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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

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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
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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
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4
Q

Homogeneous equilibrium

A

chemical equilibrium where reactants and products are in the same phase

Gas Solid or Liquid

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5
Q

Heterogeneous equilibrium

A

Chemical equilibrium where reactants and products are in different phases

Gas Solid or Liquid

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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

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7
Q

Equilibrium expression

A

K= Products/reactants concentrations

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

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8
Q

Le Chatelier’s Principle

A

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

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9
Q

Equilibrium Shift Left

A

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

Reaction favors the reactants

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10
Q

Shift to the Right

A

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

Reaction favors the products

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11
Q

(in Equilibrium)

If Reactants increase, the system…

A

decreases the amount of reactants

shift right —>

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12
Q

(in Equilibrium)

If Reactants decrease, the system…

A

Increases the amount of reactants

Shift Left <—

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13
Q

(in Equilibrium)

If Products Increase, the system…

A

Decreases the amount of products

Shift left <—

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14
Q

(in Equilibrium)

If products decrease, the system…

A

Increases the amount of products

Shift Right —>

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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 —>

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16
Q

(in Equilibrium)

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

A

tries to decrease the temperature (releases thermal energy)

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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 <—

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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 —>

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19
Q

Change in concentration graph

A

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

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20
Q

Change in temperature graph

A

No sharp changes, all concentrations will gradually change

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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

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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

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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
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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

tow 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

3 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 acid = 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 an acid 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)

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