What is the solubility of BaSO4
in a solution of
0.250 M Na2
SO4
? The Ksp of BaSO4
is 8.7 x 10-11.
BaSO4 has a certain solubility by itself; with Na2SO4 the solubility is decreased due to the common ion effect. The common ion is the sulfate ion. You have two equilibria.
........Na2SO4 ==> 2Na+ + [SO4]^2-
I.......0.250.......0......0
C......-0.250.....0.50...0.250
E........0........0.50...0.250
.......BaSO4==> Ba^2+ + [SO4]^2-
I......solid....0.........0
C......solid....x.........x
E......solid....x.........x
Ksp = (Ba^2+)[(SO4)]^2-
Ksp you know.
(Ba^2+) is x
[(SO4)]^2- is x from the BaSO4 and 0.250 from the Na2SO4 so total is x+0.250
Substitute and solve for x.
1.calculate the pH of a 0.050 M HCl solution.Since HCl is a strong acid, it dissociates completely.
2.What is the pH of a 0.0026 M NaOH solution.
3.Distinguish between table sugar dissolving in water and
table salt dissolving in water.
4.. What type of intermolecular forces of attraction must be
overcome to melt each of the following solids?
(a) ice, H2O(s) (b) iodine, I2(s)
5.State the principle on which the VSEPR theory is based.
6.Use electronegativity values and VSEPR theory to determine
whether carbon tetrachloride, CCl4
, and ammonia,
NH4
, are polar or nonpolar molecules.
To determine the solubility of BaSO4 in a solution of 0.250 M Na2SO4, we need to consider the concept of solubility product constant (Ksp). Ksp is the equilibrium constant for the dissolution of a sparingly soluble salt in water. It indicates the maximum amount of a salt that can dissolve in a solution at a specific temperature.
The equation for the dissolution of BaSO4 in water is:
BaSO4(s) ⇌ Ba2+(aq) + SO4 2-(aq)
The Ksp expression for this reaction is:
Ksp = [Ba2+][SO4 2-]
Since the concentration of Na2SO4 is 0.250 M, we can assume that the concentration of SO4 2- in the solution is also 0.250 M.
Let's assume the solubility of BaSO4 is 's' in moles per liter (mol/L). Therefore, the concentration of Ba2+ in the solution would be 's' and the concentration of SO4 2- would also be 's'.
Plugging these values into the Ksp expression:
8.7 x 10^-11 = (s)(s)
Now, solve for 's' by taking the square root of both sides:
s = √(8.7 x 10^-11)
Calculating this value yields the solubility of BaSO4 in the given solution.