UNIT# 07
SOLUTION
AND SUSPENSION
A solution can be defined as the homogeneous mixture or single
phase mixture of the molecules, atoms or ions of two or more compound. There
are mainly nine types of solution. A solution can be prepared by the
combination of solute and solvent.
|
Q# |
Questions |
Year |
|
Q# 01 |
Differentiate
between Solution and Suspension. |
[2016][2012][2011]
[2008][2007][2006] |
|
Q# 02 |
Define
Saturated solution. |
[2012][2009]
[2008] |
|
Q# 03 |
Define
Unsaturated solution. |
[2012][2008] |
|
Q# 04 |
Define
Crystallization |
[2009] |
|
Q# 05 |
Define
Hydrolysis. |
[2005] |
|
Q# 06 |
Define
Super saturated solution. |
[2012][2008] |
|
Q# 07 |
Define
Mole fraction. |
[2008] |
|
Q# 08 |
Define
Solubility. |
[2018][2016][2015]
[2009][2008] |
|
Q# 09 |
Define
molarity . |
[2012][2009][2006]
[2005] |
|
Q# 10 |
Define
molarity and molality. Also write the formula. |
[2015] |
|
Q# 11 |
Describe
in detail the factors that affect solubility. |
[2018][2016] |
Q. Define Suspension. Give some
examples of Suspension in our daily life
SUSPENSION
The heterogeneous mixture of two or
more than two substances is called Suspension.
OR
The heterogeneous mixture consists of visible particles each of
which contains thousands molecules surrounded by liquid called suspension.
|
Common examples of suspension in daily life |
|
|
Emulsion |
Suspension of droplets of one liquid into another in which one of
them is not soluble. |
|
Foam (froth) |
Suspension of gas (air) in liquid |
|
Mud (slime) |
Suspension of fine particles of soil in small amount of liquid |
|
Smoke |
Suspension of the particles of carbon in air/ gas |
Q. Define Solution, solute,
solvent and solubility.
SOLUTION
The homogenous mixture of two or more than two substances is called
solution.
Solute + Solvent = Solution
SOLUTE
Substance which is to be dissolved in another
substance is called solute. It is usually in lesser quantity.
SOLVENT
Substance which dissolves solute in it is
called solvent. It is usually in greater quantity.
SOLUBILITY
The maximum amount of solute required to
saturate 100 gm of solvent at STP is called solubility.
Q. Describe the factors
affecting on solubility.
FACTORS
AFFECTING ON SOLUBILITY
Following are the factors which affect the solubility of a solute
in a solvent:
I.
Temperature
II.
Pressure
III.
Nature
of solute and solvent
TEMPERATURE
Solubility of a solid in the liquid increase with the rise in
temperature while solubility of gases in the liquids decrease with the increase
in temperature although solubility of liquid in liquid slightly increases with
increase in temperature.
PRESSURE
Pressure has no effect on solids and liquids.
But solubility of a gas in liquid is directly proportional to the
pressure of the gas.
NATURE
OF SOLUTE AND SOLVENT
Polar solute dissolves in polar solvents whereas non polar solute
dissolves in non-polar solvents.
Q. Define Saturated, unsaturated
and super saturated solution.
SATURATED
SOLUTION
A solution that contains maximum amount of solute in a given
solvent at room temperature is called saturated solution.
UNSATURATED
SOLUTION
It is the type of solution in which solute has less quantity than
it has the capacity to dissolve is called unsaturated solution.
SUPER
SATURATED SOLUTION
It is the solution which contains greater amount of solute that
present in a saturated solution.
Q. Define Crystallization. Describe
the crystalline properties of solids
CRYSTALLIZATION
Crystallization is the process in which dissolved solute comes out
of solution and forms crystals is called crystallization.
PROPERTIES OF CRYSTALLINE
SOLIDS
1. Sharp melting point
2. Regular and definite shape
3. Contain water of crystallization
4. Homogenous solids
Q. What is Hydrolysis?
HYDROLYSIS
The chemical breakdown of a compound due to
reaction with water is called Hydrolysis
Q. Define Molarity. Also write
its mathematical formula.
MOLARITY
The number of moles of solute which dissolves in 1 liter (1 dm3)
of a solution is called molarity.
It is denoted by (M).
FORMULA
|
M = |
Mass of solute x 1000 cm3 |
|
|
Gramm formula mass X Liter of solution ml (cm3 of
solution |
|
M= |
mass of solute |
|
|
Molar mass X volume of sol in liter or dm3 |
|
M= |
Number of moles of solute |
|
|
Volume of sol in liter or dm3 |
UNIT
M = mol
dm3
Q. Define Molality. Also write
its mathematical formula.
MOLALITY
It is the number of moles dissolved in 1000gm of solvent
It is denoted by (m)
|
m = |
Mass of solute x 1000 gm |
|
|
Gramm formula mass X gram of solvent |
|
m= |
mass of solute |
|
|
Molar mass X volume of solvent in Kg |
|
m= |
Number of moles of solute |
|
|
Mass of solvent in Kg |
UNIT
M = mol
Kg
Q. Define Mole fraction.
MOLE
FRACTION
The number of moles of the component in a solution is the number of
moles of the moles of the components divided by the total number of moles
making up a solution. It is denoted by ‘X’.
Mole fraction = number of moles of solute or solvent
Total number of moles making a solution
n1 = number of moles of solute
n2 = number of moles of solvent
Than mole fraction of solute (X1) = n1
n1
+ n2
Than mole fraction of solute (X2) = n2
n1
+ n2
Q. What is mean by percentage
concentration?
PERCENTAGE CONCENTRATION
Amount of solute dissolved in 100
parts of solution is called percentage concentration.
It can be calculate by following
methods:
1.
Mass
by mass % concentration [m/m%, w/w]
2.
Mass
by volume % concentration [M/V%, W/V]
3.
Volume
by mass % concentration [V/m%, V/w]
4.
Volume
by volume % concentration [V/V %, V/V]
MASS BY MASS PERCENTAGE CONCENTRATION
The particular mass of solute
dissolves in definite mass of solvent.
% by M/M = mass of solute X 100
Mass
of solvent
MASS BY VOLUME PERCENTAGE CONCENTRATION
The particular mass of solute
dissolves in definite volume of solvent.
% by M/M = mass of solute X 100
Volume
of solvent
VOLUME BY MASS PERCENTAGE CONCENTRATION
The particular volume of solute
dissolves in definite mass of solvent.
% by M/M = Volume of solute X 100
Mass
of solvent
VOLUME BY VOLUME PERCENTAGE CONCENTRATION
The particular volume of solute
dissolves in definite volume of solvent.
% by M/M = Volume of solute X 100
Volume
of solvent
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