MCAT Chem 5/6/7

heat capacity eqn

q=CΔT

(q/ΔT= J/K or cal/°C)

specific heat capacity eqn

q= mcΔT

[q/ΔTm =usu. J/kg(K) or cal/g(ºC)]

[m=mass]

cwater
1 cal g-1 ºC-1
bomb calorimeter. __ is constant
volume. No work done
fusion def.
melting
Boiling pt. elevation d/t additn of nonvolatile solt. eqn.

ΔT = kbmi

[m=molality

i=# particles after substance dissociates

kb= constant for substance being boiled (e.g. H2O)]

Freezing pt. depressn eqn.
ΔT = kfmi
osmotic press. eqn
∏= iMRT
colligative properties (4)

vapor press, b.p., f.p., osmotic press.

[depend only on # of particles not what type]

Arrhenius acid vs. base def.
acid makes H+ in aqueous soln; base makes OH-
Bronsted-Lowry acid vs. base
acid donates p+; base accepts
Lewis acid vs. base
acid accepts pair of e-; base donates
pH=
-log [H+]
metal hydrides are
basic/neutral
nonmetal hydrides are…
acidic/neutral
more O….acidic
more acidic
strong acids
HI, HBr, HCl, HNO3, HClO4, HClO3, H2SO4
strong bases
NaOH, KOH, NH2, H, Ca(OH)2, Na2O, CaO
strong acid has __ ka & ___ pka
large (>1); small (<0)
At 25°C, kw =
10-14
Acid dissociation gen’rl eqn
HA+ H2O ;; A + H3O+
base dissociatn gen’rl eqn
A + H2O –> HA + OH
pH + pOH =
14
kakb=
kw
Henderson Hasselbach eqn
pH= pka + log [A-]/[HA]
buffer soln made from
weak acid & its conjugate base
Oxidation State Table

Atoms in elemental form…0

F…-1

H (nt: -1 when bonded to metal)….+1

O (nt: xcept when H2O2)….-2

Std. H+ electrode. Electric potential =?
2H+ +2e –> H2    E°= 0.00 V
Cell potential & ΔG eqn

ΔG = -nFEmax

[positive cell pot., neg. ΔG (spontaneous)]

non-std. state cell pot. & ΔG eqn
ΔG= ΔG° + RT ln(Q)
non-std. state cell pot. & ΔG° @ equilibrium

ΔG° = -RT ln(K)

[K & ΔG° vary w/ Temp.]

K & ΔG° & E° relationships

K=1; ΔG°=0

K>1; ΔG°<0; E°>0

K<1; ΔG°>0; E°<0

At which electrode does oxidatn or reductn occur?
An Ox; Red Cat
E or emf def?
cell potential
f.p. ΔT depends on…
# particles/g that dissociates
soluble ionic compounds contain
NO3, NH4+, alkali metals (Li+, Na+, K+…), halogens (Cl, Br, I) except Ag+, Hg22+, Pb2+
1 atm= ?mmHg= ?torr
760
equivalence point d/r titration is where…
line is vertical
half equivalence point is where…
1/2 of acid has been neutralized by base
pka given. Find pkb. Eqn=?
pka + pkb = 14 (pkb is conj. base)
calculate oxidatn state of sulfur in H2SO4
(+1)(2) + (-2)(4) = 0; S= -6
log (2.5 X10-2) vs. log (1X10-2). Which is smaller # (disregard sign)?
log (2.5X10-2)
strong acid – str. base titration equivalence pt. pH=? Xcept__
7; except for diprotic acid whose conj. base is a str. acid
Reduction potential Eº. Larger # means wants to be ___ & is better ___ agent.
reduced; oxidizing agent
At equilibrium, what is 0? ΔG, ΔGº, K…
ΔG=0
x

Hi!
I'm Larry

Hi there, would you like to get such a paper? How about receiving a customized one?

Check it out