Chapter 10 - Acids And Bases Flashcards
Arrhenius acid and base
Acid will dissociate to form excess H+ ions
Base will dissociate to form excess OH- ions
Bronsted-Lowry acid and base
Acid a species that donates hydrogen
Base a species that excepts hydrogen
Conjugate acid and base
A base becomes a conjugate acid, and an acid becomes a conjugate base
Louis acids and bases
An acid is an electron pair acceptor
A base is an electron pair donor (would bond to H)
amphoteric species
Reacts like an acid in a basic environment, but acts as a base in an acidic environment
Amphiptotic
Hey species that can either gain or lose a proton
Auto ionization
The tendency for water to form ions of hydroxide and hydronium
The water dissociation constant Kw
Kw=10^-14
PH equation
PH= -log [H+]
pOH equation
-log[OH-]
pH+pOH =
14
Strong acids
Hydrochloric acid HCl Hydrobromic acid HBr Hydroiodic acid HI Sulfuric acid H2SO4 Nitric acid HNO3 Perchloric acid HClO4
Strong bases
Sodium hydroxide NaOH
Potassium hydroxide KOH
Hydroxides of group 1 metals
Acid dissociation constant
Ka=[H3O+][A-]/[HA]
Same for Kb with base products
Neutralization reaction
What an acid and base mix to form a salt and water
Acid equivalent
One mole of H+
Polyvalent
One mole of an acid or base contains more than one acid equivalent
Acid and base Gram equivalent
Molar mass divided by the number of equivalence produced by one mole of the acid or base
Equivalence point
The point at which all of an acid has reacted with all of the base in solution
Mid point on the steep part of a titration curve
Half equivalence point
The midpoint of the buffering region
PKA determined from a titration curve
The value at the flat or buffering region of the curve
Buffer solution
A mixture of a weak acid and it’s salt
This allows for the acid to either protonate or deportonate to account for small changes in pH
Henderson-hasselbach equation
pH= pKa + log [A-]/[HA]
Buffering capacity
The ability of a system to resist change in pH
