Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry 30 > Unit 4 > Flashcards

Unit 4 Flashcards

1
Q

Equilibrium

A

A reversible equivalent between chemicals, where the rate of forward and reverse reactions are equal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Conditions of equilibrium

4 conditions

A
  1. Rate of Reverse and forward reactions are the same
  2. Properties of the system are also at equilibrium (temp, pressure, pH, concentration)
  3. Must be in a closed system
  4. Equilibrium can be approached from either direction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Physical equilibrium

3 situation

A
  1. Solid in contact with a solution containing its aqueous form
  2. Gas above a liquid
  3. A vapor above a solid
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Homogeneous equilibrium

A

chemical equilibrium where reactants and products are in the same phase

Gas Solid or Liquid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Heterogeneous equilibrium

A

Chemical equilibrium where reactants and products are in different phases

Gas Solid or Liquid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Law of chemical equilibrium

A

in an equal chemical system there is a constant ratio between concentrations of products and reactants

Kc expression

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Equilibrium expression

A

K= Products/reactants concentrations

(K>1) Products favored
(K< 1) Reactants favored
(K=1) aproximatly equal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Le Chatelier’s Principle

A

an equilibrium will try to undo the effects of any changes on its conditions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Equilibrium Shift Left

A

the reaction increases the concentration of the reactants and decreases the products

Reaction favors the reactants

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Shift to the Right

A

the reaction increases the concentration of the products and decreases the reactants

Reaction favors the products

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

(in Equilibrium)

If Reactants increase, the system…

A

decreases the amount of reactants

shift right —>

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

(in Equilibrium)

If Reactants decrease, the system…

A

Increases the amount of reactants

Shift Left <—

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

(in Equilibrium)

If Products Increase, the system…

A

Decreases the amount of products

Shift left <—

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

(in Equilibrium)

If products decrease, the system…

A

Increases the amount of products

Shift Right —>

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

(in Equilibrium)

If the temp increases in an endothermic reaction, the system…

A

tries to decrease the temperature (absorbs thermal energy)

Shift Right —>

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

(in Equilibrium)

If the temp decreases in an endothermic reaction, the system…

A

tries to increase the temperature (releases thermal energy)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

(in Equilibrium)

If the temp Increases in an exothermic reaction, the system…

A

tries to decrease the temperature (absorbs thermal bonds)

Shift left <—

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

(In equilibrium)

If the temp decreases in an exothermic reaction, the system…

A

Trying to increase the temperature (releasing thermal bonds)

Shift right —>

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Change in concentration graph

A

One concentration will change sharply and the others will gradually follow suit

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Change in temperature graph

A

No sharp changes, all concentrations will gradually change

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

(in equilibrium)

If the volume decreases AND/OR the pressure increases, the system…

A

will shift to the side of the reaction with the fewer moles of gas to make it “less crowded”

shift to the side with more moles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

If the volume increases AND/OR the pressure decreases, the system…

A

will shift to the side of the reaction with more moles of gas to add to the “crowd”

Shift to the side with more moles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

In equilibrium

Volume and pressure changes rules

4 rules

A
  1. increase V = increase P
  2. Decrease V = decrease P
  3. Moles of gas added = increase P
  4. If a reaction has the same number of moles of gas on both sides, the volume and preassure changes has no effect
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Change in Volume and pressure graph

A

All gasses have a sharp increase or decrease and then gradually return to a new steady level

25
Q

catalyst in an equilibrium affect

2 effects

A
  • speeds up the rate of reaction by lowering activation energy (by the same amount for fwd and rev reactions)
  • Equilibrium is reached faster
26
Q

Arrhenius Acid

A

a substance that will ionize in water to produce H3O+

27
Q

Arrhenius Base

A

A substance that will dissociate in water to produce OH-

28
Q

Brønsted-Lowery Theory

A

An acid-base reaction is the transfer of a proton (H+) from the acid to the base (establishes equilibrium)

29
Q

Brønsted-Lowery Acid

A

A substance that can donate a proton (H+)

30
Q

Brønsted-Lowery Base

A

A substance that can accept a proton (H+)

31
Q

Conjugate Acid-base pair

A

two substances (on either side of an equilibrium) that differ because of the transfer of a proton

32
Q

Conjugate base

A

when an acid loses a proton

33
Q

Conjugate Acid

A

when a base gains a proton

34
Q

Amphiprotic/Amphoteric substances

A

can act as both an acid and a base depending on the reaction

Ex: H2O can become OH- or H3O+

35
Q

Polyprotic Acid

A

An acid with more than one proton that can be donated

The conjugate base of a polyprotic acid becomes amphiprotic

36
Q

Polyprotic Base

A

A base that can accept more than one proton

The conjugate acid of a polyprotic base becomes amphiprotic

37
Q

Strong acid traits

4 traits

A
  • react completely in water
  • Top left of the acid and base table
  • Ka>1
  • such weak conjugate bases they wont react as bases
38
Q

Weak acids and weak bases traits

2 traits

A
  • middle of the acid base table
  • weak conjugate bases and acids
39
Q

Strong bases traits

3 traits

A
  • bottom right of the acid base table
  • includes all oxides and hydroxides of group one and group two (under beryllium)
  • such weak conjugate acids they wont react as acids
40
Q

Hydronium Ion

A

strongest acid entity that can exist in an aqueous solution

H3O+

41
Q

Hydroxide Ion

A

Strongest base entity that can exist in an aqueous solution

OH-

42
Q

Acid ionization constant equation

A

HA(aq) + H2O(l) = H3O+(aq) + A-(aq)
(Ka= [H3O+][A-]/[HA])

43
Q

Percent ionization equation

A

% = [H3O+]/[HA] x 100

44
Q

Base Ionization constant equation

A

B(aq) + H2O(l) = OH-(aq) + HB+(aq)
(Ka= [HB+][OH-]/[B])

45
Q

Titration

A

lab method used to determine the concentration of a sample

46
Q

Titrant

A

substance with a known concentration used in a titration (in the burette)

47
Q

Sample

A

Substance of an unknown concentration used in a titration (in the flask)

48
Q

Indicator

A

substance that changes colour in a titration when the sample has fully reacted

49
Q

Titration curve

A

a graph showing the pH of a titration vs. the volume of titrant added

50
Q

Endpoint

A

the point when the sample changes colour

51
Q

Equivalance point

A

The point where the sample has fully reacted

52
Q

4 possible acid-base titrations

with pH equivalence points

A
  1. Strong acid + strong base = pH 7
  2. Weak acid + strong base = pH>7 (basic)
  3. Strong acid +weak base = pH< 7 (acidic)
  4. Weak acid + weak base = equilibrium
53
Q

Buffer

A

A solution containing large equal amounts of a weak acid and its conjugate base (makes it resistant to changes in pH)

54
Q

Adding an acid to a buffer

3 things

A
  • Eq Shift Left
  • lowers H3O+
  • Buffer resists change to pH
55
Q

Adding a base to a buffer

3 things

A
  • Eq. Shift right
  • increases H3O+
  • Buffer resists change to pH
56
Q

Bicarbonate buffer system

A
  • occurs in the human body
  • maitains a pH of 7.35
  • If it gets too low (like from exersize) the buffer shifts LEFT, increasing CO2
  • If gets too high (like from hyperventilation) the buffer shifts RIGHT, increasing H3O+
57
Q

Acidosis

A

Bicarbonate buffer has been overwhelmed; Blood is too acidic

58
Q

Alkalosis

A

Bicarbonate buffer has been overwhelmed; Blood is too basic

Chemistry 30 (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions