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Grade 12 chem > Unit 4 > Flashcards

Unit 4 Flashcards

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1
Q

K

A

equilibrium constant, do not include solids in equation

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2
Q

le Chateliers principle

A

When a chemical system at equilibrium is disturbed in a change in a chemical property, the system adjusts in a way that opposes the change

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3
Q

Change in [ ]

A

System will shift opposite way

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4
Q

Thermal energy

A

System will shift towards the thermal energy q

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5
Q

Decrease in volume (increase in pressure)

A

System will shift towards the side with less gas molecules

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6
Q

What will not effect le Chateliers principle

A

Adding inner gasses, catalysts

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7
Q

Q=K

A

System is at equilibrium

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8
Q

Q>K

A

System must shift left to reach equilibrium

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9
Q

Q

A

System must shift right to reach equilibrium

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10
Q

Assumptions

A

If more than two decimal places over

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11
Q

Arrhenius theory

A

Acids produce H+ ions when dissolved. Bases produce OH- when dissolved

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12
Q

Bronsted- Lowry theory

A

Acids are proton (H+) donors, bases are proton receivers

amphoteric/ amphiprotic: a substance that can act as a B-L acid or base at the same time

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13
Q

Conjugate acid pairs

A

A pair of substances who’s molecular formula differ by one H+

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14
Q

Strong acid

A

100% ionized
Monotropic- releases only one H+
Ditropic- releases only two h+
Triprotic- releases only 3 H+

HCl, HBr, HI, H2SO4, HNO3, HCLO4

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15
Q

Weak acid

A

An acid that is less than 100% ionized, in reality, much less than 50%

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16
Q

Relative strength

A

The stronger the acid is, the weaker the conjugate base is etc.

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17
Q

Kw

A

[H+][OH-]= 1.0X10^-14

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18
Q

pH+pOH

A

=14=PKw

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19
Q

pH

A

-log^[H+]

20
Q

pOH

A

-log^[OH-]

21
Q

Strong bases

A

100% ionized

Group 1 metal hydroxides + some others

22
Q

% ionization

A

(concentration of ion ionized/ concentration of solution) X100

23
Q

Measuring pH

A

litmus paper ( red= acid, base= blue)

Phenolphalein: colorless—–> 8-10

pH meter—-> based on electrical conductivity

24
Q

Haber processes

A
  • Used to make ammonia, optimal conditions are in a closed system with a catalysts and very high temperatures
25
Q

Ka X Kb

A

Kw

26
Q

Salt hydrolysis

A

Reaction of ions with water to produce acidic or basic solutions

a) if salt contains ions from strong acid and strong base the results will be neutral
b) If the salt contains the conjugate acid of a weak base, the resulting solution will be acidic
c) If the salt contains the conjugate base of a weak acid then the resulting solution will be basic
d) When a salt contains ions from a weak acid and a weak base, the values of Ka and Kb are compared to determine acidity
e) Amphoteric ions- Compare the values of Ka and Kb
f) Metal oxides with water- bases
Non metal oxides with water- acids

27
Q

Titration

A

To determine the amount of a specific chemical in a sample by adding a known amount of another substance

28
Q

Equivalence point

A

The point where the moles of acid equals the moles of base

29
Q

End point

A

The point where the indicator changes colour and the titration ends, usually just past the equivalence point

30
Q

The first law of thermodynamics (law of conservation of energy)

A

Energy can only be transformed, not created or destroyed

31
Q

Enthalpy changes and spontaneity

A

Exothermic reactions -H have a tendency to occur spontaneously

32
Q

Entropy, S

A

Degree of randomness in a system

33
Q

Predicting the signs of S

A

Gasses» solutions > liquids» solids. If the right side has more random states, S is positive.

34
Q

Second law of thermodynamics

A

When ever a spontaneous event takes place in our universe, it is accompanied by an overall increase in entropy

35
Q

Third law of thermodynamics

A

An absolute 0, the entropy of a perfectly ordered pure crystalline substance is zero

36
Q

Standard entropy (S)

A

Sum of Sf products- sum of Sf reactants

37
Q

Gibbs free energy

A

Maximum energy that is available to do work

38
Q

G

A

H-TS

Gfinal- G initial

39
Q

Dynamic equilibrium

A

Forward and reverse rates are equal

40
Q

Solubility equilibrium

A

Salt no longer appears to dissolve at the saturation point, but on microscopic scale dissolving and crystallizing are still occurring

41
Q

Phase equilibrium

A

liquid- gas

Solid- liquid

42
Q

-H, +S

A

G is non spontaneous (+)

43
Q

+H, -S

A

G is spontaneous (-)

44
Q

Spontaneous G sign

A

-

45
Q

+H, +S

A

G is only negative at high temps

46
Q

-H, -S

A

Only spontaneous at low temps

Grade 12 chem (5 decks)

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