Studied by 1046 peopleNeutralization reactions
________ occur when an acid donates its proton to a base.
weak acids
Indicators are ________ that change colors based on pH change.
Strong acids
________ will dissolve completely in water and never reach equilibrium.
1x10^-14
value of Kw constant
14
pH + pOH =
1x10^-14
[H+][OH-] =
buffer
A(n) ________ is a solution with a stable pH.
Polyprotic acids
________ can give up more than one hydrogen in a solution.
Bases
________ do not dissociate but accepts protons.
equivalence point
When just enough acid/base is added to an acid/base to neutralize
half-equivalence point
when exactly half the amount of acid/base is turned into its conjugate in a titration
pH
Increasing ________ means decreasing [H+] and making a solution less acidic.
Greater Ka value
________ means more acid dissociation (stronger acid)
Greater Kb value
________ means more protonatization (stronger base)
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