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Chem 105 > Unit 2: Chemical Equilibrium > Flashcards

Unit 2: Chemical Equilibrium Flashcards

1
Q

Equilibrium constant

A

K, it is unitless.

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2
Q

Rate constant

A

k

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3
Q

In equilibrium are the concentrations of products and reactants the same?

A

No, the concentrations of products and reactants are just constant.

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4
Q

What can effect the equilibrium constant?

A

Change in temperature

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5
Q

What is heterogeneous equilibria

A

Reactions with species that are different phases.

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6
Q

What does not appear in an equilibrium constant equation?

A

Pure solids, liquids, and solvents

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7
Q

Large K?

A

> 10^3

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8
Q

Intermediate K?

A

10^-3 to 10^2

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9
Q

Small K?

A

<10^-4

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10
Q

What happens with a large K?

A

The reaction proceeds to completion and at eq there will be a large amount of product and a small amount of reactant.

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11
Q

What happens with a small K?

A

The reaction does not completely proceed and at eq there will be a small amount of product and a large amount of reactant.

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12
Q

Reaction Quotient

A

Q

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13
Q

If Q < K what happens?

A

The reaction will go towards the products and the Q will get larger.

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14
Q

If Q > K what happens?

A

The reaction will go towards the reactants and the Q will get smaller.

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15
Q

What happens if you increase the concentration of a substance?

A

The reactions shifts away from that substance.

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16
Q

What happens if you decrease the concentration of a substance?

A

The reaction shifts towards that substance.

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17
Q

What happens if you increase the pressure of the system?

A

The reaction shifts towards the side with fewer moles.

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18
Q

What happens if you decrease the pressure of the system?

A

The reaction shifts towards the side with more moles.

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19
Q

What happens if you increase the temperature of the system?

A

The reaction shifts away from the heat/energy.

20
Q

What happens if you decrease the temperature of the system?

A

The reaction shifts towards the heat/energy

21
Q

What happens if you add a catalyst to the system?

A

Nothing

22
Q

What are the steps for solving an intermediate K problem?

A
  1. Calculate Q to determine the direction of the reaction.
  2. Make ICE table.
  3. Substitute into K and solve for x.
23
Q

When solving a large K reaction should you let it go forward to completion?

A

Yes, this way it becomes a limiting reagent type problem.

24
Q

What are the 6 strong acids?

A

HCl, HBr, HI, HNO3, HClO4, H2SO4

25
Q

What is a polyprotic acid?

A

Acids that have several protons which can be donated.

26
Q

What is the leveling effect?

A

The inability to tell the difference between the strength of strong acids in solvents like water or with a higher pH.

27
Q

What is a buffer?

A

A solution that contains a considerable amount of a weak acid and its conjugate base.
They resist changes in pH when an acid or base is added to a solution.

28
Q

How can a buffer be prepared?

A

Partial neutralization: The addition of a strong acid or base to one component of the buffer.

29
Q

What is an equation for pKa?

A

-log[Ka]

30
Q

What is buffer capacity?

A

The measure of the buffer’s ability to maintain pH.

31
Q

What is buffer range?

A

The pH range where the buffer is effective.

32
Q

What is Solubility?

A

The amount of solid that must be dissolved to produce a solution

33
Q

What is precipitation?

A

When and how much solid will precipitate out of a solution.

34
Q

What is the solubility product?

A

Ksp.

35
Q

What is a saturated solution?

A

A solution with the maximum concentration of dissolved ions, with the solution in contact with extra undissolved solid.

36
Q

When Q > Ksp?

A

The reaction proceeds towards reactants and precipitation is formed.

37
Q

When Q < Ksp?

A

The reaction proceeds towards products and no precipitation is formed.

38
Q

What is the common-ion effect?

A

It is the effect on an equilibrium involving a substance that ads an ion that is a part of the equilibrium.

39
Q

When Q = Ksp?

A

The solution is saturated.

40
Q

What are the 4 rules of solubility?

A
  1. Nitrate salts
  2. Alkali metals and ammonium salts
  3. Cl, Br, and I salts except with: Ag, Pb, and Hg2
  4. Sulfate salts except with: Sr, Ba, Pb, Hg2
41
Q

What are the 4 rules of insolubility?

A
  1. Hydroxide salts
  2. Sulfide salts
  3. Carbonate salts
  4. Phosphate salts
    all except with: group 1 and NH4 salts
42
Q

Will basic salts be more soluble in acidic solutions?

A

Yes

43
Q

What is a complex ion?

A

A central metal ion with several groups attached.

44
Q

What is Kf?

A

The formation constant

45
Q

How does adding H3O+ affect the solubility of anion of a weak acid?

A

It increases it solubility.

Chem 105 (5 decks)

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