The value of Ksp for barium sulfate is 1.1 x 10-10.A solution of barium sulfate with a concentration of 4.0 x 10-4 mol L-1 is Question 8Select one:a.undersaturated and precipitation of solid barium sulfate will not occur.b.supersaturated and precipitation of solid barium sulfate will not occur.c.of unknown saturation so prediction is not possible.d.supersaturated and precipitation of solid barium sulfate will occur.e.undersaturated and precipitation of solid barium sulfate will occur.
Question
The value of Ksp for barium sulfate is 1.1 x 10-10.A solution of barium sulfate with a concentration of 4.0 x 10-4 mol L-1 is Question 8Select one:a.undersaturated and precipitation of solid barium sulfate will not occur.b.supersaturated and precipitation of solid barium sulfate will not occur.c.of unknown saturation so prediction is not possible.d.supersaturated and precipitation of solid barium sulfate will occur.e.undersaturated and precipitation of solid barium sulfate will occur.
Solution
The solubility product constant, Ksp, is a measure of how much of a salt can dissolve in water. If the concentration of the ions in solution is less than the Ksp, the solution is undersaturated and more salt can dissolve. If the concentration of the ions in solution is greater than the Ksp, the solution is supersaturated and precipitation will occur.
In this case, the Ksp for barium sulfate is 1.1 x 10^-10. The concentration of barium sulfate in the solution is 4.0 x 10^-4 mol L^-1.
To determine if the solution is saturated, undersaturated, or supersaturated, we need to compare the square of the concentration of the ions in the solution to the Ksp. This is because the dissolution of barium sulfate in water can be represented by the following equation:
BaSO4(s) ⇌ Ba2+(aq) + SO4^2-(aq)
The Ksp expression for this reaction is:
Ksp = [Ba2+][SO4^2-]
Since the concentration of barium ions and sulfate ions are equal in a solution of barium sulfate, we can simplify this to:
Ksp = [Ba2+]^2
So, we compare (4.0 x 10^-4)^2 = 1.6 x 10^-7 to the Ksp of 1.1 x 10^-10.
Since 1.6 x 10^-7 is greater than 1.1 x 10^-10, the solution is supersaturated and precipitation of solid barium sulfate will occur.
So, the correct answer is:
d. supersaturated and precipitation of solid barium sulfate will occur.
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