Test 2- Chem 112- St. Thomas- Summer Flashcards
True or false, The conjugate base of a strong acid has negligible acid-base properties.
true
the bigger Ka/Kb is, the ____ the acid/base is
stronger
hydronium
H3O+
hydroxide
OH-
higher pH means ____ concentration of H30
lower
lower pH means ____ concentration of H30
higher
Q
the reaction quotient at any time during reaction
K
equilibrium constant. Q, ONLY at equilibrium (the END of reaction)
Kc>1
favors products
Kc=1
they are the same
Kc<1
favors reactants
Q<K
reaction moves right (forward) to form products
Q=K
equilibrium
Q>K
reaction moves left (reverse) + forms reactants
Le Chatelier’s principle
a system in equilibrium will adjust to a stress by shifting to minimize or alleviate stress types
addition of products or reactants does what
shift in the opposite side
removal of products or reactants does what
shift in the same side
increasing temp does what
moves toward opposite side
decreasing temp does what
shifts toward the same side (energy side)
input energy (endothermic)
energy side is reactant
output energy (exothermic)
energy side is product
decrease in volume does what to pressure
increase
increase in volume does what to pressure
decrease
when does volume/pressure cause a change in equilibrium
when the reaction is with gases, it is a result of a volume change, AND there is a change in moles
increase in pressure when all conditions for eq change are met
shift toward the side with fewer gas molecules
decrease in pressure when all conditions for eq change are met
shift toward the side with more gas molecules
arrhenius definition for acids and bases
acid has H+ when dissolved, base had OH- when dissolved
Bronsted-Lowry definition
focuses more on the transfer instead of dissasociation.
Acid- donates proton
Base- accepts proton
conjugate base
deprotanated form of original acid
conjugate acid
protonated form of original base
ionization
acid-base reactions with water
autoionization
happens in every solution with water
what is not included in eq constant
liquids and solids(everything else is. g and aq)
auto ionization formula
H2O+H2O –> <– H3O + OH-
autoionization only happens in how many cases
in all cases but only in 2 out of 10^9 molecules *VERY small
amphoteric
molecules or ions that either gain or lose a proton under appropriate conditions
as [H3O] increases, pH levels ___
decrease
[H30] > [OH-]
acidic, pH lower
[H30] = [OH-]
neutral, pH 7
[H30] < [OH-]
basic, pH higher
pH <7
acidic
pH > 7
basic
pH=7
neutral
the higher the Ka is, the ____ the acid is
stronger
the higher the Kb is, the ____ the base is
stronger
% ionization
acid concentration eq/acid concentration original x100
conjugate partners of strong acids and bases are ____
neutral
conjugate partners of weak acids and weak bases are ___
weak
neutralization reaction
acid + base –> salt + (water)
always IRREVERSABLE (initial part, use stoich)
strong acid/strong base
neutral
strong acid/weak base (and why)
con acid does this- slightly acidic
weak acid/strong base and why
slightly basic (con base does this)
buffers
mixtures of weak acids and bases w conjugate partners (and I think they cause H2O to form??)
henderson-hassebach
use in buffers
strong acids
HCl
HBr
HI
HNO3
HClO4
H2SO4
strong bases
NaOH
KOH
Ba(OH)2
Sr(OH)2
Ca(OH)2
LiOH
