Calculate the solubility of cadmium sulfide, CdS, in mol/L, given the Ksp value as 8.0 x 10^-27.
write the balanced equation
CdS>><<Cd + S
ksp= [x]^2
solve for x
x= sqrt(8E-27)
To calculate the solubility of CdS in mol/L, we need to use the Ksp expression and solve for the concentration of Cd^2+ and S^2- ions in solution.
The balanced equation for the dissolution of CdS is:
CdS(s) ⇌ Cd2+(aq) + S2-(aq)
The Ksp expression for CdS is written as:
Ksp = [Cd2+][S2-]
Since CdS has a 1:1 stoichiometric ratio, the concentration of Cd2+ ions is equal to the concentration of S2- ions.
Let's assume the solubility of CdS is 'x' mol/L. This means the concentration of Cd2+ and S2- ions will also be 'x' mol/L.
Substituting these values into the Ksp expression:
Ksp = [Cd2+][S2-] = (x)(x) = x^2
Given that the Ksp value is 8.0 x 10^-27, we can set up the equation:
8.0 x 10^-27 = x^2
To solve this equation, we can take the square root of both sides:
√(8.0 x 10^-27) = √(x^2)
x = 2.8 x 10^-14 mol/L
Therefore, the solubility of CdS in mol/L is 2.8 x 10^-14.
To calculate the solubility of cadmium sulfide (CdS), we need to determine the concentration of Cd2+ and S2- ions in solution. The Ksp value represents the equilibrium constant for the dissociation of CdS into Cd2+ and S2- ions. The solubility product expression for CdS is:
Ksp = [Cd2+][S2-]
Since the molar ratio of CdS is 1:1, we assume that the concentration of Cd2+ and S2- ions will be equal, denoted as "x".
Substituting the values into the solubility product expression, we get:
Ksp = x * x
Simplifying, we have:
8.0 x 10^-27 = x^2
Taking the square root of both sides, we find:
sqrt(8.0 x 10^-27) = x
x = 2.83 x 10^-14 mol/L
Therefore, the solubility of cadmium sulfide in mol/L is approximately 2.83 x 10^-14 mol/L.