Suppose a solution contains a concentration of 1.0x10^-4M PbSO4 (Ksp=1.8x10^-8). Which of the following terms describes this solution?
saturated , unsaturated, supersaturated, or cannot be determined
You need to solve the Ksp expression to determine the solubility of PbSO4.
PbSO4 ==> Pb^+2 + SO4^-2
(Pb^+2)(SO4^-2) = Ksp.
Let S = (Pb^+2); then S = (SO4^-2)
Substitute into the Ksp expression and solve for S. Compare S with the value given in the problem (1.0 x 10^-4 M) to determine if it is saturated or not.
In order to determine the correct term to describe the solution, we need to compare the concentration of the solute (PbSO4) with its solubility product constant (Ksp).
The solubility product constant (Ksp) represents the equilibrium constant for the dissolution of an ionic compound in water. If the concentration of the solute is lower than the value of Ksp, then the solution is considered unsaturated. If the concentration is equal to the value of Ksp, then the solution is saturated. If the concentration exceeds the value of Ksp, then the solution is supersaturated.
In this scenario, the concentration of 1.0x10^-4M PbSO4 is higher than the value of Ksp (1.8x10^-8). Therefore, the solution is considered supersaturated.
To determine which term describes the solution, we need to compare the ion product (Qsp) with the solubility product constant (Ksp).
The solubility product constant (Ksp) for PbSO4 is given as 1.8x10^-8.
The ion product (Qsp) is calculated by multiplying the concentrations of the ions in the solution.
Since PbSO4 dissociates into Pb2+ and SO42- ions in solution, the concentration of the Pb2+ ion in the solution is equal to the concentration of PbSO4, which is given as 1.0x10^-4 M.
Now, let's calculate the ion product (Qsp):
Qsp = [Pb2+][SO42-] = (1.0x10^-4)(1.0x10^-4) = 1.0x10^-8
Comparing Qsp with Ksp:
1.0x10^-8 (Qsp) < 1.8x10^-8 (Ksp)
Since Qsp < Ksp, the solution is unsaturated.
Therefore, the correct term that describes this solution is unsaturated.