report in chemistry

1. By: Jazmin April Pescasio

2. - A homogenous mixture of two or more
than two substances
* Homogeneous means that the components of
the mixture form a single phase.

3. - a solute disolved in a solvent
(for example a sugar/water solution)
two components of solution:
1) solute is the dissolved substance(the sugar)
2) solvent is the dissolving medium in which
the solute is dissolved(the water)

5.  gaseous solution
 liquid solution
 solid solution

6.  Ifthe solvent is a gas, only gases are dissolved
under any given set of conditions.
Example:
air (oxygen and other gases dissolved in nitrogen).

7.  Ifthe solvent is a liquid, then
gases, liquids, and solids can be dissolved.
Examples:
Gas in liquid - Oxygen in water.
Liquid in liquid - vinegar in water
Solid in liquid – sugar in water

8.  Electrolyte solution
- solutes break up into ions in water
 Nonelectrolyte solution
- solutes does not break up into ions when it is
dissolved in water

9.  Ifthe solvent is a solid, then
gases, liquids, and solids can be dissolved.
Examples:
Gas in solid - gases absorbed on Carbon Tablets
Liquid in solid - mercury in gold, forming
an amalgam
Solid in solid - All metal alloys, like Brass

10.  Unsaturated
 Saturated
 Supersaturated
 Dilute

11. This means that if you were to add more solute
to the liquid, it would keep dissolving.
Example:
if you added another teaspoon of salt, it would
dissolve, too

12. This means that the liquid has dissolved all of
the solute that is possible.
Example:
If you add one teaspoon of sugar to iced
tea, you've got an unsaturated solution. If you
keep adding sugar to iced tea, you eventually
get to the point where the rest of the sugar just
sinks to the bottom.

13. refers to a solution that contains more of the
dissolved material than could be dissolved by
the solvent under normal circumstances.
Example:
What usually happens in this situation is that the
solute starts forming crystals at the bottom of
the container.

14. a solution in which there is a small amount
of solute compared to the total amount of
possible solute that can be dissolved in the
solvent.

15.  Increased surface area
- solid solute in powder form will dissolved faster
than when it is compact
 Increased agitation
- stirring which “forcibly” breaks up the solute
particles, allows them to combine faster with the
solven particles
 Higher temperature
- rate of dissolving becomes faster at higher
temperature

16. Amount of a substance (solute) that dissolves in
a unit volume of a liquid substance (solvent) to form a
saturated solution under specified conditions of
temperature and pressure.

17. There are three main factors that control solubility of
a solute.
1) Chemical nature
2) Temperature
3) Pressure

18. Solubility of a solute in a solvent purely depends on
the nature of both solute and solvent.
A polar solute dissolved in polar solvent.
Solubility of a non-polar solute in a solvent is
large.
A polar solute has low solubility or insoluble in a
non-polar solvent.

19. Generally in many cases solubility increases with the rise in
temperature and decreases with the fall of temperature but it
is not necessary in all cases. However we must follow two
behaviors:
In endothermic process solubility increases with the increase
in temperature and vice versa.
EX: solubility of potassium nitrate increases with the increase
in temperature.
In exothermic process solubility decrease with the increase in
temperature.
EX: solubility of calcium oxide decreases with the increase in
temperature. Gases are more soluble in cold solvent than in
hot solvent.

20. The effect of pressure is observed only in the case
of gases.
An increase in pressure increases of solubility of a
gas in a liquid.
EX: carbon dioxide is filled in cold drink bottles
(such as coca cola, Pepsi 7up etc.)under pressure.