Title: Microsoft PowerPoint - PCQA111_Week-5-Solution-and-Gas-Laws
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Jayson F. Serrano, RPh Instructor
Solute the substance that is dissolved
Solvent the dissolving medium.
Solution
The amount of solute that dissolves in a given amount of
solvent to produce a saturated solution.
Solution
Mixture
Liquid-Liquid
Liquid-Solid
Solid-Solid Types of
Gas this is a solution wherein
the solute and the solvent are
both gases.
Liquid this is a solution in
which the solute can be a solid,
liquid or a gas and the solvent
is a liquid.
Solid this is a solution
composed of a solid, liquid or a
gas solute and a solid solvent. Classification of
Saturated a solution that contains the
maximum amount of solute that a solvent can
dissolve.
Unsaturated a solution that contains less
amount of solute that the solvent can dissolve.
Supersaturated a solution that contains more
amount of solute than the solvent can dissolve.
Classification of Solutions
Classification of Solutions Miscibility (liquid solutions)
Miscible all the components of the
solution dissolve in each other in all
proportions.
Immiscible the components of the
solution are completely insoluble in one
another regardless of the proportions
involved.
Classification of Solutions Reference or Standard Solutions
Isotonic when two solutions
have the same amount of solute
concentrations
Hypotonic solution when one
solution have a lower solute
concentration than that of
another solution
Hypertonic solution when
one solution contains a higher
solute concentration than that
of another solution
Classification of Solutions
Homogeneous
Do not settle
even on long
standing
Variable
composition
Clear even when
colored
Separated by
physical means
Can pass
through a filter
medium
Classification of Solutions
The measure of how much solute can be
dissolved in a given amount of solvent at a
given temperature.
Solubility = amount of solute (max)
amount of solvent
Classification of Solutions
Factors Affecting
Solubility
Temperature
Pressure
Surface area
Nature of solvent
Stirring the mixture
Classification of Solutions
Concentration is the
amount of solute
dissolved in a given
amount of solution.
This will affect the
properties of a solution
both the physical and
chemical
Concentrated a solution
that contains large amount
of solute in relation to the
solvent in the solution.
Dilute a solution that
contains small amount of
solute in relation to the
solvent in the solution.
Classification of Solutions Weight / Volume Percent (W/V%)
Concentration = amount of solute / amount of solution
% W/V = (grams solute / millilters solution) X 100
Example :
What is the percent composition of 500 ml solution containing
12 grams sodium chloride (NaCl) crystals?
Classification of Solutions Example:
2.0 L of an aqueous solution of potassium
chloride contains 45.0 g of KCl.
What is the weight/volume percentage
concentration of this solution in g/mL?
Classification of Solutions Weight / Weight (W/W%)
(W/W%) = (grams solute / (grams solvent) X 100
Example :
A gold ring contains 10 grams gold and
5.5 grams silver. What is the weight
percent of silver?
Classification of Solutions Molarity (M)
Molarity is defined as the number of moles of solute
per liter of solution(Chang, 2007)
Molarity = moles of solute / Liter solution
M = (g solute / mwt.solute) / Liter solution
Classification of Solutions Example:
A seven (7) liter solution contains 18.6 grams
KOH. What is the molarity of the solution?
Classification of Solutions
Molality is the number of moles of solute per
kilogram solvent.
Molality = moles of solute / kilogram of solvent
m = ( wt. solute / mwt. solute ) / kg solvent
Classification of Solutions
Example :
What is the molality of a solution if 4.6 grams
H3PO 4 is dissolved in 950 grams water?
Classification of Solutions
Normality (N)
Normality is defined as the gram-equivalent weight of
solute per liter of solution.
Normality = gram-equivalent weight of solute / liter
of solution
N = gew solute / L solution
Where : gew = wt of solute / (mwt solute / oxidation
state of cation)
Classification of Solutions
What is the normality of a five (5) liters
solution containing 36 grams Ca(OH) 2 ?LEORA & GEROA
Gain of oxygen
Loss of electrons
Gain of hydrogen
Gain of electrons
Increase in
oxidation
number
Decrease in
oxidation
number
Oxidation-Reduction Reaction Properties
of
Gas
Wide spaces between particles
Move very freely
Expand to fill container
No definite volume
Readily soluble/miscible
Low density
Compressible
Expand when heated
Gas Laws
Quantities that Influence the Nature and
Behavior of Gases:
Pressure (P) force exerted by a gas per unit area
Standard Pressure: 1atm (atmosphere) = 760 mmHg
Temperature (T) average kinetic energy of gas
particles
Standard Temperature: 273 K = 0C
Gas Laws
Volume (V) space occupied by gas particles
1 mol of gas = 22.4 L
Number of Particles (n) expressed in mole
1 mol of gas = 6.02 x 10 23 particles
Molecular Mass (m)
1 mol of gas = molecular mass (g) Boyles Law:
Pressure-Volume Relationship by English
chemist Robert Boyle in 1662.
As volume becomes smaller, more
collisions occur and the air pressure
increases; pressure and volume are
directly related at constant temperature
and amount of gas
P1V1 = P 2V2 k = T and n
Where;
P1 = initial pressure
V1 = initial volume
P2 = final pressure
V2= final volume
K = constant Charles Law
Volume -Temperature Relationship by
French physicist Jacques Alexandre
Charles in 1787.
The kinetic energy of gas particles
increases as temperature increases;
the Kelvin temperature and volume of
a gas are directly related with no
change in pressure and amount of gas.
V=V
T=T
k = P and n
Where;
T1 = initial temperature
V1 = initial volume
T2 = final temperature
V2= final volume
K = constant Gay-Lussacs Law
Pressure-Temperature
Relationship by French
scientist Joseph Louis Gay-
Lussac in 1808.
If the gas is heated, its
pressure will increase, with
constant volume and number
of moles, the pressure of a
gas is directly related to its
Kelvin temperature
P=P
T=T
K= V and n Practice Problem
1.A balloon inflated in air-conditioned room at 27
C has a volume of 4.0 L. The balloon is then
heated to a temperature of 57 C. What is the
new volume of the balloon if the pressure
remains constant?
2.A Balloon contains 2.5 L He gas at 75 C. What
is the volume in milliliter if the temperature
changes to -25 C? Examples:
1.A gas exerts a pressure of 858 torr when confined in a
5.00 L container. What will the atmospheric pressure
be If the gas is confined in a 10.0 L container at
constant temperature?
2.A balloon contains 30 L of He gas at 100 kPa. What is
the volume when the balloon rises to an altitude
where pressure is only 25 kPa? Examples:
1.The gas in a used aerosol can is at a pressure of 1000
kPa at 27 C. If the can is thrown onto a fire, what
will be the internal pressure of the gas be when its
temperature reaches 927 C? Combined Gas Law
Used to solve for
changes in
pressure, volume
and temperature
of a gas. Examples:
1.The volume of a gas at 27 C and 700 mmHg is
600 ml. What is the volume of the gas at 10 C
and 660 mmHg? Avogadros Law
Volume-Mole Relationship by Italian scientist Amadeo
Avogadro in 1811
The volume of the gas is directly related to the
number of moles at constant temperature and
pressure.
V=V
n=n
K= T and P Examples:
1.A 2.0 L container contains 0.05 mol of Ar gas.
How many grams of the gas is contained in a 3.5
L container at constant temperature and
pressure? Ideal Gas Law
Boyles Law, Charles Law and Avogadros Law were
combined where the variables pressure, volume,
temperature and amount of gas equated to a single
constant R or the universal gas constant.
R= PV
nT
PV=nRT Examples:
1.What mass of N2 gas will occupy 8.2 L at 27 C and
912 mmHg? THANK YOU FOR LISTENING!