1. Solutions
Chapter 10

2. Review of Mixtures:
Heterogeneous Homogeneous
Heterogeneous Mixtures:
suspension: large particles that settle out
colloid: particles are uneven throughout the sample (positive Tyndall Effect)

4. solute: substance being dissolved
solution: a substance is dissolved in another substance and evenly distributed
Solution Parts:
solute: substance being dissolved
solvent: substance doing the dissolving

5. Phases and Solutions

6. Solid Solution
14-karat gold is a mixture of gold, silver, and copper

7. What would a mixture of gases look like?
Gas Solution
What would a mixture of gases look like?

8. Liquid Aqueous Solution
Solutions with water as the solvent

9. SATURATION

10. saturated solution: contains the maximum amount of a solute that will dissolve in a given solvent at a specific temperature.
unsaturated solution: contains less solute than the solvent has the capacity to dissolve at a specific temperature.

11. supersaturated solution: contains more solute than a solvent has the capacity to dissolve at a specific temperature, more than a saturated solution

12. Saturation Examples

13. SOLUBILITY CURVES

14. Solubility Curves The x-axis: Temperature (oC)
The y-axis: Solubility in 100g of water
When is the solution saturated, unsaturated, and supersaturated?
Solubility in 100g H2O
Temperature oC

15. What do you get from a solubility curve?
Identify the solubility at a specific temperature.
Identify the temperature at which something can dissolve.
Identify whether something is saturated, unsaturated, or supersaturated.
Identify solubility in different amounts of water.
Identify how much will crystallize with a temperature change.

16. SOLUBILITY

17. Soluble
when a substance IS capable of being dissolved in another substance
Insoluble
when a substance is NOT capable of being dissolved in another substance

18. Soluble and Insoluble Ionic Compounds

19. How do you know if something will dissolve?

20. “like dissolves like”
Two substances with similar intermolecular forces will be soluble in each other.

21. non-polar molecules are soluble in non-polar solvents
CCl4 in C6H6
polar molecules are soluble in polar solvents
C2H5OH in H2O
ionic compounds are more soluble in polar solvents
NaCl in H2O

22. Water Molecule Polarity
polar molecule
A ________ ____________ has an uneven distribution of electrical charge, which means that each molecule has a _________  __________   region at one end and a __________  __________ region at the other end.
The water molecule has a _________ or V-shape, NOT linear H-O-H.
The __________ is an electrically negative region that has a greater concentration of _____________.
The two _____________ are electrically positive.
slightly positive
slightly negative
bent
oxygen
electrons
hydrogens

23. In the picture of water below, label the atoms and indicate the partial electrical charges.
Element: ______
Charge: ______
Element: ______
Charge: ______

24. Ionic crystals are made up of two types of ions, cations and anions.
What charge is associated with a cation?
What charge is associated with an anion?
In the example sodium chloride, identify the cation and the anion:
Sodium: ________ Chlorine: __________

25. Hydration – What happens when salt dissolves?
Color in the molecules and ions below. Next to each molecule and ion identify the charge.
Hydrogen: White Oxygen: Red Sodium: Blue Chlorine: Green
DISSOLVED means:
surrounded by WATER MOLECULES
Solvation Process Simulation

26. What will make a solute dissolve in a solvent faster?
Stirring or shaking increase contact between the solute and solvent
Break up solute increase the surface area for more contact
Increase temperature more collisions between solute and solvent

27. ELECTROLYTES

28. Electrolytes
Electrolytes: When a solute dissolves in water and the solution conducts electricity
The electricity comes from the ions that form in solution when the solute is dissolved.
Strong and weak electrolytes differ in the degree of ionization.

29. Strong electrolyte: high conductor because of high number of ions in solution.
Weak electrolyte: low conductor because of small number of ions in solution.
Non-electrolyte: solution that does not conduct electricity because there are no ions.
strong electrolyte
weak electrolyte
non-electrolyte

30. THE IONS!!! How do electrolytes conduct electricity?
Cations (+) and Anions (-)
Strong Electrolyte – 100% ions
Weak Electrolyte – very few ions
Non-Electrolyte – no ions

31. Light Board Demo Sample Prediction Actual Ions Present? Water NaCl
Sugar
Gatorade
Vinegar

32. Concentration

33. Concentration
concentration: measure of the amount of solute in a given amount of solvent or solution.
measured in: molarity, molality, parts per million (ppm), parts per billion (ppb)
The opposite of concentrated is dilute.

34. Molarity (M) moles of solute M = liters of solution Mol M L
Molarity: is the number of moles of solute in one liter of solution.
M =
moles of solute
liters of solution
Mol M L

35. Example Problem 1
You have 3.50 L of solution that contains 1.54 mol of sodium chloride, NaCl. What is the molarity of that solution?

36. Example Problem 1 Solution
Given: solute = 1.54 mol NaCl
solution volume = 3.50 L
Unknown: molarity
Solution:

37. Example Problem 2
You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution contain?

38. Example Problem 2 Solution
Given: volume of solution = 0.8 L
concentration of solution = 0.5 M HCl
Unknown: moles of HCl
Solution:

39. Colligative properites

40. Colligative Properties
colligative properties: properties that depend on the concentration of solute particles but not on their identity

41. What happens when a substance boils normally?

42. Boiling-Point Elevation
To cook the pasta faster, you add salt to the water.
Adding salt to the water is like turning the escape route of the particles into a puzzle. Since it requires more energy to escape, the water boils at a higher temperature (cooking the pasta faster).

43. What happens when a solution boils?
Draw lines to show how the particles on the bottom of the pan boil to the surface through the “puzzle”.
This is called boiling point elevation.

44. What happens when a substance freezes normally?

45. Freezing-Point Depression
In the winter, salt is thrown on the road to melt the ice. When the salt comes in contact with the ice, the ice melts and cannot reform to a solid at the same temperature.
Since the salt particles are in the way, it requires a lower temperature to get the water molecules to connect to form ice. Therefore, the water freezes at a colder temperature.

46. What happens when a solution freezes?
Connect the dots below (again with straight lines) this time with salt particles in the way.
This is called freezing point depression.