related to chemistry solutions

1. Solutions

2. Mixtures – a review
• Mixtures are made by physically mixing
two or more things together. No chemical
bonds are made.
• Two types:
– Heterogeneous
– Homogeneous

3. Heterogeneous Mixture
• “Hetero” means “different”
• You can see the different parts of the
mixture. There can be different states
(solid, liquid, gas).
• Can be separated by filtering.
• Example:

4. Homogeneous Mixture
• “Homo” means the same
• It all looks like the same material, and there
is only one state.
- We call them solutions.
• Example:
Salt Water

5. Solution
• Can be physically separated
• Dissolve: When a solid becomes part of a liquid.
• Made of solutes and solvents
the thing being dissolved
the thing that takes the solute
Sugar
(solute)
Water
(solvent)
Sugar Water
(solution)
Salt water is a
solution. How can it
be physically
separated?

6. Solution
• The solvent is the biggest part of the
solution and the solute is the smallest part of
the solution
S O L V E N T
S O L U T E

7. Types of Solutions
Gaseous solutions: air = Oxygen + Nitrogen
Liquid solutions: drinks = mix + water
Solid solutions: alloys = steel, brass, etc

8. Concentration
• Concentration = How much of the
solute is dissolved.
•The solution is dilute if it
has a low concentration of
solute.
•The solution is
concentrated if it has a high
concentration of solute.

9. Concentration
•Unsaturated solution – The
solvent can take more of the
solute.
•Saturated solution – The solvent
cannot take more of the solute.

10. Things that change how quickly solids
dissolve
Temperaturee
increased temperature makes
solids dissolve faster
Shaking
shaking makes
solids to dissolve faster
smaller particles dissolve
Faster because they have
more surface area
Particle Sizee

11. • Miscible liquids can easily mix with each
other.
• Immiscible liquids cannot mix with each
other.
Chemistry-Borders

12. • 10 minutes break

13. Molarity
(M)

14. Molarity
• Molarity is the concentration of a
solution = moles of solute per liter of
solution.
Molarity (M) = moles of solute
Liters of solution

15. Molarity
M = moles (solute)
L (solution)
• Example 1: What is the molarity of a solution
that has 2.3 moles of sodium chloride in 0.45
liters of solution?
2.3 moles NaCl = 5.1M NaCl
0.45 L

16. Molarity
M = moles (solute)
L (solution)
• Example 2: How many moles of Na2CO3 are there
in 10.0 L of 2.0 M solution?
moles = M x L
10.0 L x 2.0 M
= 20.0 moles Na2CO3

17. Molarity
M = moles (solute)
L (solution)
• Example 3: How many moles of KNO3 are needed
to make 450 mL of 1.5 M solution?
moles = M x L
0.45 x 1.5
= .675 moles KNO3

18. Dilutions
Chemistry-Borders IPC-Solutions-Borders

19. Dilutions and Molarity
• Use this formula to make a more dilute
solution from a concentrated solution
Molarity1 x Volume1 = Molarity2 x Volume2
(Concentrated) (Dilute)
(before) = (after)
M1V1 = M2V2

20. Example 1
How many liters of 2.5 M HCl are
needed to make 1.5 L of 1.0 M HCl?
M1V1 = M2V2
M1 = 2.5 M
V1 = ?
M2 = 1.0 M
V2 = 1.5 L
(2.5M) V1 = (1.0M) (1.5 L)
2.5M
2.5M
= 0.60L

21. Example 2
• 250.0 mL of a 0.500 M HCl solution needs
to be made. What volume of 12.0 M HCl is
needed to make it?
M1V1 = M2V2
M1 = 12 M
V1 = ?
M2 =0.5 M
V2 = 250mL
V1 = 10.4mL

22. Translate your notes!!!
• 20 minutes.

23. Worksheet
• Finish the worksheet in DingTalk and send
it back to me.
• M1 x V1 = M2 x V2
• M = molarity
• V = volume (mL, L…)

24. Grams to Moles
How many moles in 30 grams
of carbon?
The atomic mass number shows how many
grams in 1 mole.
12g of carbon = 1 mole of carbon

25. Grams to Moles
How many moles of carbon are
in 30 g?
30
12
= 2.5 moles

26. Grams to Moles
• How many moles of H2O are in 60g of
H2O?
• (2 x hydrogen) + oxygen
(2 x 1) + 16 = 18
60 = 3.33 moles
18

27. Questions 1-7
1. 0.5 / 0.3 = 1.67M
2. 0.289 / 0.12 = 2.41M
3. 0.0877 / 0.075 = 1.17M
4. 1.55 x 0.6 = 0.93 moles
5. 0.964 x 1.63 = 1.56 moles
6. 2.11 / 1.66 = 1.27L
7. 0.55 / 0.25 = 2.2L

28. Question 8
• Atomic mass:
• Na = 23
• Cl = 35
• 58g = 1 mole of NaCl
• 63 / 58 = 1.09 moles
• M? M=moles / L
• 1.09 / 0.65 = 1.68 M

29. Question 9
• Liters = 0.5 M = 1.66
• 1.66 x 0.5 = 0.83 moles
• Atomic mass: 40+16+16+1+1 = 74g = 1
mole
• 73 x 0.83 = 61.42g

30. Question 10
• Atomic mass: 56 + 35 + 35 = 126g = 1
mole of FeCl2
• 130 / 126 = 1.03moles
• M = 0.88
• Liters = 1.03 / 0.88 = 1.17L
• https://quizlet.com/_ckr2c2?x=1qqt&i=3x9
miq

31. Worksheets 2 + 3
• Finish the worksheets in DingTalk and
send it back to me.
• Then study on Quizlet:
• https://quizlet.com/_ckr2c2?x=1qqt&i=3x9
miq