Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section15.6: Disturbing A Chemical Equilibrium
Problem 2.1ACP: Freezing point depression is one means of determining the molar mass of a compound. The freezing...
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Using the image attached please write 3 paragraphs
1st paragraph: objective stated clearly
2nd paragraph: complete condense method describe
3rd paragraph: analysis explained
Please please please answer everything it’s very important please answer fast
![EXPERIMENT 3
FREEZING POINT DEPRESSION AND VAN'T HOFF FACTOR OF
SALINE SOLUTIONS
PURPOSE
To determine the van't Hoff factor (i) for saturated and unsaturated solutions of sodium
chloride using the freezing points
PRE-LAB
Find the solubility of sodium chloride in water (at 0°C if possible). Be sure to record your
reference.
DISCUSSION
When a solute is dissolved in a solvent, the freezing point is lowered in proportion to the total
number of moles of solute particles present. This property, the freezing point depression, is a
colligative property; that is, it depends on the ratio of solute particles to solvent particles and
not on the identity of the particles (molecules, ions, or atoms). The equation that shows this
relationship is
AT = Kfx m
(1)
where AT is the freezing point depression, Kf is the molal freezing point depression constant
for a particular solvent, and m is the molality of the solution (in mol solute/kg solvent).
When an ionic compound dissolves in water, it separates into ions. The van't Hoff factor, i,
indicates the extent to which the solute separates into ions. For example, assuming that
sodium chloride separates completely into ions which act independently of each other, the
expected (or ideal) value of i would be 2 since there are two ions per formula unit of NaCl.
However, solutions approach ideality only at very low concentrations. To account for this
deviation, we use the formula
AT=ix Kfx m
(2)
where i x m gives the total molal concentration of particles in solution. In this experiment, you
will calculate the value of i for two different sodium chloride solutions and compare them to
the ideal/expected value.
MATERIALS
Coarse salt (rock salt or kosher salt)
Ice
EQUIPMENT
600 mL beaker
Thermometer: either a glass thermometer
OR a Vernier unit and thermal sensor
Stirring rod](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdab67aeb-c4d9-43f7-88d0-dfd6e7af2d5d%2Fff941839-ee6d-44b4-ac7b-7833558c6020%2Fnzfo66a_processed.jpeg&w=3840&q=75)
Transcribed Image Text:EXPERIMENT 3
FREEZING POINT DEPRESSION AND VAN'T HOFF FACTOR OF
SALINE SOLUTIONS
PURPOSE
To determine the van't Hoff factor (i) for saturated and unsaturated solutions of sodium
chloride using the freezing points
PRE-LAB
Find the solubility of sodium chloride in water (at 0°C if possible). Be sure to record your
reference.
DISCUSSION
When a solute is dissolved in a solvent, the freezing point is lowered in proportion to the total
number of moles of solute particles present. This property, the freezing point depression, is a
colligative property; that is, it depends on the ratio of solute particles to solvent particles and
not on the identity of the particles (molecules, ions, or atoms). The equation that shows this
relationship is
AT = Kfx m
(1)
where AT is the freezing point depression, Kf is the molal freezing point depression constant
for a particular solvent, and m is the molality of the solution (in mol solute/kg solvent).
When an ionic compound dissolves in water, it separates into ions. The van't Hoff factor, i,
indicates the extent to which the solute separates into ions. For example, assuming that
sodium chloride separates completely into ions which act independently of each other, the
expected (or ideal) value of i would be 2 since there are two ions per formula unit of NaCl.
However, solutions approach ideality only at very low concentrations. To account for this
deviation, we use the formula
AT=ix Kfx m
(2)
where i x m gives the total molal concentration of particles in solution. In this experiment, you
will calculate the value of i for two different sodium chloride solutions and compare them to
the ideal/expected value.
MATERIALS
Coarse salt (rock salt or kosher salt)
Ice
EQUIPMENT
600 mL beaker
Thermometer: either a glass thermometer
OR a Vernier unit and thermal sensor
Stirring rod
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