How many grams of BaSO4 can dissolve in 1.5 L of a 0.010 M solution of Na2SO4?
Ksp= 1.1 x 10^-10
I thought the answer was 1.1x10^-8 M then multiply by the molar mass to get the amount of grams but my answer isn't correct. PLEASE HELP!
You are right, you just stopped too soon./
(BaSO4) = (Ba^+2) = 1.1E-10.0.01 = ?? moles/L.
Now multiply 1.5 L (the step you omitted), THEN multiply by molar mass BaSO4 to convert to grams.
Got it, thank you!
To find out how many grams of BaSO4 can dissolve in the given solution, you need to calculate the ion product (IP) and compare it with the solubility product constant (Ksp) of BaSO4.
The balanced equation for the dissociation of BaSO4 is:
BaSO4(s) ⇌ Ba2+(aq) + SO42-(aq)
From the equation, we can see that each BaSO4 molecule dissociates to form one Ba2+ ion and one SO42- ion.
We are given the concentration of Na2SO4, which is 0.010 M. Since Na2SO4 has 2 Na+ ions and 1 SO42- ion, the concentration of SO42- in the solution is also 0.010 M.
Now let's calculate the ion product (IP) using the given concentration of SO42-:
IP = [Ba2+][SO42-]
Since both Ba2+ and SO42- ions are in a 1:1 ratio, their concentrations will be equal. Therefore, [Ba2+] = [SO42-] = 0.010 M.
IP = (0.010 M) x (0.010 M) = 0.0001 M^2
Now compare the calculated IP with the Ksp value of BaSO4. Ksp is the equilibrium constant for the dissociation of BaSO4 and represents the maximum amount of ions in a saturated solution.
If IP < Ksp, it means the solution is not saturated, and BaSO4 can dissolve further.
If IP > Ksp, it means the solution is saturated, and BaSO4 is not able to dissolve any more.
In this case, Ksp = 1.1 x 10^-10 M^2 and IP = 0.0001 M^2.
Since IP > Ksp, it means the solution is saturated and no more BaSO4 can dissolve. Thus, the amount of BaSO4 that can dissolve in 1.5 L of the solution is zero grams.
Therefore, the correct answer is that no grams of BaSO4 can dissolve in the given solution.