1. Solutions

2. Vocabulary Solution: homogeneous mixture (can be S, L, or G)
Solute: substance that dissolves
Solvent: substance in which the solute dissolves

3. Vocabulary Cont’d Insoluble: substance that cannot be dissolved
Soluble: substance that can be dissolved
Miscible: 2 liquids mix completely
Immiscible: 2 liquids that do not mix completely

4. Soluble vs. Insoluble
“Like dissolves Like” Rule: Only substances that are similar/alike will dissolve into one another
Polar and Polar (dissolve)
Nonpolar and Nonpolar (dissolve)
Polar and Nonpolar (do NOT dissolve)
Water is Polar! (IMPORTANT)

5. Water
Must be able to draw water!

6. Saturation
Unsaturated: when a solution can hold more solute and it does dissolve
Saturated: when a solution cannot dissolve any more solute
Supersaturated: contains more solute than a saturated solution at the same temperature
extremely unstable and if a small amount of solute (seed crystal) is added the excess solute quickly falls out of solution (Example: hand warmers, rock candy, and cloud seeding)

8. SUPERSATURATED SOLUTION
Solubility
UNSATURATED SOLUTION
more solute dissolves
SATURATED SOLUTION
no more solute dissolves
SUPERSATURATED SOLUTION
becomes unstable, crystals form
increasing concentration

10. Heat of Solution
Endothermic: energy is put into the compound (feels cold)
Exothermic: energy is released from the compound (feels hot)
The overall change is the heat of solution

11. Dissolving & Solubility
Factors that can effect the RATE (how fast/slow) dissolving:
Temperature
Stirring/Agitation
Surface Area

13. Temperature and Solubility
Solids
Increase Temp. will Increase Dissolving (Solubility) Decrease Temp. will Decrease Dissolving (Solubility)
Gases (Different from Solids)
Increase Temp. will Decrease Dissolving (Solubility) Decrease Temp. will Increase Dissolving (Solubility)
Increase Pressure will Increase dissolving.
Decrease Pressure will Decreases dissolving.

14. Solids dissolved in liquids Gases dissolved in liquidsTo
Sol. To
Sol.
As To , solubility
As To , solubility

15. Water and Oxygen
Dissolved Oxygen – The amount of oxygen that is dissolved in water
If dissolved oxygen is too low, animal and aquatic life is unable to survive and the water becomes toxic
Happens commonly in lakes and ponds during the summer months

16. Temperature and Solubility
Solubility of a gas increases as the external pressure increases
When pressure on the outside decreases some of the gas escapes.
Henry’s Law – At a given temperature the solubility (S) of a gas in a liquid is directly proportional to the pressure (P) above liquid
S1P2 = S2P1

17. Practice
If 0.24 g of a gas dissolves in 1.0L of water at 1.5 atm of pressure, how much of the gas will dissolve if the pressure is raised to 6.0 atm? Assume the temperature is held constant.
The solubility of a gas changes from 0.95 g/L to 0.72 g/L. If the initial pressure was 2.8 atm, what is the final pressure?

18. Concentration
How much solute is dissolved in a specific amount of solvent or solution.
Can be expressed as
Percent by mass
Percent by volume
Molarity

19. Percent by Mass (Mass of solute/Mass of solution) x 100
Used when a solid is dissolved in a liquid
Mass of solution is equal to the mass of the solute + the mass of the solvent

20. Percent by mass problems
In order to maintain a sodium chloride concentration similar to ocean water, an aquarium must contain 3.6 g of NaCl per 100 grams of water. What is the percent mass of the solution?
What is the percent by mass of NaHCO3 in a solution containing 20 grams of NaHCO3dissolved in 600 ml of water?

21. You have 1500 grams of bleach solution
You have 1500 grams of bleach solution. The percent by mass of the solute is 3.62%. How many grams of NaOCl are in solution?
How many grams of solvent are in the solution?

22. Percent by Volume
Usually describes solutions where both solute and solvent are liquids
Volume of solute/Volume of solution x 100

23. What is the percent by volume of ethanol in a solution that contains 35 ml of ethanol distilled in 115 ml of water?
If you have 100 ml of a 30% aqueous solution of ethanol, what volumes of ethanol and water are in the solution?
What is the percent by volume of isopropyl alcohol in a solution that contains 24 ml of isopropyl alcohol in 1.1 L of water?

24. Molarity Its unit is a M = mol/L Moles of solute/Liters of solution
A ml solution contains 5.10 grams of Glucose (C6H12O6). What is the molarity of this solution? The molar mass of glucose is g/mol

25. Calculate the molarity of 1. 60 liters of a solution containing 1
Calculate the molarity of 1.60 liters of a solution containing 1.55 grams of dissolved KBr.
What is the moles of solute in a solution with a molarity 9.5 M and 25 mL of solution?
What is the molarity of an aqueous solution containing 40 grams of glucose in a 1.5 L of solution?

26. A 100. 5 ml IV solution contains 5. 10 grams of Glucose (C6H12O6)
A ml IV solution contains 5.10 grams of Glucose (C6H12O6). What is the molarity of this solution? The molar mass of glucose is g/mol

27. Making a molar solution
Using the molarity of the solution figure out how many moles of the solute will be needed.
Using the moles of solute, convert it to grams of solute
How many grams of CaCl2 would be dissolved in 1.0 liters of a .10M solution?
A liter of 2M NaOH solution has how many grams of NaOH?

28. How many grams of CaCl2 should be dissolved to make 500 ml of a
How many grams of CaCl2 should be dissolved to make 500 ml of a .20M solution?
How many grams of NaOH are in 250 ml of a 3.0M solution?

29. Diluting a stock solution
Stock solution is a concentrated solution
M1V1 = M2V2
What volume in ml of 2.00M CaCl2 stock solution would you use to make 0.50 L of 0.300M calcium chloride solution?
What molarity of a 300 mL KI stock solution would you use to make L of a 1.25 M KI solution?

30. If you dilute 20. 0 ml of a 3. 5M solution to make 100
If you dilute 20.0 ml of a 3.5M solution to make ml of solution, what would the molarity of the diluted solution be?
How many ml of a 5.0M H2SO4 stock solution would you need to prepare 100 ml of 0.25 M H2SO4?

31. Viscosity Fluids resistance to flow
Fluid pours fast ________ viscosity
Fluid pours slow ________ viscosity

32. Dissolving
Ionization: The breaking up of a compound into separate ions
Electrolyte: A substance whose aqueous solutions conduct electricity
Nonelectrolyte: A substance whose aqueous solutions do not conduct electricity

33. Name
Formula
Ionic / Covalent
Soluble / Insoluble
Electrolyte or
Precipitate