THE SOLUBILITY PRODUCT CONSTANT FOR BaSO4 AT 298K IS 1.1X10-1O POWER. CALCULATE THE SOLUBILITY OF BaSO4 IN MOL\L AT 298K
Basically, when BaSO4 dissolves in water, it dissociates into the ions Ba^+2 and SO4^-2. The solubility product constant expression then becomes as follows:
Ksp=[Ba^+2][SO4^-2]
You already know that the Ksp for BaSO4 is 1.1x10^-10. This means that BaSO4, when it dissociates, has the same concentrstion for its ions.
Ksp=[Ba^+2][SO4^-2]
Ksp=[1.1×10^-10][1.1×10^-10]
Ksp=1.21×10^-20
To calculate the solubility of BaSO4 in mol/L at 298K using the solubility product constant (Ksp), we need to set up an expression using the stoichiometry of the reaction.
The balanced chemical equation for the dissociation of BaSO4 is:
BaSO4(s) ↔ Ba2+(aq) + SO42-(aq)
The solubility product expression is:
Ksp = [Ba2+][SO42-]
Since each BaSO4 molecule dissociates to form one Ba2+ ion and one SO42- ion, the equilibrium concentrations of Ba2+ and SO42- ions will be the same as the solubility of BaSO4.
Let's assume the solubility of BaSO4 is represented as "x" mol/L.
Then, at equilibrium, the concentration of Ba2+ and SO42- ions will also be "x" mol/L.
Substituting these values into the Ksp expression, we get:
Ksp = [Ba2+][SO42-] = x * x = x^2
Given that Ksp is 1.1 x 10^-10 at 298K, we can set up the equation:
1.1 x 10^-10 = x^2
Taking the square root of both sides, we find:
x = √(1.1 x 10^-10)
Calculating this on a calculator gives us:
x ≈ 3.32 x 10^-6 mol/L
Therefore, the solubility of BaSO4 in mol/L at 298K is approximately 3.32 x 10^-6 mol/L.
To calculate the solubility of BaSO4 in mol/L at 298K, we need to use the solubility product constant expression and solve for the concentration of the ions.
The solubility product constant expression for BaSO4 is given by:
Ksp = [Ba2+][SO42-]
Where [Ba2+] represents the concentration of barium ions and [SO42-] represents the concentration of sulfate ions.
Since BaSO4 is a sparingly soluble salt, we assume that x is the common ion concentration. Therefore, the solubility of BaSO4 can be represented as: 2x (for Ba2+) and x (for SO42-).
Now, substitute these concentration values into the solubility product expression and set it equal to the given Ksp value:
Ksp = [Ba2+][SO42-]
1.1x10^-10 = (2x)(x)
Rearrange the equation:
x^2 = 1.1x10^-10 / 2
Simplify the equation:
x^2 = 5.5x10^-11
Take the square root of both sides of the equation:
x = √(5.5x10^-11)
Use a calculator to find the square root:
x ≈ 7.42x10^-6 M
Therefore, the solubility of BaSO4 in mol/L at 298K is approximately 7.42x10^-6 M.