Solvation

Solution

homogenous mixture

two or more substances

solute and solvent

complete miscibility

Solvent

most abundant material in the silution

usually water

Solute

less abundant material in the solution

dissolved in the solvent

Electrolyte

Compounds that dissasociate into water comletely

metal and non metal

ionic

ex: KCl

strong electrolytes have strong colligative effect because they put more particles into solution

Nonelectrolyte

does not dissasociate into water

is covalent compounds (non metal plus nonmetal)

ex: H20

dissasociate

break apart into individual ions

ex: KCl —> K + Cl

Hydration

Solvation in water

Solvation processs

when solvent particles surround abd break solute particles to form the solution

like disolves like

Dipole - Dipole Forces

forces used to break apart the solute

Solvation is endo or exo?

endothermic

solute and solvent dissasociate into particles (absorbs energy)

solvent surrounds solute (absorbs energy

When bonds form is energy released or gained

Released

exothermic

3 factors impacting solvation rate

Agitation (strirring caused more collisions)

Surface area (break solute into small pieces)

Temperature (increases KE of particles causes more collisions

Unsaturated

less than the max, more solute can be added and dissolved

saturated

equilibrium

max amount of solute added

supersaturated

more solute is added

unstable

excess precipitated solute

are gases more or less soluble in high temperatures

Less

higher KE allows more gas molecules to escape from solution

solubility of gases increases as external pressure is increased

True or false: All solutions are liquids

False

True or false: solutes dissolve in solvents

True

True or false: High surface area increases solubility

True

True or false: ionic compounds dissolve best in ninpolar solvents

false

True or false: gas solubility ncreases as temperature increases

False

True or false: polar molecules dissolve other polar molecules, and nonpolar molecules dissolve other nonpolar molecules

true

Concentration

concentration of a soltion is a measure of how much solute is dissolved in a specific amount of solvent

solutions can be concentrated (high solute)

or dilute (low solute)

concentrated

high amount of solute

diluted

low amount of solute

Molarity

used for large quanities

Dilution

used to compare the concentration of 2 substances

molality

used when measuring small concentrations close to the boiling and freezing points of the solvent

Colligative Properties

physical properties of solutions that are affected by the number of particles of the solute

NOT affected by the identity of the solute

Van’t Hoff Factor

relationship between moles of solute and moles of particles in a solution

strong electrolytes have greater colligative effect bc they put more particles into solution than weak electrolutes or molecules

Vapor pressure lowering

vapor pressure of the solution is always lower than the vapor pressure of a pure solvent

due to solute being added (nonvolatile solute)

affects the boiling point

Boiling point elevation

when a solute lowers the vapor pressure of a solvent (vapor presssure lowering) the boiling point is also effected

boiling point occurs when vapor pressure = atm pressure

more heat is needed to increase KE enough to raise the vapor pressure to equal the atm pressure

when does boiling point occur

when vapor pressure = atmospheric pressure

boiling point elevation occurs when

there is a tenperature difference between a solutions boiling point and a pure solvents boiling point

freezing point depression

solute particles interfee with the attractive forces amount solvent particles

when does freezing point depression occur

when there is a difference in temp between it s new freezing point and the freezing point of the pure solvent