Subtopics include 1 Describing Solutions 2 Concentrations 2 Solubility amp 3 the Effects of Solutes on Solutions Solutions Describing Solutions Define solution solute solvent electrolyte ID: 268567
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Slide1
Solutions
Subtopics include: (1) Describing Solutions, (2) Concentrations, (2) Solubility & (3) the Effects of Solutes on Solutions.Slide2
Solutions
Describing
Solutions
Define:
solution, solute, solvent, electrolyte,
suspensions,
colloidal dispersions.
Explore types of solutions.
Separation of Solutions.
Concentrations
Express
the concentrations of solutions in terms of: percent, parts per million, mole fraction, molarity and molality.
Solve problems involving the measurements of concentration
Solubility
Define:
miscible, saturated, unsaturated, solubility,
supersaturation
.
Describe Factors that effect solubility.
Use “solubility rules” to predict the solubility of an ionic compound in water.
Effects of Solutes
on Solution
Effect of solutes on the boiling point and freezing point of solutions.
Solve problems involving freezing point depressions and boiling point elevation (colligative properties).
Solve problems involving solutions and chemical equations.
Effects of electrolytes on the behavior of the solution. Slide3
Describing Solutions
Define: solution, solute,
solvent, suspensions,
colloidal
dispersions, distillation filtration & chromatography.
Explore types of solutions
.
Identify homogenous mixtures that are not solutions.
Identify the process of separating
solutions: distillation, filtration & chromatography.Slide4
Aim:
What is a Chemical Solution
?
Essential Questions
:
What
is a chemical solution?
What are some types of chemical solutions?How do we separate chemical solutions? Explain.
Key Words:
solution, solute, solvent, suspensions, colloidal
dispersions, distillation, Filtration, Chromatography.Slide5
Name Some Solutions!
Q: What are some solutions you have encountered today?Slide6
Which One is a Solution?
Salt
Water
Oil Water
The Salt Water
The Oil Water
Both
NeitherSlide7
Deduction
Q:
Based on
the previous example,
how can we describe a solution?Slide8
Notes
Describing Solutions
Definitions
Solution
- homogenous mixture of a solute dissolved in a solvent.Slide9
Solutes, Solvents & Solutions
Solute
Solvent
SolutionSlide10
Notes
2
.
Solute
–
3
.
Solvent –4. Solution –Slide11
What Makes Solutions Homogenous?Slide12
Notes
B.
“Like Dissolves Like”
In a solution, all particles attract each other with intermolecular forces of similar strength.
Polar substances dissolve other polar substances or ionic substances.
Nonpolar substances dissolve nonpolar substances.Slide13Slide14
Gases
Given:
Particles of different substances must attract each other with intermolecular forces of similar strength in order to form an even distribution, which is a solution.
Given:
There are no intermolecular forces at work between particles in the gaseous phase
Deduction: Do gaseous particles form solutions (an even distribution)?
Strong Intermolecular Forces
Weak Intermolecular Forces
No
Intermolecular ForcesSlide15
Video
Dissolving Gasses
http://www.youtube.com/watch?v=wOo5f_kvjFs
Dissolving
NaCl
http://www.youtube.com/watch?v=
EBfGcTAJF4oSlide16
Notes
2.
In
gasses there are essentially no intermolecular forces, therefore
all mixtures of gasses are solutions
. Slide17
Can Solutions Exist Between Particles in Different States (Gas, Liquid, Solid)? Slide18
Notes
C. States of Matter & Solutions
The solute and solvent may be in different phases as long as the particles are evenly distributed amongst each other.
Ex:
Solid
NaCl
dissolved in liquid water
. Ex: Gaseous CO2 is dissolved in liquid soda. Slide19
Solutions Among Various Phases of Matter
Example
Phase of Solute
Phase of Solvent
Metallic Alloy
Solid
Solid
Table salt-waterSolidLiquid
Ethyl alcohol
-water
Liquid
Liquid
CO
2
-water
(Soda)
Gas
Liquid
Air
Gas
GasSlide20
How Do We Determine Which Substance is a Solute & Which is the Solvent?Slide21
Notes
D
. Identification of Solutes vs. Solvents
If the solute and solvent are in different phases, then solute assumes the solvent’s phase.
If the solute and solvent are in the same phase, then the solvent is the one that there is more of. Slide22
All solutions are homogenous mixtures, but not all homogenous mixtures are solutions.
Can you think of an example of a homogenous mixture that is not a solution?Slide23
Suspensions
E.
Suspensions
– suspensions are formed by the physical homogenous mixture of
large particles
. (Solutions are made by the chemical mixture of smaller particles).
Suspensions will settle in time (solutions will not).
A light beam passing through a suspension mixture will be visible (in a solution, it will not).Ex. Sand + WaterSlide24
Colloidal Dispersion
F.
Colloidal Dispersion
– formed
when
particles larger than those in solution but smaller than those in suspensions are dispersed in a medium
The terms dispersed substance
vs dispersed medium are used for colloidal dispersion instead of solute and solvent. A colloidal dispersion will not settle. Tyndall effect: a light beam passing through a colloidal dispersion will be clearly visible. Ex. Whipped cream, mayonnaise, paint, gelatin & marshmallow.Slide25
Tyndall EffectSlide26
Our Chemistry class has run out of salt and we want to make a new batch from collected sea water.
How do I separate the salt from the water?Slide27
G. Separating Solutions
Evaporation
Separates dissolved SOLUTE from SOLUTION
Ex. Separating salt from water
2. Simple distillation
Separates SOLVENT from SOLUTION
Ex. Obtaining pure water from sea water 3. Fractional distillation Separates one liquid from a mixture of different liquids using differences in boiling points.
Ex. Obtaining alcohol from wine or oxygen/nitrogen from air. Slide28
4. Filtration
Separates dissolved SOLUTE from SOLUTION
Ex. Filtration of blood in kidneys
5. Chromatography
Separates mixtures into their constituents by preferential adsorption by a solid.
Ex. Separating ink dyes using paper chromatography.Cont’dSlide29
Distillation
http://www.youtube.com/watch?v=mP4Hgui-g6U&playnext=1&list=PL73CDD6FFC04D04A4&feature=
results_main
Filtration
ChromatographySlide30
Learning Check
1
)
The
solvent
is the part of the solution that
A.
gets dissolved B. does the dissolving C. changes phase2) Two homogenous mixtures not known as solutions are _______________________ and _______________________.
3) What is a chemical
solution
?
4) What
are some
types of chemical solutions
?
5) How
do we
separate chemical solutions
? Explain
.Slide31
Notes
Describing & Separating SolutionsSlide32
Describing Solutions
Definitions
Solution
- homogenous mixture of a solute dissolved in a
solvent.
Solute
– substance dissolved.
Solvent – substance that does the dissolving.Solution – A homogenous mixture composed on tiny particles.“Like Dissolves Like”In a solution, all particles attract each other with intermolecular forces of similar strength.Polar molecules dissolve other polar molecules and ionic compounds.
Nonpolar
molecules dissolve nonpolar molecules
.
2. In gasses there are essentially no intermolecular forces, therefore
all mixtures of gasses are solutions
.
C
. States of Matter & Solutions
The solute and solvent may be in different phases as long as the particles are evenly distributed amongst each other
.
Ex:
Solid
NaCl
dissolved in liquid water
.
Ex:
Gaseous CO
2
is dissolved in liquid soda
.
D.
Identification of Solutes vs. Solvents
If the solute and solvent are in different phases, then solute assumes the solvent’s phase.
If the solute and solvent are in the same phase, then the solvent is the one that there is more of. Slide33
E.
Suspensions
– suspensions are formed by the physical homogenous mixture of
large particles
. (Solutions
are made by the chemical mixture of smaller particles).
Suspensions will settle in time (solutions will not).
A light bean passing through a suspension mixture will be visible (in a solution, it will not).Ex. Sand + WaterF. Colloidal Dispersion – formed when particles larger than those in solution but smaller than those in suspensions are dispersed in a medium
The terms dispersed substance
vs
dispersed medium are used for colloidal dispersion instead of solute and solvent.
A colloidal dispersion will not settle.
Tyndall effect: a light beam passing through will be clearly visible.
Ex. Whipped cream, mayonnaise, paint, gelatin & marshmallow.Slide34
G.
Seperating
Solutions
Evaporation
– separates dissolved SOLUTE from SOLUTION.
Ex. Separating salt from water
Simple distillation – separates solvent from solutionEx. Obtaining pure water from sea waterFractional distillation – separates one liquid from a mixture of different liquids that have different boiling points. Ex. Obtaining ALCOHOL from wine or oxygen/nitrogen from air.