Practice question · Multiple choice
A solution chemist claims that the solubility product constant reflects the equilibrium position of dissolution, yet it cannot serve as a universal scale for solubility. What underlies this distinction?
Hints
- How does formula stoichiometry alter the algebraic relationship between solubility product and molar solubility?
- Why might a 1:2 salt yield more dissolved ions than a 1:1 salt despite having a smaller numerical constant?
Show the answer
C. Ionic exponents depend upon stoichiometry rather than total dissolved moles
Why
Equilibrium constants scale with stoichiometric powers rather than bare moles dissolved. Assuming lower constants always mean lower solubility conflates thermodynamic constants with actual dissolved concentrations across different lattice stoichiometries.
Practise Solubility Equilibria
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