chem final

high meff

lowest vapor pressureand highest boiling point of a solution.

low meff

highest vapor pressure and lowest boiling point of a solution.

low meff

low freezing point

colloids

shining a light through will be scattered/visible, has large particles that are not pure substances ex milk

catalysts

affect rate without being used up, affect the kind of collisions, often change the mechanism, proviides lower Ea in rate limiting step, does not change products and their relative properties

instantaneous rate

slope of line tangent to the curve, diff times have diff instantaneous rates

only reaction rate graph that goes up

2nd order

half life

time required for the concentration of a reaction to fall one half of its initial value

0 order half life

[A]0/2k=t1/2

1st order half life

.693/k

2nd order half life

1/[a0]k

elementary raection

reactions that occur by a single step

how to identify a catalyst

an intermediate that was a reactant in the first step

elementary steps

divided up multistep reactions

rate determining step

slow step, overall reaction is slow step rate

chemical equillibrium

occurs when forward and reverse reaction rates are equal

chemical equillibrium is product/reactant favored when

product favored when more products than reactants, reactant when more reactants than products

catalysts and equillibrium

speed up forward reaction, also speed up reverse reaction, decrease the time needed to reach equillibrium, CATALYSTS DO NOT SHIFT EQUILLIBRIUM IN EITHER DIRECTION

k c=

kforward/kreverse

if stoichiometric values are halved, k =

root of kc

to reverse a reaction, at equillibrium

inverse the k- so reactants/products, or 1/kc

KP KC RELATION

kp=kc(RT)^delta n gas(change in mols of gaseous reactants)

heat is a product in exothermic reactants, as they release heat. this means, when temperature is increased, the reaction shifts

towards the products.

endothermic reactions mean heat is a reactant, which means adding more heat shifts the reaction to the

products

does k change if p or v change?

NO

if v doubles, what happens to concentrations

divided by two

inc in pressure, dec in volume does what to reaction

shifts to products

dec in pressure, increase in volume

shifts towards reactants

temperature is th eonly property that affects equillibrium’s

constant value

adding an inert gas

does nothing to the position of the equillib

bronsted lowry acid

proton donor

bronsted lowry base

proton acceptor

arrhenius acid

when dissolved increases H+ ions, when an arrhenius base is dissolved releases OH

lewis acid

electron pair acceptor, lewis base is electron pair donor

polyprotic

has more than one h+ ion removable. the first is easier to remove, the more you have to remove the harder each gets

what makes a strong acid

a weak bond makes a strong acid, so as you get less electronegative, the bond gets weaker, so it ionizes easier

oxoacid strength

go by the most amount of oxygen but if oxygen count is the same, go by most electronegative central atom. This is opposite of normal acid, as the stronger the electronegative force, the stronger the acid. inc oxygen increases ka value. (the more electronegative, the easier to remove the H+). same for carboxylic acids

amino acids

can generate negative and pos charges at the same time, making them zwitterions. can act as both acid and a base. zwitterions are crystalline solids at room temp. they are pH dependant. if you add an acid, you get a + charge. Add a base, get a - charge (it will assume the position of the other substance)

kw

1.0×10-14, kw=ka*kb, h3o M * OH M

if a diprotic Ka1 is sifnificantly bigger than Ka2, we can assume

H+=HA-. so, Ka2= concentration of the fully deprotonated species

Gault rule

if the original concentration/20 is way larger than x, you can assume x is a negligible value and dont have to use quadratic equation

a salt is an

ionic compound formed from acid base reactions. a strong acid + a strong base makes a neutralization reaction = water and a salt

weak acid and strong base

because the acid does not completely ionize, some remains in the product side. this results in a strong conjugate base left over, which makes it basic

weak base strong acid

produces acidic solution

if the salt has an anion and cation that dont interact with water, the ph is

neutral. however, if an anion reacts with water, the ph is basic, and if a cation interacts with water, the ph is acidic. if both interact with wter, the k value determines the nature of the pH.

blood ph

buffered at 7.5 plusminus .05

is blood ph too low

acidosis, reduces ability to move oxygen

if blood ph is too high,

alkalosis, musle weakness and cramps

pka

-log ka

buffer range

ph=pka+1

in equillibrium volume raised, relies on delta n mols of gas in that

the reaction will shift towards the side with more mols. a decrease in volume will shift to the side with less mols.

when ranking acids , stronger acids in the same row

are th eones thate are more electronegative. so if in the same row, go for more electronegative acid as stronger

beta emission

conversion of a neutron to a proton

positron emission

conversion of proton to neutron