CHEM 2 exam 1

Mole fraction

Mf= mol A/ total moles solution

Mf of other component= 1-mf

Ptotal = Xsolute(P°solute) + Xsolvent(P°solvent)

Nonvolatile= Ptotal = Xsolvent(P°solvent)

Osmosis

Movement of solvent toward solute

When is “i” equal to 1?

If it’s not a salt, strong acid, or strong base

$\pi=$ iMRT or $\pi=$ inRT

Looking for pressure, temperature, Molarity, miles/mass etc

What LOWERS the freezing point of a solvent

Soluble compounds

more ions = bigger the decrease

vise versa increases boiling point

what raises boiling point?

higher amount of molecules/ions

Solubility rules for ionic solids dissolving in water

1. Strong bases are soluble

2. +1 or -1 are soluble

mole fraction

Moles A/total moles solution

1-mf = other mole faction

Molarity

moles solute/ liters solution

molality

moles solute/kg solvent

how would heat affect the solubility of gasoline in water

ΔTf

ΔTf= Tpure- T solution

how to know if something has high boiling point

it will have a high “i”

Specific gravity

Density

find volume= mass/density

increasing temp does what to solubility for liquids

increases solubility

Solubility of a solid is ____ by an increase of temp

increased

Solubility of a solid is ___ by an increase in pressure

not affected

solubility of a gas is ___ by an increase of temperature

decreased

Solubility of gas is _____ by an increase in pressure

increased

Osmosis

movement of solvent toward solute

why is the process of dissolving a gas exothermic(releases heat)

The gas particles lose energy once they collide with the liquid, which dissipates away as heat

Freezing point depression

When a pure solute freezes, the molecules line up all neat and attach.

The presence of a solute disrupts this process, hindering their ability to attach(freeze) therefore, lower temps are needed to allow weakened IMF to attach

ΔTb

ΔTb= Tsolution- Tpure