What is the Ksp of PbCl2 if, in a saturated solution of this salt, [Cl-(aq)] = 0.032 mol/L ?
ksp=(x/2)( x)^2
=(.032)^3/2
Why did the chemist break up with their significant other? Because they had no chemistry! But let's get back to your question.
The Ksp (or the solubility product constant) of PbCl2 can be calculated using the concentrations of the ions in a saturated solution. In this case, the concentrations of chloride ions ([Cl-]) in the saturated solution is given to be 0.032 mol/L.
Now, let's assume that x mol/L of PbCl2 dissociates into Pb2+ and 2Cl- ions. Since PbCl2 dissociates in a 1:2 ratio, the concentration of Pb2+ ions would be x mol/L.
Using these values, we can set up the equation for the solubility product constant:
Ksp = [Pb2+][Cl-]^2
Substituting the values we have:
Ksp = (x)(0.032)^2
And there you have it! Solve for x and you'll find the solubility of PbCl2 in the saturated solution. But remember, this is a serious matter for the chemist, so be careful not to clown around too much!
To find the Ksp of PbCl2, we need to use the formula for Ksp:
Ksp = [Pb2+(aq)][Cl-(aq)]^2
From the information given, we know that the concentration of chloride ions ([Cl-(aq)]) in the saturated solution is 0.032 mol/L. However, we don't know the concentration of lead ions ([Pb2+(aq)]).
Therefore, we cannot determine the Ksp of PbCl2 with the given information.
To determine the value of Ksp (the solubility product constant) for PbCl2, we need to know the concentration of the dissolved products in a saturated solution.
The solubility of PbCl2 can be represented by the equation: PbCl2 ⇌ Pb2+(aq) + 2Cl-(aq)
Let's start by looking at the balanced chemical equation. According to the stoichiometry of the equation, for every 1 mole of PbCl2 that dissolves, it produces 1 mole of Pb2+ ions and 2 moles of Cl- ions.
In a saturated solution, PbCl2 is in equilibrium with its dissolved ions. At this point, the concentration of Pb2+ ions and Cl- ions remains constant.
From the given information, the concentration of Cl-(aq) in the saturated solution is 0.032 mol/L.
Since the stoichiometric ratio is 1:2 for Cl- to PbCl2, the concentration of Pb2+ ions in the saturated solution will be half of the concentration of Cl- ions.
Hence, the concentration of Pb2+ ions in the saturated solution would be 0.032 mol/L divided by 2, which is 0.016 mol/L.
Now, we can calculate the Ksp value for PbCl2 by using the equilibrium expression:
Ksp = [Pb2+][Cl-]²
Substituting the values we obtained:
Ksp = (0.016 mol/L)(0.032 mol/L)²
Ksp = 0.000016 mol/L³
Therefore, the Ksp value for PbCl2 in a solution with a [Cl-] concentration of 0.032 mol/L is 0.000016 mol/L³.