Презентация на тему Disperse systems. True solution

solutions, suspensions, and colloids.

2) Understand, compare, and contrast the

terms homogeneous mixture and heterogeneous mixture. For a homogeneous mixture, explain the difference between solute(s) and solvent.

3) Predict the effect of temperature and pressure on the solubility of gases in water and the effect of temperature on the solubility of solids in water.

4) Be able to use the Solubility Rules Table to determine if an ionic compound will significantly dissolve in water.

5) Be able to calculate the concentration of a solution using various concentration units of measurements. (%, parts per thousand, molarity, molality, normality and titer)

in the form of very small particles (in the

form of droplets, dust, gas bubbles) is uniformly distributed in a medium (volume) of the other.

Disperse System composed of:
Dispersed phase – substance that is distributed
Dispersion medium – the continuous Phase or vehicle (acts as a solvent)

– polymer solution, homogeneous system
Sol – microheterogeneous system
Molecular
Mixed

(molecular-ionic)

Ionic

phenomenon was studied for the first time by Tyndall.

The illuminated path of the beam is called Tyndall cone.

When light passes through a sol, its path becomes visible because of scattering of light by particles. It is called Tyndall effect.

cm
COLLOIDAL
SYSTEM
D = 10-7 – 10-9 cm
SUSPENSIONS
D> 10-7 cm

pure substances in water
compound
a heterogeneous mixture
a homogeneous mixture

of 2 or more substances in a single phase

SOLUTE

– the part of a solution that is being dissolved (usually the lesser amount)

SOLVENT – the part of a solution that dissolves the solute (usually the greater amount)

SOLUTE
+ = SOLUTION
SOLVENT

One part is the substance that is dissolved. What

is the name of this part of a solution?

solvent

vehicle

solution

solute

solution:
non –electrolytes, e.g. organic substances
Ionic solution:
soluble electrolytes

solution – salts, bases, acids

Mixed (molecular-ionic) solution

particles with solvent particles to form a solution
SOLUTE
Soluble –

a substance that dissolves in a solvent

Insoluble – a substance that does not dissolve in a solvent

expressed in grams, that can be dissolved in 100

g of water at a specific temperature and pressure.
UNSATURATED – a solution that contains less dissolved solute
SATURATED – a solution that contains the maximum amount of dissolved solute
SUPERSATURATED – a solution that contains more dissolved solute than a saturated solution at the same temperature (as result solute will usually precipitate out of solution)

amount of solute dispersed in the solvent

The Concentrated is

a solution in which large amount of solute is dissolved in the solvent

concentrated solution from a more concentrated solution.

and water (both H-bonded polar liquids).
Immiscible liquids form distinct

separate phases, e.g. gasoline (non-polar) and water (polar).

colorless CCl4

green NiCl2(aq)

colorless C7H16

Solute-Solvent Interactions

after mixing and settling

solvent:
Polar substances tend to dissolve in polar solvents.
Non-polar substances

tend to dissolve in non-polar solvents.

2) Temperature – solubility usually increases as T increases

3) Pressure – for gas solution solubility increases with the P

solutes in liquid solvents increases with increasing temperature.
The solubility

of gas solutes in liquid solvents decreases with increasing temperature.

gas to dissolve.
The solubility of liquids and solids does

not change appreciably with pressure.
But, the solubility of a gas in a liquid is directly proportional to its pressure.

solubility of a gas in a liquid is proportional

to the partial pressure of the gas over the solution (Henry’s law).

c = k•P

c is the concentration (mol) of the dissolved gas
P is the partial pressure of the gas over the solution
k is a constant (mol/L•atm) that depends only
on temperature

a solid substance dissolving in an aqueous solution. It

represents the level at which a solute dissolves in solution:  

in a given amount of solvent is represented by

the …

Volume of the solution

Mass of the solute

Mass of the solution

Concentration of the solute

of solute present in a given quantity of solvent

or solution.
There are many different units for this purpose, including:
Percent by weight or volume,
Molarity,
Normality,
Molality,
Titer.

Concentration Units

of the solute divided by the mass of the

solution, multiplied by 100 (%):



2) Molarity is the number of moles of solute per liter of solution (mol/l):

weight of a solute per 1 liter of solution

(mol*eq/l):



4) Molality is the number of moles of solute per 1 kilogram of solvent (mol/kg):

a solute per 1 milliliter of solution (g/ml):