ba2+] = x
[SO42-] = x

Substituting these values into the Ksp expression, we have:
Ksp = x * x
1*10^-10 = x^2

Taking the square root of both sides, we get:
x = √(1*10^-10)

x ≈ 1*10^-5

Therefore, the sulfate concentration required to saturate the solution with BaSO4 is approximately 1*10^-5 M.

To calculate the sulfate concentration necessary to saturate the solution with BaSO4, you first need to write the balanced equation for the precipitation of BaSO4:

BaCl2 + Na2SO4 -> BaSO4 + 2NaCl

From the equation, we can see that 1 mole of BaSO4 is formed for every 1 mole of BaCl2 reacted. Thus, the concentration of BaCl2 will be the limiting factor in determining the amount of BaSO4 that can be precipitated.

Given that the concentration of BaCl2 is 0.002 M, and the stoichiometry shows that 1 mole of BaCl2 reacts with 1 mole of BaSO4, we can conclude that the concentration of BaSO4 produced will also be 0.002 M.

Now, the Ksp expression for BaSO4 is given as:

Ksp = [Ba2+][SO42-]

We can assume that all of the BaCl2 dissociates into Ba2+ ions, so the concentration of Ba2+ is also 0.002 M. Now, replacing the values for Ksp and [Ba2+] into the Ksp expression, we get:

1 x 10^-10 = (0.002)[SO42-]

Rearranging the equation and solving for [SO42-], we get:

[SO42-] = (1 x 10^-10) / (0.002) = 5 x 10^-8 M

Therefore, the sulfate concentration required to saturate the solution with BaSO4 is 5 x 10^-8 M.