Chapter 10 - Acids and Bases Flashcards
Arrhenius Acid
Forms excess of H+
- H at beginning of formula
EX: HCl, HNO, H2SO4
Arrhenius Base
Forms excess of OH-
- OH at end of formula
EX: NaOH, Ca(OH)2, Fe(OH)3
Bronsted-Lowry Acid
Donates hydrogen ions (H+)
Bronsted-Lowry Base
Accepts hydrogen ions
Lewis Acid
Electron pair acceptor
Lewis Base
Electron pair donor
Amphoteric
Can behave as an acid or a base
Amphiprotic
Amphoteric species that specifically can behave as Bronsted-Lowry acid or base
Strong Acids and Bases
Completely dissociate in solution
Weak Acids and Bases
Do not completely dissociate in solution
Equivalent
One mole of the species of interest
Normality
Concentration of acid or base equivalents in solution
Polyvalent
Can donate or accept multiple electrons
Titrations
Determine the concentration of a known reactant in a solution
Titrant
Known concentration and is added slowly to the titrand to reach the equivalence point
Titrand
Unknown concentration but a known volume
Half-equivalence point
Midpoint of the buffering region in which half of the titrant has been protonated
Equivalence Point
of acid equivalents in the original solution equals the # of base equivalents added or vice-versa
Indicators
Weak acids or bases that display different colors in their protonated and deprotonated forms
Endpoint
When indicator reaches its final color
Buffer solutions
Mixture of a weak acid and its conjugate salt or a weak base and its conjugate salt
Buffering capacity
Ability of a buffer to resist changes in pH
Henderson-Hasselbalch equation
Quantifies the relationship between pH and pKa for weak acids and between the pOH and pKb for weak bases
