A saturated solution of a certain metal(II) chloride has a chloride ion concentration of 0.032M. The Ksp for this compound can be determined to be is?
This is similar to another question I posted that gave the Ksp and I had to find the pH. I am not sure how to start this problem using the concentration.
............MCl2 ==> M^2+ + 2Cl^-
equil.......................0.032M
If Cl is 0.032 then M must be 1/2 that or 0.016M
Then Ksp = (M^2+)(Cl^-)^2
Substitute the numbers and solve for Ksp. You should get 1.6E-5
To determine the value of Ksp (the solubility product constant) for a certain compound, you need to utilize the given information about the concentration of one of its ions in a saturated solution.
In a saturated solution of a metal(II) chloride, the compound dissociates into its ions. Let's assume the formula of the chloride compound is MCl2, where M represents the metal ion.
The dissociation process can be represented as: MCl2(s) ⇌ M2+(aq) + 2Cl^-(aq)
According to the given information, the concentration of chloride ions (Cl^-) in the saturated solution is 0.032 M. We can assume that the concentration of the metal ion (M2+) also becomes 0.032 M, based on a 1:1 stoichiometry of the dissociation reaction.
Now, to find the value of Ksp, we need to set up an equation using the relationship between the concentrations of ions in the equilibrium expression. In this case, it is:
Ksp = [M2+][Cl^-]^2
Since we assume the concentration of M2+ to be 0.032 M and the concentration of Cl^- is also 0.032 M, we can substitute these values into the equation:
Ksp = (0.032)(0.032)^2
Simplifying, we find:
Ksp = 0.032 * 0.032 * 0.032 = 3.2768 × 10^-5
Therefore, the Ksp value for the metal(II) chloride compound is approximately 3.2768 × 10^-5.