FINAL

Question 1

K =

Answer 1

[Products]/[Reactants

Question 2

What is not included in the K expression?

Answer 2

Solids and Liquids

Question 3

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

Answer 3

(1/k)^n

Question 4

Q is the what?

Answer 4

Reaction Quotient

Question 5

What is Q, before equilibrium?

Answer 5

Q<K

Question 6

What is Q, at equilibrium?

Answer 6

Q=K

Question 7

What is Q, after equilibrium?

Answer 7

Q>K

Question 8

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

Answer 8

Le Chatliers Principle

Question 9

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

Answer 9

Effect of Volume, Effect of Temperature, Concentration Effect

Question 10

Effect of Volume

Answer 10

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

Question 11

Effect of Temperature

Answer 11

Depends on whether the reaction is endothermic or exothermic.

Question 12

Concentration Effect

Answer 12

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

Question 13

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

Answer 13

No change or effect

Question 14

What makes a substance amphoteric and what are some examples?

Answer 14

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

Question 15

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

Answer 15

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

Question 16

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

Answer 16

Neutral

Question 17

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

Answer 17

Basic

Question 18

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

Answer 18

Acidic

Question 19

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

Answer 19

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

Question 20

What is the equation for pH and pOH?

Answer 20

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

Question 21

pH + pOH =

Answer 21

14

Question 22

pKa =

Answer 22

-log (Ka)

Question 23

Kw =

Answer 23

Ka x Kb

Question 24

What is the value of Kw?

Answer 24

1.0 x 10^-14

Question 25

10^-pH = 10^-pOH =

Answer 25

[H3O+] [OH-]

Question 26

What is an Arrhenius acid and base?

Answer 26

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

Question 27

What is a Bronstead acid and base?

Answer 27

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

Question 28

What is the relationship between NH3 and NH4+?

Answer 28

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

Question 29

What is the Henderson Hasselback equation?

Answer 29

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

Question 30

What is Ka and Kb?

Answer 30

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

Question 31

A strong acid has a what conjugate base?

Answer 31

weak conjugate base

Question 32

A weak acid has a what conjugate base?

Answer 32

strong conjugate base

Question 33

A strong base has a what conjugate acid?

Answer 33

weak conjugate acid

Question 34

A weak base has a what conjugate acid?

Answer 34

strong conjugate acid

Question 35

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

Answer 35

Whichever has the largest Ka

Question 36

Larger Ka or Kb =

Answer 36

Stronger acid or base

Question 37

Smaller Ka or Kb =

Answer 37

weaker acid or base

Question 38

Rxn + H2O ->

Answer 38

Use ICE

Question 39

Rxn -> H20

Answer 39

Use BACA

Question 40

ICE (molarity)

Answer 40

Initial Concentration Change in Concentration Equilibrium Concentration

Question 41

BACA (in moles)

Answer 41

Before Addition Change After

Question 42

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

Answer 42

When A[Init] > Ka x 100

Question 43

How do we find the conjugate base from an acid?

Answer 43

Remove H+ Ex: HPO42- CB = PO43-

Question 44

How do we find the acid from a conjugate base?

Answer 44

Ad H+ Ex: HSO3- H2SO3

Question 45

What is used as a placeholder for an unknown acid?

Answer 45

HA

Question 46

Is ICE used for a SA & SB?

Answer 46

NO ICE

Question 47

Is ICE used for a WA & WB?

Answer 47

ICE

Question 48

What is a buffer?

Answer 48

solution that resists change in pH

Question 49

What is a polyprotic acid?

Answer 49

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

Question 50

What is a binary acid?

Answer 50

Acid that contains H and another element Y

Question 51

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

Answer 51

Electronegativity of element Y and Bond strength

Question 52

More Electronegative =

Answer 52

Stronger Acid

Question 53

Weaker Bond =

Answer 53

Stronger Acid

Question 54

What are oxyacids?

Answer 54

Acids with oxygen and another nonmental

Question 55

More oxygens attached =

Answer 55

Stronger Acid

Question 56

More electronegative nonmetal =

Answer 56

Stronger Acid

Question 57

Lewis Acid

Answer 57

electron pair acceptor

Question 58

Lewis Base

Answer 58

electron pair donator

Question 59

Larger Ksp =

Answer 59

More soluble

Question 60

Common Ion Effect

Answer 60

Prescence of common ion decreases the solubility of a solid

Question 61

Basic anions will dissolve better in what?

Answer 61

Acid

Question 62

Undersaturated

Answer 62

Q < K No ppt

Question 63

Saturated

Answer 63

Q = K Ppt starts to form

Question 64

Supersaturated

Answer 64

Q > K Ppt