Acid/base Equalibrium Flashcards
Acid
The proton (H+) donor
Base
The proton (H+) acceptor
pH
A measure of acidity; pH = -log[H+]
Hydronium ion
Formed when water bonds to a proton donated from an acid. H3O+
Amphoteric
Able to act as both an acid and a base
Polyprotic
An acid that can donate multiple protons.
Ionization constant
The equilibrium constant for the ionization of a weak electrolyte
Buffer solution
A solution that resists changes in pH; contains a weak acid and it’s conjugate base.
Henderson-Hasselbalch equation
Used to calculate the pH of a buffer solution.
pH=pKa + log [conj base]/[acid] ; pOH= pKb + log [conj. Acid]/[base]
Dissociation
The separation of ions that occurs when an ionic compound dissolves .
ex. CaCl2 (s) -> Ca^2+(aq) + 2Cl^- (aq)
Neutralization reaction
A reaction between an acid and a base
Buffering capacity
The amount of acid or base the buffer can neutralize before the pH behind to change appreciably
Hydrolysis
The reaction of a substance with water
Common ion effect
Suppression of ionization of a weak electrolyte by the presence of a common ion from a strong electrolyte
End point
The point in a titration where the indicator changes color
