1. SOLUTION CHEMISTRY

3. Adhesion is an attraction between different substances.
C. Adhesion
Adhesion is an attraction between different substances.
Water molecules are attracted to many other polar substances.
Adhesion causes a behavior known as capillary action.
Cohesion causes water to form drops
Surface tension causes them to be round
Adhesion keeps the drops in place

4. D. Density in Liquid & Solid States
As the temperature decreases, the forming of hydrogen bonds creates a crystalline structure which is very "open”.
This “openness” created actually lowers the density of water as it freezes.
The empty space between the molecules lowers the over all mass for a given volume.
Which state of water has the greatest density? LIQUID
E. The Universal Solvent
The polarity of water enables many substances to dissolve into it.
Ionic compounds and polar molecules dissolve best in water. (Ex: salt)
Nonpolar molecules do not dissolve well in water. (Ex: Oil)
The polar nature of water, which is very strong, causes water to be considered the greatest dissolving agent known to man.

5. *** PRACTICE PROBLEMS:
Which property of water causes attraction between molecules of liquid water?
Which state of water has the greatest density and why?
Describe the property of water that allows fish to survive through severe winters:

6. SOLUTIONS:
Mixtures with properties throughout

7. Solutions . . . Need to know…
1. Substances that are capable of being dissolved are called soluble.
2. Substances that are incapable of being dissolved are called insoluble.
3. The dissolving medium in a solution is called the solvent.(what is doing the dissolving)……. usually water, but not always!!!!
4. The substance dissolved in a solution is called the solute. (what is being dissolved)
5. Solutions may exist as solids, liquids or gases.
**All solution are not necessarily liquids!!!
6. Miscible liquids are able to dissolve freely in one another in any proportion.
7. Immiscible liquids are not soluble in each other(forms layers).
Miscible and immiscible refer to liquid-liquid solutions, only.

8. SOLUTE SOLVENT EXAMPLE
Gas
Liquid
Solid
solid
A insoluble solid that collects at the bottom of a solution is a ____________________
Determine if the following are miscible or immiscible
Rubbing alcohol and water (miscible / immiscible)
Oil and water (miscible / immiscible )

9. “Like Dissolves Like” Rate of Dissolution:
1. Polar and ionic solutes dissolve in polar solvents.
2. Non-polar solutes dissolve in non-polar solvents.
3. Most compounds are either polar or ionic. Water is a polar solvent. Therefore water is universal solvent
Rate of Dissolution:
Solubility:
refers to how quickly a solute dissolves
refers to the amount of solute that can be dissolved at a specific temperature.

10. Increase surface area of solute (crush/grind)
Dissolution Rate of a Solid
Solubility of a
Solid
Gas
Heating Solution
Increase ↑
Decrease ↓
Agitating Solution
(stir or shake)
No effect
Increase surface area of solute (crush/grind)
Increasing Surface Pressure of Solution

11. Solubility & Concentration
Level of concentration
gdsdf
Unsaturated Solution contains less dissolved solute than the maximum amount at a given temperature *More can be dissolved*
Saturated Solution contains the maximum amount of dissolved solute at a given temperature No more can be dissolved
Supersaturated Solution contains more than the maximum amount of solute at a given temperature. Unstable – if disturbed, the excess solute will crystallize out of solution

13. Using Solubility Curves
**Shows the dependence of solubility on temperature.
1. Any amount of solute below the line indicates the solution is unsaturated at a certain temperature.
2. Any amount of solute above the line in which all of the solute has dissolved shows the solution is supersaturated
3. If the amount of solute is above the line but has not all dissolved, the solution is saturated and the extra grams of solute have precipitated (settled) to the bottom. (# of grams precipitated = total # grams in solution - # of grams of a saturated solution at that temperature

14. Which substance maintains almost constant solubility over the temperature range?
Which substance decreases in solubility?
What is the solubility of KClO3 at 600C ?
A solution containing 50 g CaCl2 in 100 g H2O is prepared at 100 C. Is the solution saturated, unsaturated or supersaturated?
A supersaturated solution at 100C contains 40 g KCl in 100 g of H2O. At what temperature was the solution saturated before being cooled to 100C ?
If the supersaturated solution in the previous question is disturbed, how many grams of KCl will fall out of solution? (Suddenly Crystallize)

15. Electrolytes: A substance that dissolves in water to make a solution that can conduct electrical current
A. Any soluble, ionic compound is an electrolyte
B. Some highly polar covalent molecules, such as strong acids, are
also electrolytes.
Questions to ask to determine if a substance is an electrolyte:
Is the substance ionic?
Is the substance soluble in water? (dissolve)
CaCl2
H2SO4
NaOH

16. ***DISSOCIATION REACTIONS (Only occur if a substance is soluble (able to be dissolved) in water. Determine if the following compounds are electrolytes. If they are, write the dissociation reaction:
CaCl2
H2SO4
NaOH
Li3PO4
BaSO4

17. CONCENTRATION –measure of the amount of solute in a given amount of solvent or solution.
MOLARITY – (M) is the number of moles of solute in one liter of solution. (any solvent, not just water).
If you are given mass, you will need to divide by the molar mass in order to find mol of solute.
Molarity is designated by using the capital “M” directly after the number. MOLAR refers to molarity.
**As you increase molarity, the solution is more CONCENTRATED……low molarity means you have a dilute solution, and high molarity means you have a CONCENTRATED solution

18. EXAMPLES:
. What is the molarity of a solution that contains 1.54 mol NaCl in 3.5 L solution?
. How many moles of HCl are required to prepare
0.8 L of a 0.5 M HCl solution?
. If 35.8 g of LiOH are dissolved in enough water to make 750 ml of solution, what is the molar concentration (molarity) of the solution?

19. DILUTIONS More Concentrated Less Concentrated (Diluted)
Imagine we have a salt water solution with a certain concentration. That means we have a certain amount of salt (a certain mass or a certain number of moles) dissolved in a certain volume of solution. Next we'll dilute this solution - we do that by adding more water, not more salt:
More Concentrated
Less Concentrated (Diluted)

20. V1M1 = V2M2
What volume of concentrated sulfuric acid, 18.0 M, is required to prepare 5.00 L of M solution by dilution with water?

21. 1. A chemist starts with 50. 0 mL of a 0
1. A chemist starts with 50.0 mL of a 0.40 M NaCl solution and dilutes it to mL. What is the concentration of NaCl in the new solution?

22. 2. A chemist wants to make 500. mL of 0. 050 M HCl by diluting a 6
2. A chemist wants to make 500. mL of M HCl by diluting a 6.0 M HCl solution. How much of that solution should be used?

23. 3. How much 2. 0 M NaCl solution would you need to make 250 mL of 0
3. How much 2.0 M NaCl solution would you need to make 250 mL of 0.15 M NaCl solution?