Acids and bases Flashcards
Bronsted -Lowry ACIDS AND BASES
ACIDS = Donate protons BASES = Accept protons
Lews ACIDS AND BASES
ACIDS = accept electrons BASES = Donate electrons
Strong and weak acids and bases
Strong acids and bases dissociate completely in an aqueous solution, whereas weak acids and bases only partially dissociate
Buffer Solution
One that resists changes in pH when small amounts of acid or alkali are added
Conjugate ACID - BASE pair
Conjugate acid-base pair these differ by one proton (H+); when an acid donates a proton it forms the conjugate (CH3COO- is the conjugate base of CH3COOH); when a base gains a proton it forms the conjugate acid (H30+ is the conjugate acid of H20)
Equivalence point
The point at which numbers of moles of acids and alkali have been added in a titration
Ionic product Constant
a modified equilibrium constant for the dissociation of water
Kw = {H+(aq)}{OH-(aq)}
Kw has a value of 1.0 x 10-14 at 25 degrees
Monoprotic acid
HCL is an example as it dissociates to form one proton per molecule
PH
The measure of the concentration of H+ ions in an aqueous solution; decribed as the negative logarithm to base.
10 of the hydrogen ion concentration in aquoues solution
Ph = -log10 [H+(aq)]