A generic salt, AB, has a molar mass of 159 g/mol and a solubility of 3.20 g/L at 25 °C. What is the Ksp of this salt at 25 °C?
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To determine the Ksp (solubility product constant) of a salt, we need to calculate the concentration of the ions in the saturated solution.
In this case, we have a generic salt, AB, which might be of the form A⁺B⁻.
First, let's find the concentration of the ions in the saturated solution. We know that the solubility of AB is 3.20 g/L at 25 °C.
1. Convert the solubility from grams to moles:
- 3.20 g/L ÷ 159 g/mol = 0.0201 mol/L (concentration of AB)
Since the stoichiometry of AB is not specified, we will assume it dissociates into A⁺ and B⁻ ions in a 1:1 ratio.
2. Concentration of A⁺ and B⁻ ions:
- Concentration of A⁺ = 0.0201 mol/L
- Concentration of B⁻ = 0.0201 mol/L
Now that we know the concentrations of the ions, we can calculate the Ksp.
3. Write the expression for the solubility product constant:
- Ksp = [A⁺][B⁻]
4. Substitute the concentrations of the ions into the expression:
- Ksp = (0.0201 mol/L)(0.0201 mol/L)
- Ksp = 4.04 x 10⁻⁴ mol²/L²
Therefore, the Ksp of the salt AB at 25 °C is 4.04 x 10⁻⁴ mol²/L².