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General Chemistry A: Chapter 18 Complex Ions and Solubility Summary
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- Orange Coast College
Concise overview of Complex Ions and Solubility. Exam review
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Solubility equilibrium Factors affectingsolubility
- solubility equilibrium: in an - solubility of a salt is lower
aqueous solution, in a solution containing
sparingly soluble salt common ion
exists in equilibrium w/ - b/c common ion
component ions suppresses ionization of
- ksp: solubility product weak acids and bases
constant that governs - can understand more by
equilibrium of these applying le chatelier
sparingly soluble salts principle
- for dissolution of ionic - when anion of slightly
cpmd in h2o soluble salt is conjugate
- molar solubility: solubility base of weak acid or base oh-,
in units of mol/l. salt becomes more soluble
- larger ksp doesnt always in acidic solution
mean higher solubility. - b/c when ph is more acidic,
- when set of cmpds have that means there is more
same stoichiometric h3o+. H3o+ can react with
amounts, then higher oh-, making solution more
ksp means higher soluble
solubility - when anion of slightly soluble
- ie: ab—>cd salt is very weak conj. Base
a2b—> c2d (cl-, br-, etc. Conj. Bases of
- when Stoichiometry strong acids), ph has no effect
differs, assumption is on solubility
invalid - b/c when h3o+ reacts with
- to see which is the very weak conj. Bases,
larger, need to find it will just form back to
molar solubilities a strong acid. Doesn’t help
solubility
- bc strong acids & bases
ionize completely, salts composed
of them dont make impact on eq.
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