Chemistry 8.1

Acids and Bases Equilibria

arrhenius model: acids

releases a proton or hydrogen ion.

arrhenius model: base

donates a hydroxide ion

bronsted-lowry model: acid

acids are proton donors

bronsted-lowry model: bases

proton acceptors

conjugate acid-base pair

results after an acid loses a proton, differ by a single proton

strong acid/base

fully dissociates

weak acid/base

minimally dissociates

strong acids (6)

HClO, HI, HBr,HCl,HNO3,H2SO4 (perchloric, hydrochloric,hydrobromic,hydroiodic,nitric,sulphuric)

strong bases

group 1 and group 2 metal hydroxides

relationship between acid strenght to its conj. base

stronger acid means weaker conj base and same for strong base with conj acid

autoionization

one in every billion H2O tranfer a proton and form hydronium and hydroxide

Kw expression

[H+][OH] = 1.0 X 10^-14 for all aqueous solutions at SATP

pH calculation

-log[H+]

pOH calculation

-long[OH-]

amphoteric or amphiprotic

can be classified as both an acid and a base in different chemical reactions; water