Acids and bases Flashcards
what did the Arrhenius theory say about acids
an acid contains H+ and forms H30+ which increases the concentration of H+
what does the Arrhenius theory say about bases?
base forms OH in water and increases the concentration of OH
what is the benefit of the Arrhenius theory?
easy to sort substances into acids and bases
what is a problem with the Arrhenius theory
many bases do not contain hydroxides and only addresses what happens in aqueous solutions
what did the Brontsted lowry theory
transfer of H+ ions from one substance to another// identify conjugate pairs
what is a conjugate base?
what is left of the acid after it donates H+// substance accepts the proton if it was in the reverse reaction
what a conjugate acid?
what is left of the base after it accepts the H+// substance that donates the H+ in reverse reaction
bronsted lowry acid:
donates a proton ( H+)
what does polyprotic mean and how many H+ do they lose
acids with more than 1 H+ and it loses one H+ at a time
what happens to H+ in weak organic acids
the H that is lost is attatched to the Oxygen within carboxyl group bc of polarity
bronsted lowry base:
accepts the proton
what arrow do you use to show a weak acid
two-way arrow
what is amphiprotic and what is an example
can act as an acid or base// water
in an image what would a strong acid/ base look like
completely dissociated
in an image what would a weak acid/ base look like
not fully dissociated
what % do weak acids and bases dissociate
below 100%
what % do strong acids and bases dissociate
100%
which type is a strong conductor and which type is weak
strong acids and bases// weak acids and bases
what pH is weak acids and bases closest to?
7
what pH # is strong acids and bases closest to?
less than 7
where would strong acids and bases lie near equilibrium
product side
where would weak acids and bases lie near equilibrium
reactant side
monoprotic acids in weak acids and bases
acid > H+
monoprotic acids in strong acids and bases
acic = H+
what are some strong acids
HI, HBr, HCL, HNO3, H2SO4, HCLO3, HCLO4,
what are the strong bases
group 1 and 2 hydroxides except Be and Mg
what is autoionization and what is an example
self dissociate and an example would be water
how does water autoionize
water will produce a very small amount of ions but not enough to make electricity
for any solution in water what is Kw
Kw = [h+][OH-] = 1 x 10^-14 @ 25 degrees
what is the Kw for water
1 x 10 ^-14 at 25 degrees
why is water’s Kw important?
acids release H+ ions into water and since water is present it autoionizes to form an equilibrium system and there will be a small amount of OH ions as well. Vice versa for bases
H+ = OH
neutral
H+ > OH
acidic
H+ < OH
basic
what will an increase of H+ ions do to the pH scale
decrease the pH
what can also replace H+
H30+
what equals 14
PH + pOH
pH –> H+
10^-pH
H+ —> pH
log[h+]
pOH to OH
10^pOH
OH to POH
-log[OH]
H+ to OH
[H+][OH”] = 1 x10^-14
when would the Kw value be different
@ different temperatures bc Kw is affected by temp
what happens when temp increases
Kw value increases// shift to products// endothermic reaction
what is the pH of neutral water @25
7
whaat does it mean to be neutral at other temperatures
H = OH
what needs to be included when writing the reaction for weak acids and bases
H20
what exactly needs to be calculated with weak acids and bases
the exact % of dissociation
how to calculate the % ionization
amount becoming ions/ original concentration
how to calculate the acid%
H+/ acid concentration
how to calculate base %
OH/base concentration
