Exam 2 - ch.15-17 Flashcards by Ella Fischer

chemical equilibrium

occurs when the forward and reverse reaction rates are equal

How well did you know this?

Not at all

Perfectly

once equilibrium is achieved…

the concentration of products and reactants remain constant

How well did you know this?

Not at all

Perfectly

do K constants have units?

How well did you know this?

Not at all

Perfectly

K»1

rxn favors products/forward

How well did you know this?

Not at all

Perfectly

K«1

rxn favors reactants/reverse

How well did you know this?

Not at all

Perfectly

homogeneous equilibria

all reactants and products are in the same phase

How well did you know this?

Not at all

Perfectly

heterogeneous equilibria

reactants and products are in different phases

How well did you know this?

Not at all

Perfectly

are pure solids and liquids included in equilibrium expression?

How well did you know this?

Not at all

Perfectly

reaction quotient, Q

identical to calculating K, but for current conditions

How well did you know this?

Not at all

Perfectly

Q<K

rxn moving toward products

How well did you know this?

Not at all

Perfectly

Q>K

rxn moving toward reactants

How well did you know this?

Not at all

Perfectly

Q=K

reaction is at equilibrium

How well did you know this?

Not at all

Perfectly

inc in concentration of reactants

shift to right

How well did you know this?

Not at all

Perfectly

dec in concentrations of products

shift to left

How well did you know this?

Not at all

Perfectly

inc in concentrations of products

shift to left

How well did you know this?

Not at all

Perfectly

dec in concentration of products

shift to right

How well did you know this?

Not at all

Perfectly

dec in volume=inc in pressure

shift to fewer moles

How well did you know this?

Not at all

Perfectly

inc in volume=dec in pressure

shift to more moles

How well did you know this?

Not at all

Perfectly

endo temp inc

shift right

How well did you know this?

Not at all

Perfectly

endo temp dec

shift left

How well did you know this?

Not at all

Perfectly

exo temp inc

shift left

How well did you know this?

Not at all

Perfectly

exo temp dec

shift right

How well did you know this?

Not at all

Perfectly

effect of catalyst on equilibrium shift

no shift

How well did you know this?

Not at all

Perfectly

arrhenius acid

will increase [H+] when dissolved in water

How well did you know this?

Not at all

Perfectly

arrhenius base

will increase [OH-] when dissolved in water

bronsted-lowry acid

a proton donor

bronsted-lowry base

a proton acceptor

lewis acid

electron pair acceptor

lewis base

electron pair donor

amphiprotic substance

can act as an acid or base ex: water

conjugate acid-base pair

compound pair which differ by a H+

the stronger the acid...

the weaker the conjugate base

the weaker the acid...

the stronger the conjugate base

Kw=

1.0x10^-14

neutral solution

[H3O+]=[OH-]

acidic solution

[H3O+]>[OH-]

basic solution

[H3O+]<[OH-]

-log

strong acids

HCl, HBr, HNO3, HI, H2SO4, HClO3, HClO4

strong bases

alkali metal and heavier earth metal +hydroxides

%I=

[H+]/[HA] x100

%I>5%

we can not assume that the x value is really small and negligible

polyprotic acid

has more than one acidic proton

Ka1>

Ka2

hydrolysis

breaking apart water to produce H+/OH- ions

cations can be...

acidic/neutral

anions can be...

acidic/basic/neutral

anions of strong acids are...

neutral

anions of weak acids form...

basic solutions

Ka>Kb anion is...

acidic

basic

neutral metal cations

group 1/ group 2

acidic metal cations

transition and post-transition metals

hydrated cations

more acidic than free water molecules

hydrated metal cations w/ higher charges

=stronger metal/ water complex

both an anion and cation that do not react w/ water

pH is neutral

an anion which reacts w/ water and a cation that doesn't

pH is basic

cation which reacts w/ water and anion that doesn't

pH is acidic

both anion and cation reacts w/ water

compare Ka and Kb values

bond polarity: more polar

=more acidic

bond strength: decrease bond strength

=acid strength

stability: more stable

=more acidic

w/in a group look at...

bond strength to determine acidity

w/in a period look at...

polarity to determine acidity

oxyacid

H,O, and nonmental: XOH

as electronegativity increases, acidity...

increases

oxidation # increase=

increase in acidity

carboxylic acids

organic acids containing the -COOH group

buffers

soln of weak acid and it's conjugate or weak base and it's conjugate

buffer ------ pH change

resist

henderson-hasselback equation

pH=pKa+ log([A-]/[HA])

when [HA]=[A-]...

pH=pKa

equivalence point

when the amount of acid equals the amount of base

titration of strong acid w/ strong base

pH=7 at equivalence point

titration of weak acid w/ a strong base

at the equivalence point the pH>7

titration of weak base w/ strong acid

at equivalence point the pH<7

weak acid/ weak base titration pH=pKa at

halfway to the equivalence point

Ksp=

[cation][anion] (w/ respect to coefficients and powers)

solubility

the quantity of solute which can dissolve (g/L or mol/L)

common ion effect

when one of the ions are in solution it affects the solubility of the salt by decreasing it

when a salt has an anion that is the conj. base of a weak acid it is ------- soluble in an acidic solution

when a salt has an anion that is the conj. base of a strong acid solubility -------

is unchanged

amphoteric oxides + hydroxides

ions which are soluble in strong acid or strong base

Q=Ksp

at equilibrium, saturated, no ppt

Q>Ksp

excess solute, ppt formed

no ppt

selective precipitation

ions can be separated from soln based on their solubilities in the presence of different ions

Exam 2 - ch.15-17 Flashcards

(87 cards)