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SOLUTIONS

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A mixture in which the particles are more or less evenly dispersed throughout a liquid or gas. ... Ethyl alcohol. Rubbing alcohol (2-propanol) Water ... – PowerPoint PPT presentation

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Title: SOLUTIONS


1
SOLUTIONS
  • ICP
  • What you need to know

2
Heterogeneous mixturesWhat do these have in
common?
  • Fruit salad
  • Granite
  • Mica
  • Sand
  • Clay
  • Dirt
  • Blood
  • Milk

3
A suspension is a heterogeneous mixture
  • A mixture in which the particles are more or
    less evenly dispersed throughout a liquid or gas.

4
Examples of suspensions
  • Orange juice
  • Muddy water
  • Milk
  • (a solution, colloid, and suspension)
  • Blood
  • (a solution, colloid, and suspension)
  • Smoke

5
The particles in a suspension
  • Can be filtered out of the suspension
  • Will often settle out if left undisturbed for a
    while

6
Suspension have large particles.
  • These particles are too large to dissolve, so
    they eventually settle out.

7
Colloids
  • Colloids have particle sizes that are smaller
    than in suspensions, but larger than in
    solutions.
  • They are more stable than suspensions. They tend
    not to settle out.

8
Examples of colloids
  • Blood plasma (blood cells removed)
  • Egg whites
  • Fog

9
The Polar Express
10
An oil slick. There is an iridescent interface
between the polar, dense water and the nonpolar,
thin, and less dense oil layer.
11
  • What is a SOLUTE?
  • The SOLUTE is the substance dissolved in the
    SOLVENT.
  • In salt water
  • salt is the SOLUTE
  • water is the SOLVENT

12
Some relatively polar solvents.
  • Water
  • Ethyl alcohol
  • Rubbing alcohol (2-propanol)

13
Water
  • Water is considered a universal solvent because
    many different substances dissolve in water.

14
Water is polar due to H-bonding
15
LIKE DISSOLVES LIKE.
  • Water and oil dont mix.
  • Nonpolar solvents like oil
  • tend to dissolve other nonpolars.
  • Polar solvents like water tend to dissolve polar
    solutes and ionic compounds (salts).

16
  • Water will pull apart many ionic compounds
    (like table salt, NaCl, and other salts, like
    MgO, and other ionic compounds)
  • See board

17
Molarity
  • Molarity is the number of moles of solute in a
    liter of solution.

18
A one molar (1M) solution contains one liter of
solute per liter of solution.
  • 1M 1 mole solute per liter of solution.
  • The molar mass of NaCl is 58.6 grams/mole.
  • How many grams of NaCl do I need to make two
    liters of a 1M NaCl solution?
  • 58.6 grams NaCl x 1 mole x 2 liters
    117.2 grams NaCl
  • mole liter

19
SOLUBILITY
  • Solubility reflects how much (mass) of a
    substance can dissolve in 100 mL of water.
  • The main variable that affects how much of a
    substance can dissolve in a solvent is
    TEMPERATURE.
  • As a rule, the higher the temperature, the
    greater the solubility. WHY?

20
Interpreting graphs
  • What two variables are shown in this graph?

21
  • At what temperature are the solubilities of
    sodium nitrate and potassium nitrate the same?

22
  • Which of the three salts is MOST sensitive to
    change in temperature?
  • Which of the salts is LEAST sensitive to
    changes in temperature?

23
  • What is the solubility of KNO3 at 50oC?
  • What is the solubility of NaNO3 at 20oC?

24
  • Which salt is most soluble in water at 10oC?
  • Which salt is most soluble in water at 90oC?
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