acids and bases Flashcards
-Arrhenius acid is
substance that dissociates in water to produce HYDROGEN ions (H+)
Arrhenius base is
a substance that dissociates in water to produce HYDROXIDE ions (OH-)
Arrhenius theory
works with many compounds in water, but misses some (particularly bases, and clearly doesn’t describe non-aqueous solutions.)
Bronsted-Lowry Acid
Proton DONOR , gives H+ ion
Bronsted-Lowry Base
Proton ACCEPTOR, takes H+ ion
Acid “dissociation” is an equilibrium where KA only describes
the reaction of an ACID with the solvent H20 as a BASE
Base “dissociation” is an equilibrium where KB only describes
the reaction of a BASE with the solven H20 as an ACID
Stronger Base or Acid, the larger the
Kb or Ka
Amphiprotic
Able to both donate and accept protons eg. water
Amphoretic
Act as both acid and base
Kw in water is
the concentrations of products multiplied together
for pH to OH to pOH conversion draw memorize Ryans square thing
When is Kw constant
in AQUEOUS solutions at 25 degrees C
a strong acid dissociates _____ in water
fully
a weak acid dissociates ______ in water
partially
An inert acid dissociates ________ in water
lol it doesn’t dissociate
u can tell when an equation is Kb if
theres OH- in the products
Kw for conjugate base pair is
Ka x Kb
Conjugate acid-base pairs u can tell by (2 things)
addition of an H is the acid
large Ka <–> Small Kb
the conjugates below are
Strong acid
Weak acid
Inert acid
inert base
weak base
strong base
(flip the list and change acid to base)
Strong acids memorize
HCIO4
H2SO4
HNO3
H + cl or br or I on right side
Strong bases memorize
Most left starting with Li to NA to K add (OH)
then on the left Ca to Sr to BA add (OH)2
pKa and pKb can be found using what
-logKa
-logKb
Ka or Kb can be calculated as
10⁻ᵖᴷᵇ
10⁻ᵖᴷᵃ
pKa + pKb =
14
pH =
-log[H3O+]
percent disociation formula
([HA]dissociated / [HA] initial) x 100
% dissociated depends on the _____ and increases with ___
Acid
Ka
% dissociation also _______ with increasing ______
increases
dilution
The more polar the H-A bond,
the stronger the acid
on periodic table acid strength and electronegativity is determined how
2nd column of right is strongest acid
larger atom leads to ______ bond which leads to ______ acid.
weaker
stronger
as electronegativity increases ____ to ____ on periodic table, acidity ___
left
right
increases
As bond strength decreases ____ the periodic table, acidity ______
down
increases
If equal concentrations of reactants and products, and there is acid on both side, which would the reaction proceed?
to the side with the weaker acid as the strong acid is the better proton donator
how to find pH or pOH as a single thing? If you have one of them?
-log (acid or base concentration)
14 - pOH or pH to get the other
how to find [OH-] or [H+]?
10^⁻[ᵖᴼᴴ] ᵒʳ ⁻[ᵖᴴ]
SALT SOLUTIONS from CONJUGATES of strong acids and strong bases are
neutral
For double weak salts, how will the amount of acid compared to base affect acidity?
Ka > Kb = acidic (< 7 pH)
Ka < Kb = basic (>7 pH)
Ka ~ Kb (pH 7)
Lewis acid is a species that
accepts electron pair
Lewis Base is a species that
DONATES!! an electron pair
in order for reaction constant > 1 (Kc > 1)…
reaction must shift to product. The two strong acid and base must be on the reactant side
the smaller the kA the _____ the ___
LARGER
pKa
less oxygen =
weaker acid
kW value is
ionization constant of water 1x10^-14
