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Chemistry > Chem 162 (Chapters 15 + 16) > Flashcards

Chem 162 (Chapters 15 + 16) Flashcards

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1
Q

What is the equation for the equilibrium constant Keq of this chemical equation.

N2(g)+O2(g)⇔2NO(g)

A

K = [NO]2/[N2][O2]

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2
Q

What does it mean to be in dynamic equilibrium?

A

The rates of the forward and reverse reactions are the same.

The concentrations (or any other values) are not necessarily equal.

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3
Q

When the equilibrium constant K is 2.1·10-20, what can be said about this reaction?

a) At equilibrium the concentrations of products and reactants are the same.
b) At equilibrium the concentration of products is much greater than that of reactants.
c) At equilibrium the concentration of reactants is much greater than that of products.
d) There are no reactants left over.

A

c) [reactants] >> [products] at equilibrium

because K is so small

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4
Q

In the equilibrium constant equation for heterogeneous equilibria what is omitted?

A

Concentrations of pure solids and liquids.

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5
Q

Given:

2HgO(s)+H2O(l)+2CO2(g)⇔2HOCl(aq)+HgO·HgCl2(s)

What is the equilibrium constant expression for this heterogeneous reaction?

A

K = [HOCl]2/[CO2]2

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6
Q

Given [OH-], what is the pOH?

A

-log[OH-]

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7
Q

Given pH, how would you find [H+]

A

10-pH

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8
Q

Given pOH, how would you find pH?

A

14-pOH=pH

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9
Q

What is H2SO4?

A

Sulfiric Acid

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10
Q

What is HNO3?

A

Nitric Acid

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11
Q

What is HC2H3O2?

A

Acetic Acid

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12
Q

What is the Arrhenius definition of acids and bases?

A

Acid: Produces H+ (H3O+)

Base: Produces OH-

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13
Q

What is the Bronsted-Lowry definition of acids and bases?

A

Acid: Proton donor.

Base: Proton acceptor.

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14
Q

What is the definition of a strong acid?

A

100% ionization.

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15
Q

What is the difference between a strong acid and a weak acid?

A

Strong acids completely dissociate in water whereas weak acids only partially dissociate.

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16
Q

What are the six important strong acids?

A

HCl (Hydrochloric Acid)

HBr (Hydrobromic Acid)

HI (Hydriodic Acid)

HNO3 (Nitric Acid)

HClO4 (Perchloric Acid)

H2SO4 (Sulfuric Acid)

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17
Q

What is a diprotic acid?

A

An acid containing two ionizable atoms.

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18
Q

Of the six important strong acids, which is diprotic?

A

H2SO4 (Sulfuric Acid)

-because of the two hydrogens

19
Q

Name at least 3 of the main weak acids.

A

1) HF (Hydrofluoric Acid)
2) HC2H3O2(Acetic Acid)
3) HCHO2 (Formic Acid)
4) H2SO3 (Sulfurous Acid)
5) H2CO3(Carbonic Acid)
6) H3PO4(Phosphoric Acid)

20
Q

Given:

HA(aq) ⇔ H+(aq) + A-(aq)

What is the Ka of this reaction?

A

Ka={[H+][A-]}/[HA]

21
Q

Is water an acid or a base?

A

It can act as either one.

22
Q

What is Kw and what is its value at 25oC?

A

Kwis the ion product constant for water.

At 25oC, Kw=1.0x10-14

23
Q

How do you calculate percent ionizaton?

24
Q

What is a strong base?

A

A base that completely dissociates in water.

25
Q

Name at least 3 of the main strong bases.

A
  1. LiOH (Lithium Hydroxide)
  2. NaOH (Sodium Hydroxide)
  3. KOH (Potassium Hydroxide)
  4. Sr(OH)2 (Strontium Hydroxide)
  5. Ca(OH)2 (Calcium Hydroxide)
  6. Ba(OH)2 (Barium Hydroxide)
26
Q

Given:

B(aq)+H2O(l)⇔BH+(aq)+OH-(aq)

What is Kb?

A

Kb=[BH+][OH-]/[B]

27
Q

If an anion is the conjugate base of a weak acid then it is…

A

…a weak base itself.

28
Q

If an anion is a conjugate base of a strong acid it is…

A

…pH neutral.

29
Q

What is Kw’s relationship to Ka and Kb?

A

Kw=KaKb

30
Q

A cation that is the conjugate acid of a weak base…

A

…is a weak acid.

31
Q

Salts in which the cation does not act like an acid and the anion acts like a base form…

A

…basic solutions.

32
Q

Salts in which the cation acts as an acid and the anion does not act like a base form…

A

…acidic solutions.

33
Q

How do polyprotic acids dissociate?

A

In several successive steps.

Each has its own Ka.

34
Q

What equation relates pH to pKa?

A
35
Q

What does a buffer do?

A

Resists pH change by neutralizing added acids or bases.

36
Q

When an acid is added to a buffer, a stoichiometric amount of the [ ] is converted to the [ ].

A
37
Q

When a base is added to a buffer, a stoichiometric amount of the [ ] is converted to the [ ].

A
38
Q

pKa+pKb=?

(numerical value)

A

14

39
Q

What is the relation between [H3O+], [OH-] and Kw?

A

Kw=[H3O+] [OH-]

40
Q

When can some ions behave like acids or bases?

A

In an aqueous solution.

41
Q

What is required for a buffer solution?

A

A weak acid and its conjugate base or a weak base and its conjugate acid.

42
Q
A
43
Q

What are Lewis acids and bases?

A

Lewis acid: electron pair acceptor

Lewis base: electron pair donor

Chemistry (9 decks)

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