Arrhenius acids and bases Bronsted-Lowry relative
- acids: when dissolved in water, strength table
increases concentration of h+ - strong acids: hcl, hno3,
ions hclo4, h2so4, hi, hbr
- bases: whe dissolved in water, - top of acid column
increases concentration of - produce weak conjugates
oh- - conjugates unlikely to
- for aqueous solutions only attract a proton
- completely transfer their
Brønsted-Lowry acids and protons to water
bases - strong bases: koh, lioh,
- Brønsted-Lowry acid-base rxn sr(oh)2, naOH, ca(oh)2,
is an equilibrium rxn involving ba(oh)2, rb(oh)2, cs(oh)2
proton transfer - bottom of column
- acid: a substance that can - strong ability to attract
donate a proton (h+) proton from an acid in
-base: a substance that can aqueous solution
accept a proton (H+) - ionize completely in water
- every acid has conjugate base - produce very weak
pair formed by removing conjugates
proton from acid - weak acids and bases are in
- ie: hf and f- middle of table
- every base has conjugate - only partially ionize in
acid formed by adding proton aqueous solutions
to base - exist in solutions as
- ie: h2o and h3o+ mixture of acid molecules
- strong acids/bases push & their conjugates
equilibrium forward or back, - weak bases in this group
depending on what side of have slight ability to
equation it lies remove protons from
- ie: if on reactants, pushes water
rxn to products. If on - weak acids are Any acid
product side, pushes to that’s not a strong acid +
reactants conj. acids of weak bases
, - strong acids/bases have weak - weak bases are nh3 + any
conjugates structure similar to nh3
- weaker the conjugate, the (nh2, etc)
more stable, non-reactive - can use table to predict
and weak it is which side equilibrium
- strong acids/bases ionize 100% favored.
- weak acids/bases partially ionize - the favored direction is
- when writing equations from stronger to
for them, must add them weaker member of conj
w/ h2O acid-base pair
- ie: hf + h2O —> Self-ionization of
- the more easily an acid/base water
donates/accepts a proton, the - amphiprotic / amphoteric:
less easily its conjugates a substance that can act
accepts/gives up a proton like an acid or base
- ie: hcl conjugate, cl-, - ie: water
doesn’t accept proton as - autoionization: water
easily b/c hcl is strong acting like an acid and a
acid that gives up base with itself
proton easily - [h3o+], [oh-], and kw have
a relationship when in
Ph and other related scales
aqueous solution
- ph > 7 = basic
- kw = [h3o+][oh-]
- ph = 7 = neutral
- kw = 1.00 x 10^-14
- ph < 7 = acid
- ph + poh = 14.00
- ph = -log [h3o+]
- to find [h3o+] when ph is known:
10 p
# =
[+130-1]
-
- for sig figs, # sig figs in log
operation = # decimals in ph
- poh = -log [oh-]
- acids: when dissolved in water, strength table
increases concentration of h+ - strong acids: hcl, hno3,
ions hclo4, h2so4, hi, hbr
- bases: whe dissolved in water, - top of acid column
increases concentration of - produce weak conjugates
oh- - conjugates unlikely to
- for aqueous solutions only attract a proton
- completely transfer their
Brønsted-Lowry acids and protons to water
bases - strong bases: koh, lioh,
- Brønsted-Lowry acid-base rxn sr(oh)2, naOH, ca(oh)2,
is an equilibrium rxn involving ba(oh)2, rb(oh)2, cs(oh)2
proton transfer - bottom of column
- acid: a substance that can - strong ability to attract
donate a proton (h+) proton from an acid in
-base: a substance that can aqueous solution
accept a proton (H+) - ionize completely in water
- every acid has conjugate base - produce very weak
pair formed by removing conjugates
proton from acid - weak acids and bases are in
- ie: hf and f- middle of table
- every base has conjugate - only partially ionize in
acid formed by adding proton aqueous solutions
to base - exist in solutions as
- ie: h2o and h3o+ mixture of acid molecules
- strong acids/bases push & their conjugates
equilibrium forward or back, - weak bases in this group
depending on what side of have slight ability to
equation it lies remove protons from
- ie: if on reactants, pushes water
rxn to products. If on - weak acids are Any acid
product side, pushes to that’s not a strong acid +
reactants conj. acids of weak bases
, - strong acids/bases have weak - weak bases are nh3 + any
conjugates structure similar to nh3
- weaker the conjugate, the (nh2, etc)
more stable, non-reactive - can use table to predict
and weak it is which side equilibrium
- strong acids/bases ionize 100% favored.
- weak acids/bases partially ionize - the favored direction is
- when writing equations from stronger to
for them, must add them weaker member of conj
w/ h2O acid-base pair
- ie: hf + h2O —> Self-ionization of
- the more easily an acid/base water
donates/accepts a proton, the - amphiprotic / amphoteric:
less easily its conjugates a substance that can act
accepts/gives up a proton like an acid or base
- ie: hcl conjugate, cl-, - ie: water
doesn’t accept proton as - autoionization: water
easily b/c hcl is strong acting like an acid and a
acid that gives up base with itself
proton easily - [h3o+], [oh-], and kw have
a relationship when in
Ph and other related scales
aqueous solution
- ph > 7 = basic
- kw = [h3o+][oh-]
- ph = 7 = neutral
- kw = 1.00 x 10^-14
- ph < 7 = acid
- ph + poh = 14.00
- ph = -log [h3o+]
- to find [h3o+] when ph is known:
10 p
# =
[+130-1]
-
- for sig figs, # sig figs in log
operation = # decimals in ph
- poh = -log [oh-]
