(a) Calculate the concentration of barium and sulfate ions in saturated barium sulfate at 25oC.
-10
(b) the solubility in g/L of barium sulfate, BaSO4.
Solution:
Example 3:
Copper(II) iodate has a Ksp of 1.4 X 10-7 @ 20oC. What is the molar solubility of the salt?
Solution:
Ksp= 1.1 x 10
(a) Calculate the concentration of barium and sulfate ions in saturated barium sulfate at 25oC.
Two questions: First what is that -10 just below the question? Second I don't know what you're usin for Ksp for BaSO4. I will use Ksp = 1.1E-10 but you should look up and use the value in your notes/text/tables.
......................BaSO4 ==> Ba^2+ + SO4^2-
I.......................solid.............0............0
C......................solid-x..........x.............x
E........................solid............x.............x
Ksp = (Ba^2+)(SO4^2-) = 1.1E-10
So (x)(x) = 1.1E-10 and x = 1.05E-5 M
(b) the solubility in g/L of barium sulfate, BaSO4.
You have 1.05E-10 moles/L. then grams = mols x molar mass so
1.05E-10 moles/L x 233.34 g/mol = ? g/L
Example 3:
Copper(II) iodate has a Ksp of 1.4 X 10-7 @ 20oC. What is the molar solubility of the salt?
Solution:
Ksp= 1.1 x 10
You do this one the same way.
..................Cu(IO3)2 ==> Cu^2+ + 2IO3^-
I..................solid................0.............0
C.................-x....................x.............2x
E..................solid................x...........2x
I'll leave the rest for you. Just plug the E line into Ksp expression and solve for x to find molarity solubility in moles/L = M