1. Solutions

2. Solutions Solute- the substance being put into the solution.
Solvent- the substance in which the solute is being put into.
Solution- the substance that results from a solute being put into a solvent.
Example: Salt is a solute, Water is the solvent, Salt Water is the solution.

3. Types of Solutions Are all solutions liquids?! NO!
Write down some examples:
Solute
Solvent
Example Solution
Gas
Air
Liquid
Soda
Juice
Solid
Sweet Tea
Steel

4. Solutions Soluble versus Insoluble. Miscible versus Immiscible.
Soluble – dissolved in solution.
Insoluble – will not dissolve in solution.
Miscible versus Immiscible.
Miscible – “Mixable” able to mix together. (Ex. Water and Bleach)
Immiscible – Not able to mix together. (Ex. Water and Oil)

5. Types of Mixtures Solution Colloid Suspension Particle Size smallest
middle
largest
Tyndall Effect (scattering of light; or cloudy) No
Yes
Settles out/Filtration
Mixture Type
Homogeneous
Heterogeneous
Example
Salt water
Fog/Milk
Muddy water

6. Water as the Universal Solvent
What are some properties of water that make it a good solvent?
Polar molecule: dissolves other polar substances
IMF’s: High boiling point so it remains a liquid at room temperature and higher
Most abundant liquid on earth

7. “likes dissolves likes”
Polar substances dissolve other polar substances
Nonpolar substances dissolve other nonpolar substances
Polar substances do NOT dissolve nonpolar substances

8. Will they be soluble?
CH4 and H2O
NH3 and H2O

9. Will they be soluble?
CH4 and H2O – CH4 is nonpolar, H2O is polar. They will NOT be soluble.
NH3 and H2O – Both are polar. They will be soluble!

10. Solutions as Electrolytes
Electrolyte: substances that dissolve in water to give a solution that conducts electricity
Good electrolytes: substances that form IONS  ionic compounds, acids, bases
Non-electrolytes: DON’T FORM IONS: most molecular compounds (COVALENT)

11. Electrolyte Versus Nonelectrolyte
Electrolyte- Ionic compounds that dissociate (or break apart) into their charged ions. Conducts electricity
Nonelectrolyte- do not dissociate therefore they don’t conduct electricity

12. Play the Electrolytes video from the website

13. Play this video as well

14. Decide if each chemical is an electrolyte or a nonelectrolyte

15. Electrolyte or Nonelectrolyte?
NaCl
Electrolyte - Ionic

16. Electrolyte or Nonelectrolyte?
H2SO4
Electrolyte - Acid

17. Electrolyte or Nonelectrolyte?
CO2
Nonelectrolyte - covalent

18. Electrolyte or Nonelectrolyte?
C6H12O6
Nonelectrolyte - covalent

19. Electrolyte or Nonelectrolyte?
K3PO4
Electrolyte - Ionic

20. Electrolyte or Nonelectrolyte?
CCl4
Nonelectrolyte - covalent

21. Electrolyte or Nonelectrolyte?
Ca(OH)2
Electrolyte – ionic, base

22. Electrolyte or Nonelectrolyte?
HCl
Electrolyte - acid

23. Electrolyte or Nonelectrolyte?
SO2
Nonelectrolyte - covalent

24. Electrolyte or Nonelectrolyte?
KOH
Electrolyte – ionic, base

25. The Solution Process
Solvation: process by which solvent particles surround solute particles
Dissociation: separation of ionic compounds into ions
Hydration: Solvation with water as a solvent; ions are surrounded by water molecules and kept separate (H on the water is attracted to the negative ion; O is attracted to the positive ion)

26. Dissociation
The separation of ions from one another.

27. Hydration
Water molecules attach to dissolving molecules and ions.

28. Play this video:

29. Factors that Affect Rate of Solution
Increasing surface area: the smaller the crystals, the faster it will dissolve because of the greater surface area, stirring also increases surface area and rate of solution
Increasing temperature: Increases rate because particles move faster

30. More Factors that Affect Rate of Solution
Increasing pressure: GASES ONLY, increasing pressure increases the increases the rate (Think about soda)
Increasing concentration – more particles means more collisions, so rate increases
Using a catalyst – speeds up the rate by lowering activation energy

31. Solubility
Solubility refers to HOW MUCH solute can be dissolved in an amount of solvent
(Different than RATE which is the SPEED at which something dissolves)

32. Factors that Affect Solubilty
Nature of solute/solvent: Polar dissolves polar, nonpolar dissolves nonpolar, polar does NOT dissolve nonpolar
Temperature:
For solid and liquid solutes: increasing temperature increases solubility
For gas solutes: increasing temperature decreases solubility (think about soda
Pressure: GASES ONLY! Increasing pressure means MORE can dissolve (increased solubility)

33. Key Terms:
Saturated – solution is holding the maximum amount of solute that it can hold
Unsaturated – solution is holding less than the maximum amount of solute
Supersaturated – solution is holding more than the maximum amount of solute

34. Solubility Curves
Shows the amount of a solute (in grams) that will dissolve in a specific amount of water (usually 100g) at various temperatures.

35. Play Solubility Curves video

36. Try It: 1. Which substance has the highest solubility at 10°C?
2. How much KCl can 100 g of water hold at 50°C?
3. How much KCl can 300g of water hold at 50°C?
4. If a solution contains 100 g of NaNO3 at 20°C, is the solution saturated, unsaturated, or supersaturated?

37. Solution Concentration
Concentration is a measure of the amount of solute in the amount of solvent or solution.
Qualitative measures of concentration
Dilute: small amount of solute compared to the amount of solvent (could be a saturated solution)
Concentrated: large amount of solute compared to the amount of solvent

38. Play Molarity video

39. Molarity and Concentration
Quantitative measures of concentration:

40. Practice Problem 1
What is the molarity of a solution containing 5.85 grams of potassium iodide in 125 mL of solution?

41. Practice Problem 2
How many moles of sulfuric acid are present in 500 mL of a M solution?

42. Practice Problem 3
What is the mass of sodium chloride in 240 mL of a 3.00 M solution?

43. Play dilutions video

44. Diluting Solutions H2O 2M 12M M1V1=M2V2 Moles = Moles
M=mol/volume ; mol= (M)(V)
M1V1=M2V2

45. Diluting Solutions – Practice Problem
What volume of 2.00M CaCl2 would you use to make 0.5L of 0.300M CaCl2?

46. Quiz Topics Solutions Vocab Molarity Calculations
Solubility (how is it affected)
Solubility Curves
Saturated, Unsaturated, Supersaturated

47. Colligative Properties
Definition: Physical properties of a solution that are affected by the number of solute particles.
Four you need to know:
Vapor pressure lowers
Boiling point rises
Freezing point lowers
Osmotic pressure increases

48. Colligative Properites
Electrolytes:
NaCl(s)  Na+(aq) + Cl- (aq)
Since electrolytes break apart in solution, there are more particles, and therefore a bigger effect on the colligative properties
Nonelectrolytes:
C12H22O11(s)  C12H22O11(aq)
They don’t break apart in solution, so there are fewer particles, and a smaller effect.

49. Vapor Pressure Lowering
Vapor pressure lowers when a solute is present, because it is more difficult for a solvent to evaporate because of the strong IMF formed between the solute and solvent

50. Boiling Point Elevation
Adding salt (or any solute) to water increases its boiling point
Increases boiling point because more imfs between solute and solvent to break before the solution boils

51. Freezing Point Depression
Decreases freezing point because more imfs to overcome before the solution freezes

52. Osmotic Pressure The pressure needed to reverse or stop osmosis
Osmosis: the diffusion of solvent particles across a semipermeable membrane