LO 47 - 53 Flashcards
The [H3O+] in a strong acid solution is ________ the concentration of the strong acid because it __________
equal
completely ionizes
Strong acids solutions that are extremely diluted (10^-5 M or less) do NOT _______
completely ionize
How can you find the [H3O+] of a weak acid solution?
set up a RICE table using the neutralization reaction, initial concentration of the weak acid, and the Ka value at equilibrium
__________ is the ratio of the ionized acid concentration to the initial acid concentration times 100%
percent ionization
% ionization = __________
( [H3O+] equil. / [HA] initial ) · 100%
The equilibrium [H3O+] of a weak acid ___________ with increasing initial concentration
increases
The % ionization of a weak acid _________ with increasing initial concentration
decreases
In a mixture of a strong and weak acid, the formation of H3O+ by the strong acid will _________ of additional H3O+ by the weak acid
suppress the formation
In mixtures of strong and weak acids, what sources of H3O+ are almost always negligible?
ionization of the weak acid
autoionization of the water
In a mixture of two weak acids, how do you determine the pH?
use a RICE table and associated Ka values for each acid to determine the H3O+ ionized from each weak acid.
[H3O+] 1 + [H3O+] 2 = total [H3O+]
-log (total [H3O+]) = pH total
Just like strong acids, strong bases ___________ in solution
fully ionize
Unlike diprotic acids, bases containing 2 or more OH- ions ___________
dissociate in a single step, NOT one after another
the ____________ constant (Kb) quantifies the extent ionization of a weak base
base ionization
Kb = __________
[BH+] [OH-] / [B]
The smaller the Kb value, the ________ the base
weaker, less basic
Most weak bases are _______, which are an ammonia with one or more ______ groups
amines
hydrocarbon
Anions in solution tend to form ______ or _______ solutions
basic
neutral
Cations in solution tend to form _______ solutions
acidic
You can think of dissociated anions as the _______ to their acids
conjugate bases
ex. Cl - as the conjugate base to HCl
Anions that are the conjugate to weak acids are themselves _________
weak bases
Anions that are the conjugate to strong acids are __________
pH neutral
log(Ka) + log(Kb) =
pKa + pKb =
Ka · Kb =
log(Kw)
14
Kw
What three categories do dissociated cations typically fall into?
- counter anions to strong bases
- conjugate acids to weak bases
- small, high charged metals
In solution, strong bases completely dissociate to form OH- and the solvated __________ which do NOT ionize in water and are this considered _______
counter anion
pH neutral
Nonionic weak base + (H+) creates the ____________ cation which acts as a ________
conjugate acid
weak acid
Cations such as Al 3+ and Fe 3+ form _____________ solutions because the hydration of the ion means they act as a __________ acid
weak acid
Bronsted-Lowry
Summarize the properties of anions
Conjugate bases of acids that generally act as weak bases or are neutral
Summarize the properties of cations
Counterions of strong bases, conjugate acids of weak bases, and small highly charged metals
The stronger the acid, the ________ the conjugate base
weaker (thus weaker acids make more basic conjugate, and stronger acids a more neutral conjugate)
