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OAT- General Chemistry > Day 5: Equilibrium and Acid/Base > Flashcards

Day 5: Equilibrium and Acid/Base Flashcards

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1
Q

Equilibrium

A

-forward rate = reverse rate

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2
Q

Equilibrium

A

-forward rate = reverse rate

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3
Q

Dynamic rxn

A

No net change in concentration

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4
Q

K»1

A

Products favored at eq.

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5
Q

K

A

Reactants favored at eq.

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6
Q

K ~1

A

Considerable Prod/Rec present at eq.

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7
Q

Keq

A

No solids/ liquids. Kp for gases

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8
Q

Reaction Quotient

A

can be calculated @ any point in time

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9
Q

K changes when

A

Temperature changes

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10
Q

Q

A

Shift right

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11
Q

Q>K

A

Shift left

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12
Q

Q=K

A

at equilibrium

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13
Q

If a reaction is doubled or ect. the K changes

A

exponentially

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14
Q

K for the reverse reaction is inverse of

A

the forward reaction

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15
Q

Increase in temperature causes a shift to the

A

left

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16
Q

Increase in pressure causes a decrease in _____ and an increase in ____ and a shift ________

A

volume, molarity, left

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17
Q

Le Chatelier’s Principle

A

Systems placed under stress will respond to counter stress. System takes it out of the equilibrium.

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18
Q

Solids & liquids do not affect the eq. but are affected by

A

shifts

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19
Q

Add reactants

A

Shift right

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20
Q

Remove products

A

Shift right

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21
Q

Add a solid

A

no stress. no shift

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22
Q

Add inert gas

A

No shift

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23
Q

Solubility

A

Ksp

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24
Q

Common Ion effect

A

Ionic solids disassociating into separate ion in water. Reactants are always solids

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25
Q

Adding ion shifts

A

reduces solubility of your solid

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26
Q

Mass action ratios

A

equilibrium constant ratios

27
Q

Arrhenius –> Acid

A

H+ donor in H2O

28
Q

Bronsted-Lowry–>Acid

A

H+ donor

29
Q

Lewis- Acid

A

Electron acceptor

30
Q

Arhenious- Base

A

OH- donor in H2O

31
Q

Bronsted-Lowry- Base

A

H+ Acceptor

32
Q

Lewis- Base

A

Electron donor

33
Q

Conjugate acid/Base pairs are

A

Amphoteric (molecule or ion that can react both as an acid as well as a base) substances

34
Q

Strong Acids

A

HClO4, H2SO4, HI, HBr, HCl, HNO3 HClO3

35
Q

Strong Bases

A

Group 1 metal hydroxides, Ba(OH)2, Sr(OH)2, Ca(OH)2

36
Q

Binary Acid Trend

A

Acid composed of 2 elements, one being H you can have more than one H

37
Q

Oxoacid Trends

A
  1. More oxygens, more acidic HClO3 (more acidic) than HClO2

2. More Electronegative hetero atom (two different), more acidic. i.e. HClO3 is more acidic than HBrO3

38
Q

[H+] –> pH

A

pH = -log[H+]

39
Q

pH –> pOH

A

pH + pOH = 14

40
Q

pOH–> [OH-]

A

[OH-] = 10^-pOH

41
Q

[OH-] –> [H+]

A

[H+][OH-] =1 * 10^-14

42
Q

Acid dissociation in water

A

[H+] = √(Ka)[HA]

43
Q

Base dissociation in water

A

[OH-]= √(Kb)[A-]

44
Q

Higher Ka

A

Lower pKa, stronger acid

45
Q

Higher Kb

A

Lower pKb, strong base

46
Q

Exothermic reactions are

A

reversed

47
Q

Endothermic reactions

A

forward

48
Q

pKa + pKb

A

14

49
Q

Water diss. into ions in

A

Water

50
Q

Temp affects

A

Kw

51
Q

Stong acid + Strong base

A

Tend to release heat

52
Q

Hydrolysis of salts (ionic compounds)

A

Reacts with water

53
Q

Lewis acid

A

the more (+) the cation, the more acidic the acid

54
Q

Base salts are more soluble

A

when you add acid & vice versa

55
Q

Neutral Cations

A

Li+ Na+, K+, Rb+. Cs+, Ca 2+, Sr 2+, Ba 2+,

All other cations are acidic; the more positively charged, the more acidic

56
Q

Neutral Anions

A

Cl-, Br-, I-, NO3-. ClO4-, ClO3-

Almost all other anions are bases

57
Q

Acidic Anions

A

HSO4-

58
Q

Buffer

A

Weak acid + conjugate base

59
Q

pKa =

A

-logKa

60
Q

Titration

A

naMaVa = nbMbVb

61
Q

Strong Acid/ Strong base pH @ eq. pt.

A

7

62
Q

Weak acid/ strong base pH @ eq. pt.

A

> 7

63
Q

Strong Acid/ Weak base pH @ eq. pt.

A

OAT- General Chemistry (7 decks)

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