Study Set Content:
the product of the molar concentrations of H+ and OH ions at a particular temperature
: ion-product constant
Basic
nitrogen bases
amines
a compound that donates a proton to another compound (proton donor
Bronsted-Lowry acid:
is a substance that, when dissolved in water, increases the concentration of hydroxide ion, OH(aq).
base(Arrhenius)
a species that can form a covalent bond by accepting an electron pair from another species
Lewis acid
can act either as a base or an acid
Amphiprotic:
of a solution is defined as the negative logarithm of the hydrogen ion concentration
pH
strong electrolytes that, for practical purposes, are assumed to ionize completely in water; e.g. HCl, HNO3 , HClO4 , H2SO4
Strong acids
strong electrolytes that ionize completely in water; e.g. NaOH, KOH
Strong base
ionize only to a limited extent in water; e.g. HF, CH3COOH, NH4
Weak acids
is the shift in equilibrium caused by the addition of a compound having an ion in common with the dissolved substance
common ion effect
is simply an application of Le Châtelier’s principle
common ion effect
In either case this changes the values of
• [HB]/ [B- ] • [H+ ] ion concentration • pH of the buffer
Buffers contain either a weak acid and its conjugate base or a weak base and its conjugate acid. Thus, a buffer solution contains both an acid species and a base species in
equilibrium
When a strong acid is added to the buffer,
it supplies hydronium ions that react with the base A-
When a strong base is added to the buffer,
it supplies hydroxide ions. These react with the acid HA
resists changes in pH through its ability to combine with both
buffer solution
weak electrolytes; ionize to a limited extent in water
Weak base
is the amount of acid or base the buffer can react with before giving a significant pH change.
buffer capacity
