Topic 14: Acids, Bases, Buffers and Solubility 2
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Polyprotic acid
Acids that can lose more than 1 proton
Each successive proton is .. to remove even if proton are …
harder equivalent
At buffer point [A^-] and [HA] are … pH =
in equal amounts (pKa1 + pKa2) / 2
Lewis acid (A)
electron pair acceptor
Lewis base (B)
electron pair donor
5 types of Lewis acid
Molecules with an incomplete octet of valance electrons, completed by accepting an electron pair A metal cation, which accepts an electron pair supplied by the base A molecule or ion with a complete octet that can rearrange valence electrons and accept an electron pair. Lewis base-Lewis acid complex adduct A molecule or ion that can expand its valence shell (or be large enough) to accept another electron pair
Dissolution (dissolving) of a material occurs when
the free energy required to disrupt the lattice bonding (ΔGL ) is offset by the free energy released in the formation of aqueous species
solubility
The amount of solid (g or mol) that dissolves in a given volume of solvent (dm3)
The solubility product (Ksp)
an equilibrium constant that is related to the solubility of a salt in a solvent
K sp =
[M+]^a[X-]^b
MaXb (s) <=>
aM^+(aq) + bX^-(aq)
The common-ion effect
If a salt MX (e.g. NaCl) is added to an aqueous solution containing the solute MY (e.g. NaBr), e.g. the ion M+ is common to both salts the presence of the originally dissolved M+ ions suppresses the dissolution of MX compared with that in pure water Same effect if there is a common anion e.g. AgCl will be more soluble in water than in KCl solution