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MCAT Chemistry Question — Aqueous Solution
- by
- Aug 14, 2014
- MCAT Question of the Day
- Reviewed By: Liz Flagge
In order to determine how much Ag(NO3) can dissolve in aqueous solution, which value must be known?
a) Ka
b) pKa
c) the standard reduction potential, E°, for the silver half-reaction
d) Ksp
Explanation
The solubility product, Ksp, is an equilibrium constant for a solvation reaction. Like any other equilibrium constant, Ksp equals products over reactants raised to the power of their coefficients. Pure solids and pure liquids are left out of the Ksp. For example, Ba(OH)2 (s) dissolved in aqueous solution has Ksp=[Ba2+][OH–]2.
a) Ka, incorrect, Ka is a measure of how much an acid dissociates: Ka=[H+][A–]/[HA].
b) pKa, incorrect, pKa is related to the Ka by pKa=-log(Ka) and has nothing to do with solubility.
c) the standard reduction potential, E°, for the silver half-reaction, incorrect, The standard reduction potential is useful for calculating the voltage in a galvanic, concentration, or electrolytic cell.
d) Ksp, correct.
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