Studied by 1 personNeutralization reactions
________ occur when an acid donates its proton to a base.
Indicators are ________ that change colors based on pH change.
weak acids
________ will dissolve completely in water and never reach equilibrium.
Strong acids
1x10^-14
value of Kw constant
pH + pOH =
14
[H+][OH-] =
1x10^-14
A(n) ________ is a solution with a stable pH.
buffer
________ can give up more than one hydrogen in a solution.
Polyprotic acids
________ do not dissociate but accepts protons.
Bases
When just enough acid/base is added to an acid/base to neutralize
equivalence point
half-equivalence point
when exactly half the amount of acid/base is turned into its conjugate in a titration
Increasing ________ means decreasing [H+] and making a solution less acidic.
pH
________ means more acid dissociation (stronger acid)
Greater Ka value
________ means more protonatization (stronger base)
Greater Kb value
Complete dissociation, only hydrogen and hydroxide ions remail
Strong acid and strong base reaction
Proton is donated, conjugate of base is created
Strong acid and weak base reaction
Protons accepted, created conjugate of acid and water
Weak acid and strong base
Simple proton transfer
Weak acid and weak base reaction
Ka
equilibrium constant for weak acids
Kb
equilibrium constant for weak bases
Note
Flashcard