Unit 3: Equilibrium and Acid-Base

Question 1

What is equilibrium?

Answer 1

• Balanced but not equal.
• They are exchanging in a balanced rate, but not in amount.

Question 2

What is microscopic and macroscopic properties?

Answer 2

• Microscopic: Changes in a small level
  Ex: Bonds forming/breaking
• Macroscopic: Observable, and measurable
  Ex: pH, temp, colour

Question 3

What are the requirements to stay at equilibrium?

Answer 3

1. Closed system
2. Constant temperature

Question 4

What is the equilibrium law expression?

Answer 4

Kc = [Product]ⁿ / [Reactant]ⁿ

Question 5

What are the equilibrium law expression rules?

Answer 5

1. Never include solids
2. Only include liquids if there are more than one.

Question 6

How to know which one is favoured based of the Kc?

Answer 6

• If K is greater than 1 (K>1), then products are favoured
• If K is less than 1 (K<1), then reactants are favoured.

Question 7

How to read an equilibrium graph?

Answer 7

• x-axis: time
• y-axis: concentration of all
• Concentration of reactants are decreasing, while products are increasing in the same rate
• When all lines are parallel, state of equilibrium is reached.

Question 8

What is the Le Chatelier Principle?

Answer 8

-* System at equilibrium is disturbed by any change, it does the opposite of that change. *
- Add something, then the sytem will remove, vise versa.
- It does this to move towards a state of equilibrium.

Question 9

Equilibrium Shifts #1
Concentration Change

Answer 9

• Add more of a substance, temporarily increasing it, and then it will be consumed by the system, thus shifting it to the other side.

Question 10

Equilibrium Shifts #2
Energy/Temperature Change

Answer 10

• Add heat then it will shift to the other side.
• Cool the system, it will **stay **in that side.
  Ex: Heat up an endothermic, it will move to products.
  Cool it up, it will stay in reactants

Question 11

Equilibrium Shifts #3
Volume/Pressure Change

Answer 11

Note: Volume and Pressure are inverse (V/P)
- Volume increase = shift to most amt of total moles
- Volume decrease = shift to least amt of total moles

If volume increases then pressure decreases

Question 12

Equilibrium “Shift” #4
Adding catalyst and Inert Gas

Answer 12

• Inert Gas: Noble Gases
• Adding a catalyst and inert gas does nothing

Question 13

How to read Le Chatelier Graphs?

Answer 13

Energy/Temp Graphs: All gradually changing
Volume/Pressure Graphs: All increase at once
Concentration Graph: One temporarily changed

Question 14

What is the difference between Modiefied Arrhenius Theory VS Bronsted-Lowry?

Answer 14

Modified Arrhenuis: Defines acid and base with H30+ and OH-
Bronsted-Lowry: Defines acid and base with proton donor and proton acceptor.

Question 15

What is Amphiprotic?

Answer 15

Amphiprotic: Can act as an acide or basic in different situations.

Question 16

How to go from pH to H30+ and vise versa?

Answer 16

pH = -log[H30]
[H30] = 10⁻ᵖᴴ
pH + pOH = 14

Question 17

When to use the Rule of 1000?

Answer 17

• You only use the rule of a 1000 when you do not have x
• Make sure to write down Rule of a 1000 and prove it to cancel the -x.

Question 18

How to figure out what is a monoprotic and a monobasic?

Answer 18

Monoprotics can be identified with an H at the start or -COOH.
Monobasics can be identified with a charge.

Example:
Monoprotic: HCO₃
Monobasic: PO⁻

Question 19

How to figure out if they are amphiprotic?

Answer 19

If they have an H and a charge at the same time
Example: H₂PO₄ ⁻

Question 20

What is a buffer zone?

Answer 20

Buffer Resists the change in pH

Question 21

What is Acid Deposition?

Answer 21

Acid Deposition: Acid deposited into the environment through gas burned.
Example of gases: SO2, CO, NO

Question 22

What are ways you can reduce acid deposition?

Answer 22

• Liming: Adding Calcium Carbonate
• Recycle
• Insulation
• Not driving