Acids, bases and buffers
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Acid - Brønsted–Lowry
proton donor
Base - Brønsted–Lowry
proton accpetor
Buffer
a solution that resists change of pH when small amounts of acid or base are added or on dilution
End point
the point in a titration when the volume of reactant added just causes the colour of the indicator to change
Equivalence point
the point in a titration at which the reaction is just complete
Ka
Acid dissociation constant, a quantitative measure of the strength of an acid in solution. The larger the Ka value the stronger the acid, since it means the acid is largely dissociated into its ions.
Kw
Ionic product of water. At 298K, Kw = 1.0 x 10−14 mol2 dm−6
pH curve
A graph that plots pH against volume of acid/base that is added to a solution will produce a pH curve. The curve usually has a vertical part which can be identified as the equivalence point
Protonated
describes an atom, molecule or ion to which a proton (an H+ion) has been added
Strong acid
an acid that is fully dissociated into ions in solution
Strong base
A base which ionises almost completely in water. e.g. NaOH
Titration
An experimental technique used to determine the concentration of an unknown solution by using a different solution with known concentration
Weak acid
an acid that is only partially dissociated into ions in solution