DAY 1&2

Solutions

Matter- substances vs mixtures

solvent: (yellow/blue/green) colored liquid which was the part that _________ solute: (yellow/blue/green) colored liquid which was the part that______________ solution: (yellow/blue/green) colored liquid which was the part that _____________

Demo #1: Making a solution

Solvation: making a solution

Video Clip #1Video Clip #2PhET

How does solvation happen between salt and water?

Lets make a solution continued

When watching the clip, make sure you can explain why the rate of dissolving is affected by:

1. Hot versus cold water 2. Size of solute (particle size) 3. Stirring versus not stirring

Video Clip

Factors that affect solution formation

Ways to increase the opportunities of solute 1. Higher temperature

a. faster moving solvent particles = more collisionsb. solute breaks free faster

2. Agitation (stirring)c. faster moving particles= more collisionsd. Solute breaks free fastere. Sweeping away the dissolved portion

3. Smaller Particle Sizef. more total surface area = more possible collision

sites

Likes Dissolve Likes

1. Have you ever used Italian dressing or any kind of vinaigrette? Why do you have to shake the bottle before you using it? Why does this happen?

2. Have you ever washed your hands after getting oil on them? What happens if you just rinse them with water? Why is this?

Blue colored isopropyl alcohol (C3H7OH), Red colored water ( H2O), & Yellow Vegetable oil (C6H5O6) are mixed

together.Now, answer the following: 1. What happened when all three were added

together? 2. Explain why these observations make sense. 3. What did the color change represent?4. Why is water considered to a universal

solvent? 5. Compare the terms Soluble and Insoluble.

Demo #2: Likes dissolve Likes

Conclusion to demo: Water is polar or nonpolar Isopropyl alcohol is polar or nonpolar Vegetable oil is polar or nonpolar

Likes Dissolve Likes

Likes Dissolve Likes

Water:

Carbon Tetrachloride:

Likes Dissolve Likes

Solutes Molecular Shape if applicable

Polar, Ionic, or Nonpolar

Solvents Carbon

Water Tetrachloride

Potassium Nitrate

Soluble orInsoluble

Soluble orInsoluble

Iodine Soluble orInsoluble

Soluble orInsoluble

Boron Trifluoride

Soluble orInsoluble

Soluble orInsoluble

Nitrogen Trichloride

Soluble orInsoluble

Soluble orInsoluble

Look at the image below, what word would you use to describe: miscible or immiscible.

Look at the image below, what word would you use to describe: miscible or immiscible.

Demo # 3

Determine if the following are strong, weak, or nonelectrolytes. Explain why the observations make sense.

1. Solid NaCl2. NaCl (aq)3. C12H22O114. 1M HCl (strong acid)5. 6M HCl (strong acid) 6. HC2H3O2 (weak acid)

Electrolyte vs Nonelectrolyte

Electrolytes: conduct electricity Ionic substances and strong acids

The higher the concentration the stronger the electrolyte. Why do you think this is?

Chemistry Music Video

SOLUTION SONG

Formula: moles of solute Liter of solution

*** remember if your solute is given/measured in grams you can convert to moles by using molar mass ( unit 5)

Molarity

Unit(s) : moles/L or molar or M (which stands for molar) or [value in

brackets]

ex: 3 moles/L or 3 molar or 3M or [3]

Molarity

Vocab; Concentrated: a lot of solute per solvent Dilute: small amount of solute per solvent

Think of the following scenario: Your making chicken & stars soup, you

dump the can into a bowl (this is concentrated) and then you add water (making it more dilute).

Molarity

1. A saline solution contains 0.90 g NaCl in exactly 100mL of solution. What is the molarity of the solution?

2. How many moles of solute are present in 1.5L of 0.24M Na2SO4?

Examples

Molarity by Dilution

Purpose: making a more dilute solution Formula: M1V1 = M2V2

How many milliliters of a stock solution of 2.00M MgSO4 would you need to prepare 100.0 mL of 0.400M MgSO4?

FOR THOSE ABOUT TO DISSOLVE WE SOLUTE YOU

Chemistry Music Video

Colligative Properties

1. Why do we salt the roads in the winter? How does it work?

2. Why would you add salt to a pot of water before it boils?

3. Why do you add antifreeze to your car in the winter? How does it work?

4. Why do you add coolant to your car in the summer? How does it work?

Colligative Properties

When a solute is added to a solvent, it can change some solvent properties like:

- raising the boiling point - lowering the freezing point

Colligative Properties: vapor pressure

When adding a solute to a solvent, it (decrease/increases) the vapor pressure of the liquid.

Colligative Properties: freezing point

Book ClipWhen adding a solute to a solvent, it is harder for the solvent to form a _______ network. So more energy needs to be removed resulting in a (lower/higher) temperature at which it becomes a solid (freezing point). The more solute added the (lower/higher) the freezing temperature.

Colligative Properties: boiling point

Book ClipBoiling is when the _____pressure =

atmospheric pressure. When a solute is added (more/less) energy needs to be added to cause the vapor pressure to equalize with the atmospheric pressure. Therefore the temperature at which a solution boils is (higher/lower) than the pure solvent.