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Bioscience > Ch 9 Acid Base Buffers > Flashcards

Ch 9 Acid Base Buffers Flashcards

1
Q

What is an Acid?

A

Substance that yields H+ when dissolved in Water. Simplified: A proton, H+, donor.

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2
Q

An acid that donates one proton is termed?

A

Monoprotic

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3
Q

An acid that donates two protons is termed?

A

Diprotic

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4
Q

An acid that donoates three protons is termed?

A

Triprotic

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5
Q

How do strong acids behave in water?

A

Fully dissociate, one-directional rxn, into hydronium ion (H3O+) and conjugate base (reactant minus a H+)

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6
Q

How do weak acids behave in water?

A

Do NOT fully dissociate - create an equilibrium rxn.

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7
Q

What is the relationship between pH and [H+] concentration?

A

inverse relationship. As pH goes up, [H+] goes down.
As pH goes down, [H+] goes up.

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8
Q

The larger the [H+] the more ____ the solution

A

Acidic

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9
Q

What is a Base?

A

A base is a proton, H+, Acceptor.

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10
Q

Concentration of Base is measured by?

A

[OH-]

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11
Q

As [OH-] goes up, what is happening to the solution?

A

More alkaline aka Basic Bitch

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12
Q

what is the relationship between,
pOH and [OH-]

A

Inversely proportion. As [OH-] increases, pOH decreases.

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13
Q

What is the relationship between pH and pOH

A

Low pH = High pOH
High pH = Low pOH

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14
Q

13 on the pOH scale means the solution is basic or acidic?

A

ACIDIC

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15
Q

2 on the pOH scale means the solution is basic or acidic?

A

BASIC

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16
Q

As [OH-] goes up, what happens to pOH, pH, and [H+]?

A

pOH: goes down, a smaller number which means more basic

pH: goes up, bugger number, which means more basic

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17
Q

pH + pOH always equals?

A

14

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18
Q

An acid, once losing/donating its proton, becomes what on the product side?

A

Conjugate Base (of the acid)

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19
Q

A base, once gaining/accepting a proton, becomes what on the product side?

A

Conjugate Acid (of the base)

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20
Q

what is the pH equation?

A

pH = -log^[H+]

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21
Q

What is the pH of a solution with a [H+] concentration of 1x10^-7?

A
  1. Just take the absolute value of the exponent!
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22
Q

What is the difference in [H+] of a pH of 6 compared to 8?

A

pH of 6 has 100x more H+

Each 1 change in pH is equal to 10x the change in [H+]

23
Q

Which is more acidic:
[H+] = 1x10^-5
[H+] = 1 x 10^-7

A

1x10^-5 because the exponent is 5, this is equal to the pH. 5 is less than 7, meaning it is more acidic on the pH scale.

24
Q

What is an amphoteric substance?

A

It can act as an acid or base, depending on the situation. Water is the primary example/

25
Q

Stronger or weaker have a higher Ka

A

Stronger Acids

26
Q

What is Kw?

A

Equilibrium constant for water. 1 x 10^-14

27
Q

Which rxn would give you relatively more product? A strong acid or weak acid?

A

Strong because it will not reverse back into the reactant

28
Q

Which has a larger Ka, strong or weak acids? Why?

A

Strong Acids have larger Ka.

Because Ka= [product] / [reactant] , strong acids fully dissociate, there will be more product.

29
Q

equation for pKa

A

pKa = -logKa

30
Q

What are 5 strong acids

A

H2SO4, HI, HBr, HCL, HNO3

31
Q

What does Ka represent?

A

The strength of the acid, meaning how likely/much the acid wants to donate/loss its proton(s).

32
Q

When reviewing two weak acids, how do you determine which one is stronger?

A

Look at Ka. Stronger weak acid will have the large Ka.

33
Q

For polyprotic acids, which proton is donated more quickly/strongly?

A

The first proton donated. Review triprotic phosphoric acid.

34
Q

Regarding relationships between an acid and its conjugate base. The stronger the acid, the _______ its conjugate base.

A

Weaker

35
Q

Regarding relationships between a base and its conjugate acid. The stronger the base, the _______ its conjugate acid.

A

weaker

36
Q

What is the relationship between Ka and Pka?

A

Inverse. Higher Ka , lower pKa
(same as base, Kb and pKb)

37
Q

pKa +pKb =

A

14

38
Q

if given a concentration, M, of a strong acid what is your concentration of the conjugate acid?

A

Same concentration of reactant strong acid

39
Q

if given a concentration, M, of a strong base what is your concentration of the conjugate base?

A

Same concentration of reactant strong base

40
Q

If your Ka or Kb value is high, (greater than 10^3) what direction will your reaction favor?

A

Product conc > reactant conc. So, a forward reaction is favored. Equilibrium lies to the right.

41
Q

If your Ka or Kb value is low (less than 10^-3), what direction will your reaction favor?

A

Reactant conc > product conc. So, a reverse reaction is favored. equilibrium lies to the left

42
Q

If your K value is about 1, what direction will your reaction favor?

A

Neither direction is favored. The reaction proceeds halfway. Conc of reactants ~ Conc of products

43
Q

What are some strong bases?

A

LiOH, KOH, NaOH, Ba(OH)2

44
Q

Why isn’t Mg(OH)2 a strong base?

A

its insoluble

45
Q

The stronger the acid, the ______ its conjugate base.

A

Weaker. The conjugate base is “weak” if it is less likely to accept the proton it donated. Such is the case for a strong acid-conjugate base pair.

46
Q

The stronger the base, the _____ its conjugate acid.

A

Weaker. The OH- is less likely to donate the hydrogen it accepted.

47
Q

Does the conjugate base of a weak acid have base strength or not?

A

Does. It is capable of accepting the proton it initially donated, reversing the reaction.

48
Q

The reaction equilibirum always favors the formation of a?

A

weaker acid

49
Q

A change in 1 unit pH is equal to a ___ fold change in H+

A

10x

50
Q

pKw = ?

A

14
-log(Kw)

51
Q

pKa + pKb = ?

A

14

52
Q

IMPORTANT CONCEPT
What is pKa relative to pH?

A

pKa is the pH at which 50% of the compound in solution is ionized and 50% of the compound is unionized.
AKA: half acid, half conjugate base

53
Q

Why is NaCl neutral pH when dissolved in water?

A

Fully dissociates but does not react with water. Because water is neutral pH, and NaCl does not react, the pH of solution remains neutral.

54
Q

An Alpha plot demonstrates the ratio of?

A

The % ratio of ACID to Conjugate Base.

Bioscience (17 decks)

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