Unit 7 - Acids and Bases Flashcards
Arrhenius theory
acid = ionizes in water to generate a proton; base = ionizes in water to produce hydroxide ions
Bronsted-Lowry theory
acid = proton donor; base = proton acceptor
Lewis theory
acid = electron pair acceptor; base = electron pair donor
Strong acids
dissociate to a large extent;
have very weak conjugate bases;
HCl, HBr, HI, H2SO4, HNO3, HClO4
Strong bases
dissociate to a large extent;
group 1 and 2 hydroxides, hydrides, oxides
Weak acids and bases
do not ionize completely;
the conjugate acid/base of a weak acid/base is also weak
pH and percent ionization
for a strong acid, regardless of a concentration, it is always 100% ionized;
for a weak acid, the percent ionization decreases as concentration increases;
however, acidity always increases with higher concentration
Binary acid trends
increases down a group;
charge spreads out making the conjugate base more stable;
increases from left to right;
conjugate base is more stable as EN increases
Oxyacid trends
the more oxygen atoms, the stronger the acid;
for system with the same number of oxygen atoms, higher EN leads to a stronger acid
Common gas-forming reactions
HSO3 - (H+) ; SO3 2- (2 H+) ; HCO3 - (H+) ; CO3 2- (2 H+) ; S 2- (2 H+) ; NH4 + (OH -)
Ocean acidification
CO2 in the atmosphere dissolves into ocean surface waters and lowers the pH;
this can lead to the phenomenon of coral bleaching;
carbonate ions usually used to produce calcium carbonate are instead consumed by carbon dioxide and water ions
Dangers of HF
HF is a weak acid due to the unstable anion of F- ;
however, it is still a very hazardous chemical as it precipitates with calcium and magnesium ions in the bloodstream
Acidic/alkaline foods
ingestion of acidic/alkaline food has little to no effect on blood pH
