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SCH4U1 - Chemistry > Equilibrium > Flashcards

Equilibrium Flashcards

1
Q

Chemical EQ

A

All R & P reach constant C in a closed system

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2
Q

Dynamic EQ

A

Rates F & B are equal (usually)

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3
Q

EQ Position

A

Relative C of R & P in a sys in a dynamic EQ

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4
Q

K Values change based on

A
  • Temp, closed system
  • Stays the same regardless of C
  • k = P/R
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5
Q

Heterogeneous EQ

A
  • Sys has more than 1 state
  • Pure liquids, & solids C can’t change, therefore not included
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6
Q

Magnitude of K

A
  • K < 1: R over P
  • K = 1: P & R are similar
  • K > 1: P over R
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7
Q

Le Châtelier Principle

A

When chem sys at EQ is changed, sys will do the opposite to return to EQ

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8
Q

EQ Shift

A

C of R & P are restored to EQ

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9
Q

More R added

A

EQ shifts R, to P

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10
Q

Less R added

A

EQ shifts L, to R

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11
Q

If endo rxn cooled

A

Shift L bc R has to decrease

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12
Q

If endo rxn heated

A

Shift R bc increase of nrg to make more P

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13
Q

If exo rxn cooled

A

Shift R bc nrg is released to counteract change

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14
Q

If exo rxn heated

A

Shift L bc nrg will be used as P to R

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15
Q

Partial Pressure

A
  • Pressure a gas in a mixture would exert, even alone
  • P inverse to V (if V halved, P double)
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16
Q

Factors that changes EQ Sys w/o EQ position

A
  • Catalysts
  • Inert gas: unreactivity helps pressure but not partial pressure
  • States: EQ only affected by C in same state
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17
Q

If Q < K

A

EQ shifts R

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18
Q

If Q = K

A

Sys at EQ

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19
Q

If Q > K

A

EQ shifts L

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20
Q

Solubility EQ

A

Dynamic EQ btwn solute & solvent in a sat sol

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21
Q

Ksp

A

Value from EQ law in a sat solution based on temp

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22
Q

Molar Solubility

A
  • The amount of mol dissolved in 1 L of sat sol
  • Combines to calculate for Ksp
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23
Q

If Q > Ksp

A

Solubility shifts L, precips happens

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24
Q

If Q < Ksp

A

Solubility shifts R, no precip

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25
Q

If Q = Ksp

A

EQ, no precip or C change

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26
Q

Common Ion Effect

A

Decrease of solubility of ionic compound bc of presence of ion existing in both compounds

27
Q

Arrhenius Theory of Acids & Bases

A

Acids will make H, bases makes OH

28
Q

Bronsted-Lowry Theory

A

Acids are H donors, bases are H acceptors

29
Q

CA

A

Acid formed when base accepts H from acid

30
Q

CB

A

Base formed when acid loses H to base

31
Q

Amphiprotic

A

Able to donate or accept H

32
Q

If H2O is stronger base than basic sol

A

EQ shifts R

33
Q

If basic sol is stronger than H2O

A

EQ shifts L

34
Q

Strong acids make

A

Very Weak CB

35
Q

Weak acids make

36
Q

Bases with grp 1 & 2 are

A

Strong bases

37
Q

Strong bases make

A

Very Weak CA

38
Q

Weak bases make

39
Q

% Ionization

A

C of ionized acid/initially C of acid

40
Q

Salts

A

Solid, ionic compound at SATP

41
Q

If cation is from grp 1 or 2

42
Q

If anion is a CB to a strong acid

43
Q

Anions make

44
Q

Cations make

A

Acidic Sol

45
Q

If anion is a CB to a WA

A

Rxn will make basic sol

46
Q

If cation is a CA to a WB

A

Rxn will make acidic sol

47
Q

If both ions react

A

Anything can happen, must compare Ka & Kb values

48
Q

If Ka > Kb

49
Q

If Ka < Kb

50
Q

If Ka = Kb

51
Q

Metallic Oxides form

A

Basic solutions

52
Q

Non-metallic Oxides form

A

Acidic Solutions

53
Q

Buffer

A
  • Aq sol w/ its CAB pair to keep pH constant (WA/B + conjugate ion)
  • Stops ions from accumulating, replaces another ion
54
Q

Acidic Buffers have

A

WA + CB ion

55
Q

Basic Buffers have

A

WB + CA ion

56
Q

When acid is added to a buffered sol

A

H reacts w/WB

57
Q

When base is added to buffered sol

A

OH reacts w/WA

58
Q

Buffering Capacity

A

Buffer’s ability to resist change in pH

59
Q

Strong Acid + Weak Base

60
Q

Strong Base + Weak Acid

61
Q

Strong Acid + Strong Base

62
Q

Very Weak Acids make

63
Q

Very Weak Bases make

SCH4U1 - Chemistry (6 decks)

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