chem final mid term

Ligand

ions/molecules with lone pairs that can act as lewis bases

Lewis base

an atom that has a lone pair that shares it

Lewis acid

accepts electron pair

ksp

ksp is a salt dissolving so the ksp will only be the molarity of salts ions multiplied

insoluble salt

less than 0.01 mol in 1 L

how is solubility determined

comparing ksps of salts with the same cation and anion ratio, if the mole ratios are different you can calculate the M of the salt at eq

when to use net k

net k=ksp*kf

AB(s) + C(aq)→. AC(aq) +B(aq)

←

low solubility salts

dissove better in solutions w relevant ligands

Q and ksp

Q=ksp its at equilbrium/saturatedd

Q<Ksp too few products

Q>ksp too many products, unsaturated some must precipitate so depending on how different molarity you can find how much precipitate

Delta s>0 when

S to liquid L to gas or s to gas

Dissolving solute in solid

Increasing volume of gas

Increasing temp

Increasing number of moles of gas (delta n gas>0)

∆G

the amount of energy that can be used to do work aka energy that is not lost because it is too dispersed

if it is negative it will be product favored

when is a system spontaneous

when gibbs is negative, entropy being positive or negative does not necessarily determine spontaneity

when a reaction is irreversible

How to manipulate gibbs free energy

 to double or triple multiple by 2 or 3

add them together to combine

negative to turn around

Whats soluble

all compounds containing alkali metals (Li+, Na+, K+, Rb+, Cs+)

Nitrates (No3-)

Acetates (CH3COO−)

Sulfates (SO42

Microstates

-possible forms of energy dispersal, gives probability of energy being in atoms

-states that disperse energy over a larger amount of atoms are more probable

-entropy increases with number of microstates

Dispersal of atoms

-increase of volume causes increase of number of micro states in gases

-so mixing gases, mixing miscable liquids, dissolving soluble solid in liquid are spontaneous and irreversible

Trends in entropy

-larger molecules have larger entropy

-structures that are more complex have a larger entropy

-entropy of solid is lower than an entropy of liquid which is lower than gas

Gibbs change as reactants go to products

initially gibbs energy decreases, reaches 0 at equilibrium then increases

For product forward equilibrium is closer to products free energy and vice versa