Question
calculate the solubility of barium sulfate (Ksp=1.1x10^-10) in
a) water
b) a 0.10 M barium chloride solution
help is GREATLY appreciated
a) water
b) a 0.10 M barium chloride solution
help is GREATLY appreciated
Answers
DrBob222
In water: let x = solubility
.......BaSO4 => Ba^2+ + SO4^2-
.........x.......x.......x
Ksp = (Ba^2+)(SO4^2-)
Substitute from the chart above and solve for x =solubility.
For 0.1M BaCl2.
For (Ba^2+) = x from BaSO4 and 0.1 from BaCl2 for a total of 0.1+x
x = SO4^2-
Substitute into Ksp and solve for x = solubility.
The latter is an example of the common ion effect.
.......BaSO4 => Ba^2+ + SO4^2-
.........x.......x.......x
Ksp = (Ba^2+)(SO4^2-)
Substitute from the chart above and solve for x =solubility.
For 0.1M BaCl2.
For (Ba^2+) = x from BaSO4 and 0.1 from BaCl2 for a total of 0.1+x
x = SO4^2-
Substitute into Ksp and solve for x = solubility.
The latter is an example of the common ion effect.