boyles law
P1V1 = P2V2
charle’s law
V1/T1 = V2/T2
gay lussac’s law
P1/T1 = P2/T2
combined gas law
(P1V1)/T1 = (P2V2)/T2
batter cell gibbs energy
change in G = -FEcell
galvanic cell
change in G < 0, Ecell > 0, spontaneous, positive electromotive force
electrolytic cell
change in G > 0, Ecell < 0, nonspontaneous, negative electromotive force
charge through a batter cell
q = It
oxidation
loss of electron
reduction
gainig electron
Ksp equation
[catin]^x[anion]^y
electrochemical cell
any cell in which oxidation-reduction reactions take place
- anode is the site of oxidation, attracts anions
- cathode is site of reduction, attracts cations
- electrons flow from anode to cathode
- current flows from cathode to anode
simple diffusion
separate compounds with bp > 25C apart
fractional diffusion
separate compounds with bp < 25C apart
vacuum diffusion
separate compounds with high bps (>150C)
lewis acid/base
Defined as a species that accepts an electron pair or donates an electron pair, respectively
brownstead lowry acid/base
Defined as a species that donates a proton or accepts a proton, respectively
arrhenius acid/base
Defined as a species that dissociates into a H+ or OH- ion, respectively
molarity (M)
Ratio of the moles of solute to the liters of solution
molality
Ratio of the moles of solute to the kilograms of solvent
common ion effect
the presence of a common ion in a solution decreases the solubility of an incoming salt
oxidation number equation
oxidation number = group valence - noncoding electrons - assigned bonding electrons
pKa and acid strength relationship
acid strength increases at pKa decreases (the acid with the smallest pka or largest Ka is the strongest acid and yields the solution with the highest H+ and lowest pH)
how does the pH change if a strong acid is added to a buffer solution?
buffer consumes it and small pH decrease
