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CHEM1B > FINAL > Flashcards

FINAL Flashcards

1
Q

K =

A

[Products]/[Reactants

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2
Q

What is not included in the K expression?

A

Solids and Liquids

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3
Q

What is done to the K expression of a reaction in a Hess Law problem?

A

(1/k)^n

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4
Q

Q is the what?

A

Reaction Quotient

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5
Q

What is Q, before equilibrium?

A

Q<K

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6
Q

What is Q, at equilibrium?

A

Q=K

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7
Q

What is Q, after equilibrium?

A

Q>K

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8
Q

What principle states that the change in conditions will cause a reaction to try and counteract those changes?

A

Le Chatliers Principle

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9
Q

What are the three main changes to a reaction based on Le Chatliers principle?

A

Effect of Volume, Effect of Temperature, Concentration Effect

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10
Q

Effect of Volume

A

Increase Volume = Decrease Pressure -> rxn shifts to side with the MOST gas particles

Decrease Volume = Increase Pressure -> rxn shifts to side with the FEWEST gas particles

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11
Q

Effect of Temperature

A

Depends on whether the reaction is endothermic or exothermic.

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12
Q

Concentration Effect

A

Increase Reactant -> Product Side
Decrease Reactant -> Reactant Side
Increase Product -> Reactant Side
Decrease Product -> Product Side

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13
Q

Change in volume, Adding a Inert gas and adding a catalyst, have what type of change to a reaction?

A

No change or effect

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14
Q

What makes a substance amphoteric and what are some examples?

A

The substance can act as an acid or base
Ex: H20, HCO3-, HS-, H2PO4-

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15
Q

What is the difference between and monoprotic acid and a polyprotic acid?

A

Monoprotic acid donates one H+ and a polyprotic acid donates more than one

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16
Q

When classifying salt solutions what are the properties of strong bases and strong acids?

A

Neutral

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17
Q

When classifying salt solutions what are the properties of weak acids?

A

Basic

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18
Q

When classifying salt solutions what are the properties of weak bases?

A

Acidic

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19
Q

When classifying salt solutions what are the properties of strong highly charged cations and what are some examples?

A

Acidic
Mn2+, Cu2+, Fe3+, Al3+

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20
Q

What is the equation for pH and pOH?

A

pH = -log([H3O+]) and pH = -log([OH-])

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21
Q

pH + pOH =

A

14

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22
Q

pKa =

A

-log (Ka)

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23
Q

Kw =

A

Ka x Kb

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24
Q

What is the value of Kw?

A

1.0 x 10^-14

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25
Q

10^-pH =
10^-pOH =

A

[H3O+]
[OH-]

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26
Q

What is an Arrhenius acid and base?

A

Acid that increases the concentration of H+
Base that increases the concentration of OH-

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27
Q

What is a Bronstead acid and base?

A

Acid is the H+ donor
Base is the H+ acceptor

28
Q

What is the relationship between NH3 and NH4+?

A

NH3 is a weak base and NH4+ is a strong conjugate acid

29
Q

What is the Henderson Hasselback equation?

A

pH = pKa + log ([weak base]/[weak acid])

30
Q

What is Ka and Kb?

A

Ka = equilibrium constant for acids
kb = equilibrium constant for bases

31
Q

A strong acid has a what conjugate base?

A

weak conjugate base

32
Q

A weak acid has a what conjugate base?

A

strong conjugate base

33
Q

A strong base has a what conjugate acid?

A

weak conjugate acid

34
Q

A weak base has a what conjugate acid?

A

strong conjugate acid

35
Q

When classifying sat solutions and both the cation and anion are acidic and basic, which prevails?

A

Whichever has the largest Ka

36
Q

Larger Ka or Kb =

A

Stronger acid or base

37
Q

Smaller Ka or Kb =

A

weaker acid or base

38
Q

Rxn + H2O ->

39
Q

Rxn -> H20

40
Q

ICE (molarity)

A

Initial Concentration
Change in Concentration
Equilibrium Concentration

41
Q

BACA (in moles)

A

Before
Addition
Change
After

42
Q

When do we ignore x, when solving for the K expression?

A

When A[Init] > Ka x 100

43
Q

How do we find the conjugate base from an acid?

A

Remove H+
Ex: HPO42-
CB = PO43-

44
Q

How do we find the acid from a conjugate base?

A

Ad H+
Ex: HSO3-
H2SO3

45
Q

What is used as a placeholder for an unknown acid?

46
Q

Is ICE used for a SA & SB?

47
Q

Is ICE used for a WA & WB?

48
Q

What is a buffer?

A

solution that resists change in pH

49
Q

What is a polyprotic acid?

A

Acid that contains more than one ionizable H+
Ex: H3PO4, H2C03

50
Q

What is a binary acid?

A

Acid that contains H and another element Y

51
Q

What are the two main things that play into the strength of binary acids?

A

Electronegativity of element Y and Bond strength

52
Q

More Electronegative =

A

Stronger Acid

53
Q

Weaker Bond =

A

Stronger Acid

54
Q

What are oxyacids?

A

Acids with oxygen and another nonmental

55
Q

More oxygens attached =

A

Stronger Acid

56
Q

More electronegative nonmetal =

A

Stronger Acid

57
Q

Lewis Acid

A

electron pair acceptor

58
Q

Lewis Base

A

electron pair donator

59
Q

Larger Ksp =

A

More soluble

60
Q

Common Ion Effect

A

Prescence of common ion decreases the solubility of a solid

61
Q

Basic anions will dissolve better in what?

62
Q

Undersaturated

A

Q < K
No ppt

63
Q

Saturated

A

Q = K
Ppt starts to form

64
Q

Supersaturated

CHEM1B (5 decks)

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