solutions

1. SOLUTIONS

2. RECAPITULATION
•WHAT IS MATTER?
•WHAT ARETHE FIVE PHASES OF MATTER?
•HOW DOWE CLASSIFYMATTER?

4. SOLUTIONS
•is made up of more than one component,
but each component is evenly distributed.
•Solutions of this kind are known as
homogenous solutions.
•homogenous mixture of two or more
substances evenly distributed in each
other

5. CLASSIFICATIONS OF SOLUTIONS
ACCORDING TO PHASES
•gaseous solution
•solid solutions
•liquid solutions

6. DILUTE
• solute is present in small
amounts
CONCENTRATED
• the solute is present in
considerably significant
amounts

7. SOLUBILITY
•is the measure of how much
solute will dissolve in a solvent
at a specific temperature
•The famous saying “like
dissolves like” is important in
predicting the solubility of a

8. MISCIBILITY VS. SOLUBILITY
Miscibility
•term used when
two liquids are
completely
soluble with one
another in all
Solubility
•term used when a solid
or gas is completely
soluble in liquid in all
proportions

9. Factors Affecting Solubility of a
SoluteA. Temperature
•In the previous experiment, you were able
to dissolve excess solute upon heating.
Thus, temperature affects the solubility of
substances. The solubility of a solid in liquid
usually increases with increasing
temperature since most dissolution process
that involves a solid solute over a liquid
solvent is endothermic. However, in the
case of the solubility of gas in liquid,

10. B. Nature of Solvent
•The ability of a solute to be dissolved in a
given solvent is affected by the type of bond
of both the solute and solvent. In general,
polar liquids dissolve polar compounds and
the same is true with nonpolar liquids. Thus
goes the saying “like dissolves like”. This is
the guiding rule in preparing solutions. Since
water is a polar liquid, it dissolves polar
compounds such as sugar (C6H12O6) and
salt (NaCl). Sometimes, in spite of all
attempts, a substance does not appreciably

11. C. Pressure
•The effect of pressure on the solubility of a
solid or liquid solute is not as noticeable as
that of a gaseous solute. The solubility of
gases in water usually increases with
increasing pressure. This relationship is first
noticed by William Henry (1775-1836) in
1803 and its law is called after his name—
Henry’s law or Pressure-Solubility Law. This
law states that in a given temperature, the
mass of a gas that dissolves in a given
volume of liquid is directly related to its
pressure.

12. Factors Affecting the Rate of
Dissolution
A. Surface area
Surface area does not affect the amount of solute
that will dissolve, but it does affect the solute’s rate of
dissolution.Thus, in order to make a solid solute
dissolve faster, we frequently powder it, thereby
increasing the surface area.This is why powdered
coffee dissolves faster than granulated coffee even
without stirring.

13. B. Rate of Stirring
•The rate at which a solute
dissolves can be increased
by stirring the mixture. This
process brings fresh solvent
into contact with the solute
and so permits a faster rate
of dissolution.

14. C. Temperature
•Generally, solubility increases with
increasing temperature for most
cases of solid in liquid. The
increase in temperature causes an
increase in kinetic energy of the
solute, solvent and the solution thus
facilitating rapid interaction with one
another.

15. •A. Identify the condition that will make the
solute in each mixture dissolve faster.Write
stirring, crushing, or using heat energy in
your notebook.
1. maggi cubes and water
2. powdered milk and water
3. salt and water
4. instant coffee and water
5. sugar and pure buko juice

16. given questions in your notebook.
•1. Mother told you to prepare a glass of
milk for your small brother. After putting
amounts of sugar into the glass, you
noticed that the sugar particles are still
there. What should you do to make the
sugar dissolve faster?
•2. In your EPP subject, your group was
assigned to cook fish “sinigang”. Your
classmate bought rock salt instead of fine
salt. What should you do to the rock salt
so that it will dissolve faster in your

17. Saturated, Unsaturated and
Supersaturated Solutions•Unsaturated solution contains less solute than
it has the capacity to dissolve.
•Saturated solution is one that contains as
much of the solute as it can hold at a given
temperature.
•supersaturated solution contains more solute
than is present in a saturated solution. This is
a rather unstable condition. In this case, the
excess solid will eventually separate from the
solution as a precipitate in a process known

20. Concentration of a solution
•The amount of solute present in a given
quantity of solvent or solution.
•Four most common units of concentration:
percent composition, mole fraction,
molarity, and molality.

21. LET’S PRACTICE
•What is the mass percent of a solution of 7.6
grams sucrose in 83.4 grams of water?
•How many grams of sucrose must be added to
375 grams of water to prepare a 2.75 % by mass
solution of sucrose?
• If concentration by mass of 600 g NaCl solution is
40 %, find amount of solute by mass in this
solution.

22. Solve for the unknown. Show all work and
report answers with units.
1.What is the percent by mass of 5.0 g of iron (II)
sulfate dissolved in 75.0 g of water?
2.A solution is made by adding 25 mL of benzene to 80
mL of toluene. What is the percent by volume of
benzene?
3.A solution is formed by adding 35 g of ammonium
nitrate to 250 g of water.What is the percent by mass
of ammonium nitrate?

23. 3.What is the mass percent of each
component in the mixture formed by adding
12 g of calcium sulfate, 18 g of sodium
nitrate, and 25 g of potassium chloride to
500 g of water?
4.An experiment requires a solution that is
80% methyl alcohol by volume. What
volume of methyl alcohol should be added
to 200 mL of water to make this solution?