The Properties Of Solutions

Front 1

solute

Back 1

The solute is the less abundant component of a solution

Front 2

solvent

Back 2

The solvent is the most abundant component of a solution

Front 3

miscible

Back 3

When substances aer soluble in each other in any proportion, and it is meaningless to distinguish between solute and solvent, the substances are considered to be miscible.

Front 4

solubility (S) of a solute

Back 4

It is the maximum mount of solute that dissolves in a fixed quantity of a particular solvent at a specified temperature, given that excess olute id present.

Front 5

like-dissolves-like rule

Back 5

Substances with similar types of intermolecular forces dissolve in each other.

Front 6

hydration shell

Back 6

When an ion dissociates in water, more water molecules cluster around it forming hydration shells.

Front 7

ion-induced dipole force

Back 7

These are one of the two types of charge induced dipole forces that result from an ion causing a nearby non-polar molecule to polarize.

Front 8

dipole-induced dipole force

Back 8

These are weaker than ion induced dipole forces but are similar in that a dipole causes a nearby nonpolar molecule to polarize and feel an attraction.

Front 9

alloy

Back 9

These are solid-solid solutions typically metallic in character.

Front 10

saturated solution

Back 10

A saturated solution contains the maximum amount of dissolved solute at a given temperature in the presence of undissolved solute.

Front 11

unsaturated solution

Back 11

A solution that contains less than the maximum concentration of dissolved solute is called unsaturated.

Front 12

supersaturated solution

Back 12

It is a relatively unstable solution that contains more than the equilibrium concentration of dissolved solute.

Front 13

Temperature and solubility

Back 13

Gas solubility in water decreases with rising temperature. This causes thermal pollution.

Front 14

Henry's Law

Back 14

Solubility of a gas is directly proportional to the partial pressure of the gas above the solution. Sgas= kH * Pgas, where kH is called Henry's law constant and depends on gas-solvent combination at a given temperature.

Front 15

molality (m)

Back 15

molality = amount(mol) of solute / mass (kg)of solvent

Front 16

mass percent

Back 16

100 * [Mass of solute / mass of solution]

Front 17

volume percent

Back 17

100 * [volume of solute /volume of solution]

Front 18

mole fraction (X)

Back 18

[moles of solute]/[moles of solute + moles of solvent]

Front 19

colligative porperty

Back 19

In the case four solution properties, the number of solute particles rather than their chemical identity make a difference in the physical properties of the solution. These are vapor pressure lowering, boiling point elevation, freezing point depression and osmotic pressure.

Front 20

electrolyte

Back 20

A substance that dissociates into ions in aqueous solutions.

Front 21

nonelectrolyte

Back 21

A substance that does not dissociate into ions in aqueous solutions.

Front 22

volatie

Back 22

Nonelectrolytes that have negligible vapor pressure even at the boiling point of the solvent are considered to be volatile.

Front 23

vapor pressure lowering (∆P)

Back 23

The vapor pressure of a solution of a nonvolatile nonelectrolyte is always lower than the vapor pressure of the pure solvent.

Front 24

Raoult's Law

Back 24

Vapor pressure of solvent above the solution equals the mole fraction of the solvent in a solution times the vapor pressure of the pure solvent.

Front 25

ideal solution

Back 25

It is a solution that follows Raoult's law at any concentration.

Front 26

boiling point elevation

Back 26

A solution boils at a higher temperature than the pure solvent.

Front 27

freezing point depression

Back 27

Because the vapor pressure of the solution is lower than that of the solvent at any temperature, the solution freezes at a lower temperature than the solvent. This is called the freezing point depression.

Front 28

semipermeable membrane

Back 28

A membrane that allows only the solvent molecules but not the solute molecules to pass through.

Front 29

osmosis

Back 29

The process by which solvent molecules from a solution of one concentration passes through a semipermeable membrane into a solution of different concentration is called osmosis.

Front 30

osmotic pressure (Π)

Back 30

It is the applied pressure required to prevent the net movement of water from solvent to solution through a semipermeable membrane.

Front 31

osmotic pressure (Π)

Back 31

Π=(nsolute/Vsolution)RT = MRT, where M is the molarity.