1. Unit 2: Solutions

2. Solutions Unit Overview
Thursday 10/5: Introduction to Solutions Video. Start “Saturated and Unsaturated Solutions”
Friday 10/6: “Saturated & Unsaturated Solutions”. Work on Independent Practice #1 with extra time
Monday 10/9: “Solubility” & Solubility Curves
Tuesday 10/10: Solubility Curves. Independent Practice #1 is Due
Wednesday 10/11: Quiz #1. Introduction to the Mole
Thursday 10/12: Molar Mass Problems
Monday: Molar Mass Problems / “Molarity”
Tuesday/Wednesday: “Molarity” and Independent Practice #2 Due (end of class)
Thursday 10/19: Review Independent Practice #2 & Quiz #2
Friday 10/20: Review
Monday: Unit 2 Exam

3. Wednesday Learning Objectives: Components of a Solution
Classify mixtures as heterogeneous or homogeneous
Classify heterogeneous mixtures as suspensions or colloids
Define solute, solvent, and solution
Describe a solution as saturated or unsaturated

4. Solutions Video While you are watching, take notes about:
The different types of mixtures
What makes them unique

6. Post video check in! 1. What is not a characteristic of a mixture?
Two or more components are combined with one another
A chemical change occurs within a mixture
Elements in a mixture are combined without creating a chemical reaction
All of the above

7. Post video check in! 2. What are the three main types of mixtures?
Girded, lattice, suspension
Solid, liquid, gas
Solution, colloid, suspension
None of the above

8. Post video check in! 3. What is a characteristic of a solution?
The particles are visible and identifiable with the naked eye
The particles are too small to be visible with the naked eye
They contain emulsifiers that help two substances that do not blend
All of the above

9. Matter Pure Substances Elements Compounds Mixtures Homogeneous
Heterogeneous
Anything that:
Has mass
Takes up space (has volume)
A collection of identical particles
A collection of two or more different particles
A collection of single atoms of the same kind
Two or more different types of atoms chemically combined
 A mixture which has uniform composition and properties throughout
 A mixture where the parts remain separate after they are mixed

10. Saturated & Unsaturated Solutions
Start working on the Saturated & Unsaturated Solutions POGIL as a team!

11. Thursday Describe a solution as saturated or unsaturated
Learning Objectives:
Components of a Solution
Classify mixtures as heterogeneous or homogeneous
Classify heterogeneous mixtures as suspensions or colloids
Define solute, solvent, and solution
Describe a solution as saturated or unsaturated

12. Saturated & Unsaturated Solutions
Work as a team to complete the saturated and unsaturated activity
When you are done, take the check in quiz. (write the answers on your own paper – the quiz is too tiny for writing )
Take a look at the key - If you got a 100% on the check in quiz, move on to solubility
If you get less than 100% on the check in quiz, review the activity and go over your independent practice questions before you move on to solubility

13. Friday Learning Objectives: Read and interpret Solubility Curves
Use solubility curves to determine solubility of a substance when given a temperature

14. Monday 10/9/17 Learning Objectives:
Read and interpret Solubility Curves
Use solubility curves to determine solubility of a substance when given a temperature
We’ll start by talking about last week – including the exam 
Looks like some people still need to finish!
Have your binder out and your work from last week.

15. NEW PLAN Today (Monday) Tuesday Wednesday Thursday
Finish Exam (as needed)
Quick Notes
Check in on Saturated vs. Unsaturated
Solubility
Check in on Solubility
Tuesday
Solubility Curves
Finish Independent Practice #1
Wednesday
Quiz 1 (pick up Independent Practice #2
Thursday
What is a MOLE?
Mass to Mole Conversions

16. Matter Pure Substances Elements Compounds Mixtures Homogeneous
Heterogeneous
Anything that:
Has mass
Takes up space (has volume)
A collection of identical particles
A collection of two or more different particles
A collection of single atoms of the same kind
Two or more different types of atoms chemically combined
 A mixture which has uniform composition and properties throughout
 A mixture where the parts remain separate after they are mixed

17. Recap from last week
Solution: A type of homogenous mixture which has uniform composition and properties throughout. Particles are too small to be visible with your eyes
Solute: the stuff you are adding to the solvent
Solvent: what you are adding the solute to
Example:
Salt water- solution
Salt – solute
Water - Solvent

18. Saturated / Unsaturated / Supersaturated
Saturated: The maximum amount of solute has been dissolved in the solvent for that volume and temperature
Unsaturated: more solute can be dissolved in the solvent at that volume and temperature
Supersaturated: more solute has been dissolved in the solvent than would be in a saturated solution. Usually done by manipulating the temperature or by evaporating some of the solvent

20. Solubility Work as a team to complete the solubility activity
When you are done, take the check in quiz. Write the answers on your own paper – the quiz is too tiny for writing )
Take a look at the key - If you got a 100% on the check in quiz, move on to the solubility curves worksheet as a group.
If you get less than 100% on the check in quiz, review the activity and go over your independent practice questions before you move on to the solubility curve activity

22. Solubility Check in! (check the key when you’re done)

23. Solubility Curves
Work with your team to complete the solubility curves practice. One per group – when you’re done, write your own question using the solubility curve given on the large paper. Write the answer on the back. When you are done work on Independent Practice #1 because we will be checking answers at the end of class

24. Wednesday 10/11/2017
WARM UP
Clear your table of everything except something to write with and a calculator.
When you are done with the quiz, pick up the molar mass notes and independent practice #2

25. Thursday 10/12/2017 Learning Target Moles & Molar Mass WARM UP
Identify number of atoms of each element when given a chemical formula.
Define the chemical mole as 6.022x1023 particles of any substance
Explain why chemists use the chemical mole as a counting number
WARM UP
Have your notes out and pick up a periodic table

26. What is a mole? 6.022 x 1023 of ANYTHING
Just like a dozen is 12 of anything, a mole is x 1023 of anything.
A mole of cats would be x 1023 of cats
A mole of eggs would be x 1023 eggs
A mole of carbon atoms would be x 1023

27. How did chemists determine the mole?

28. Why do we use it?
The mole is so extremely useful because atoms are so very small!
If we try to take the mass of individual atoms we get mass readings in AMU (atomic mass units) which aren’t super helpful.
Instead, chemists created the mole – a way of taking the mass of x 1023 atoms or particles or molecules so we can get our mass readings in grams.

29. Relative Mass and the Periodic Table
55.847 Fe 26
 Relative Atomic Mass
 Atomic Number

30. How many atoms are present in a compound?
A chemical formula for a compound represents two things:
The elements contained in the compound
The number of atoms of each element in the compound, written as subscripts
A few hints:
Each capital letter starts a new element
If parentheses are present, the subscripts inside the parentheses multiply by those on the outside to calculate a total number of atoms

31. (NH₄)₂CO₃

32. Learning Target: Moles and Molar Mass
Warm-up: How many atoms of each element are in the compound (NH₄)₂CO₃ N: H: C: O:
Learning Target: Moles and Molar Mass
Plan for today:
Review Unit 1 Exam
Review Unit 2 Quiz 1
Moles & Molar Mass

33. Molar Mass The mass of one mole of that substance (typically in grams)
EXAMPLE: (NH₄)₂CO₃
Find the Molar Mass of the above compound

34. Conversions 1 mole of a substance = the molar mass of that substance
Can use this to convert between moles of a substance and grams of a substance
EXAMPLE:
How many grams are in 1.7 moles of (NH₄)₂CO₃?
How many moles are in 654 g of (NH₄)₂CO₃?

35. Plan for Today
Finish Notes
Complete Molar Mass & Gram-Mole Conversion practice
Complete first page of Independent Practice #2

36. Molarity Work as a team to complete the molarity activity
When you are done, take the check in quiz.
If you get a 100% on the check in quiz, start studying for the quiz and exam
If you get less than 100% on the check in quiz, review the activity and go over your independent practice questions before you start studying for the quiz

37. CuCl2 (Copper Chloride)
Block Day
Warm-Up (on your paper- be ready to share out)
Calculate the Molar Mass of the following compounds:
CuCl2 (Copper Chloride)
C12H22O12 (Glucose)
Learning Target: Molarity
Define Molarity
Use molarity equation to calculate for molarity, moles, or volume
Explain the concept of molarity as it relates to concentration
Plan for today:
Molarity Notes
Trashketball

38. What is Molarity and why do we care about it?

40. “2 M” is read as “two molar”
Molarity
M= molarity
“2 M” is read as “two molar”

41. Check in
Write a mathematic equation to show how the molarity of a solution is calculated (hint: it should have three variables)

42. Use your formula to calculate the molarity of the following solution:
210 grams of Copper Chloride mixed in 400 mL of solution

43. Use your formula to calculate the molarity of the following solution:
2 moles of Glucose mixed in 4 L of solution

44. Use your formula to calculate the VOLUME of the following solution:
A 5.3M solution with 350 g of Copper Chloride

45. Calculate the molarity of a solution containing 1.5 moles of NaCl in 0.50 L of solution.

46. Calculate the molarity of a solution containing 0
Calculate the molarity of a solution containing moles of acetic acid in liters of solution

47. 74.55 g KCl (potassium chloride) in 2000 mL of solution
What is the molarity?

48. Calculate molarity
2.5 grams of Copper Chloride in 1 L of solution.

49. 37.3 grams of KCl in 500 mL of solution.

50. Calculate the molarity of a solution containing 2
Calculate the molarity of a solution containing moles of NaCl dissolved in 2L of water.

51. Calculate the number of moles of NaCl necessary to make. 5L of a 4
Calculate the number of moles of NaCl necessary to make .5L of a 4.0M solution.

52. Calculate the number of grams necessary to make. 5L of a 4
Calculate the number of grams necessary to make .5L of a 4.0M solution of NaCl.

53. Calculate the molarity of a solution where 5
Calculate the molarity of a solution where 5.6g of C2H6O2 are dissolved in 0.3L of water.

54. When sugar is dissolved in water, what term best describes the sugar?

55. How many grams of solute are contained in 64. 3mL of a 1
How many grams of solute are contained in 64.3mL of a 1.40M H2SO4 solution

56. Grams = Molarity x molar mass of the substance (g) x Liters

57. What mass of sodium sulfate Na2SO4 is present in 250 mL of a 2
What mass of sodium sulfate Na2SO4 is present in 250 mL of a M solution?

58. How many grams of NaCl are contained in 0. 350 L of a 0
How many grams of NaCl are contained in L of a 0.28 M solution of sodium chloride?

59. Calculate the number of moles in 78g of carbon monoxide (CO)

60. Molarity Work as a team to complete the molarity envelope activity.
When you are done, take the check in quiz.
If you get a 100% on the check in quiz, start studying for the quiz and exam
If you get less than 100% on the check in quiz, review the activity and go over your independent practice questions before you start studying for the quiz

61. Equations for Molarity
M = moles / liters Or
Grams = Molarity x molar mass of the substance (g) x Liters