The concept of solubility product (Ksp) is a beautiful intersection of stoichiometry and chemical equilibrium. It tells us exactly how much of a sparingly soluble salt can dissolve in a given amount of solvent before the solution becomes saturated. Let's dive into the mechanics of this problem.
Analyzing the Setup
Imagine a beaker filled with pure water. When we drop solid AB2 into it, it doesn't just sit there; a tiny fraction of it begins to dissolve. The solid lattice breaks apart, releasing ions into the aqueous medium.
The balanced chemical equation for this dissociation is our roadmap:
AB2(s)⇌A2+(aq)+2B−(aq)
Notice the stoichiometry here. For every one mole of AB2 that dissolves, it produces one mole of A2+ ions and two moles of B− ions. If we define the molar solubility of the salt as S mol L−1, then at equilibrium, the concentration of A2+ will be S, and the concentration of B− will be 2S.
The Master Equation
The solubility product constant, Ksp, is defined as the product of the equilibrium concentrations of the dissolved ions, each raised to the power of its stoichiometric coefficient.
For our salt, the expression is:
Ksp=[A2+][B−]2
Now, we substitute our equilibrium concentrations into this master equation:
Ksp=(S)(2S)2
This is where many students make a silly mistake. You must square the entire
(2S) term, which gives
4S2. Multiplying this by
S yields:
Ksp=4S3
Final Calculation
The problem provides us with the value of
Ksp, which is
3.20×10−11. We can now set up our equation to solve for
S:
4S3=3.20×10−11
Dividing both sides by 4 gives:
S3=0.8×10−11
To make taking the cube root easier, let's shift the decimal point. Multiplying the coefficient by 10 and dividing the exponent by 10 gives us a much friendlier number:
S3=8×10−12
Now, we take the cube root of both sides. The cube root of 8 is 2, and the cube root of
10−12 is
10−4:
S=2×10−4 mol L−1
The question asks for the value that multiplies 10−4, so our final answer is 2. Always remember to check the requested format of the answer!