Chapter 13 - Properties of Solutions

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Gen Chem II (Lecture)

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28 Terms

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dissolution

solute + solvent —→ solution

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crystallization

solution —→ solute + solvent

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saturated solution

have the amount of solute dissolved

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unsaturated solutions

have any amount of solute less than the maximum amount dissolved in solution

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supersaturated solutions

the solvent holds more solute than is normally possible at that temperature

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solubility

the maximum amount of solute that can dissolve in a given amount of solvent at a given temperature

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miscible liquid

mix in all proportions

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immiscible liquid

do not mix in one another

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higher pressure = ______ solubility (gases)

higher

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Henry’s Law

Sg = K Pg

Sg = solubility of the gas in solvent (molarity)

Pg = partial pressure of the gas over the solution

K = solubility constant (varies)

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higher temperature = _______ solubility

lower

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dilute

a solution with a relatively small concentration of solute

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concentrated

a solution with a large concentration

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mole fraction (X)

X = (moles of component) / (total moles of all components)

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molarity

M = (mol of solute) / (L of solution)

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molality

m = (mol of solute) / (kg of solvent)

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molality is _______ of temperature

independent

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molarity is ________ on temperature

dependent

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colligative properties

depend only on the quantity of substance and not on the identity of the solute particles

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higher concentration = ________ vapor pressure

lower

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Raoult’s Law

Psolution = Xsolvent Posolvent

ΔP = Xsolvent Posolvent

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boiling point elevation formula

ΔTb = Tb(solution) - Tb(solvent) = iKbm

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freezing point depression formula

ΔTf = Tf (solution) - Tf (solvent) = iKfm

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osmotic pressure formula

π = iMRT

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crenation

red blood cells will shrivel up if stored in a hypertonic solution

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hemolysis

red blood cells will swell and burst if stored in a hypotonic solution

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colloids

suspension of particles larger than individual ions/molecules but too small to be settled out by gravity

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Tyndall Effect

colloidal suspensions can scatter rays of light