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CHEM/OCHEM (MCAT) > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

Arrhenius base

A

species that produces OH- in aqueous solution (hydroxide ions)

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2
Q

Arrhenius acid

A

species that produces H+ (hydrogen ions) in aqueous solution

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3
Q

An Arrhenius base can react with an Arrhenius acid in a/an ___________________ reaction.

A

neutralization

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4
Q

What is a neutralization reaction?

A

acid + base –> water + salt

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5
Q

Bronsted-Lowry acid

A

species that produces H+

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6
Q

True or False: Bronsted-Lowry bases and acids are the same as Arrhenius bases and acids.

A

FALSE: Bronsted-Lowry ACIDS are the SAME as Arrhenius ACIDS (species that produces H+)…but Bronsted-Lowry BASES are different from Arrhenius BASES.

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7
Q

Bronsted-Lowry Base

A

species that accepts H+

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8
Q

When a Bronsted-Lowry acid _______ a proton, it forms a conjugate base.

When a Bronsted-Lowry base _______ a proton, it forms a conjugate acid.

A

acid LOSES proton

base GAINS proton

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9
Q

Lewis acid

A

electron-pair acceptor

hint: lewis Acid = electron pair Acceptor

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10
Q

Lewis base

A

electron-pair donor

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11
Q

A Lewis acid is a/an:

a) electrophile
b) nucleophile

A

a) electrophile

hint: lewis Acid = electron pair Acceptor

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12
Q

A Lewis base is a/an:

a) electrophile
b) nucleophile

A

b) nucleophile

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13
Q

Which species is fundamental to understanding MCAT OCHEM?

a) Arrhenius
b) Bronsted-Lowry
c) Lewis

A

c) Lewis

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14
Q

True or False: a given species cannot have multiple classifications (Arrhenius, Bronsted Lowry, Lewis).

A

FALSE

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15
Q

List the strong acids (7).

A 
HI (hydroiodic acid)
HBr (hydrobromic acid)
HCl (hydrochloric acid)
HNO3 (nitric acid)
HClO4 (perchloric acid)
HClO3 (chloric acid)
H2SO4 (sulfuric acid)
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16
Q

List the strong bases (7).

A 
NaOH (sodium hydroxide)
KOH (potassium hydroxide)
NH2- (amide ion)
H- (hydride ion)
Ca(OH)2 (calcium hydroxide)
Na2O (sodium oxide)
CaO (calcium oxide)
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17
Q

What does the term “pH” refer to?

A

“potential of the hydrogen ion”

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18
Q

how is pH defined in terms of the proton concentration? (provide equation)

A

pH = -log[H3O+]

hint: p = -log[whatever]

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19
Q

How is pOH defined in terms of the hydroxide ion concentration? (provide equation)

A

pOH = -log[OH-]

hint: p = -log[whatever]

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20
Q

pH + pOH = ?

A

pH + pOH = pKw = 14 (at room temperature)

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21
Q

Calculate the following pH/pOH:

  • log[1M] = ?
  • log[1 x 10^-1 M] = ?
  • log[1 x 10^-2 M] = ?
  • log[1 x 10^-13 M] = ?
  • log[1 x 10^-14 M] = ?
A
  • log[1M] = 0
  • log[1 x 10^-1 M] = 1
  • log[1 x 10^-2 M] = 2
  • log[1 x 10^-13 M] = 13
  • log[1 x 10^-14 M] = 14
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22
Q

Calculate the following:

\+log(1) = ?
\+log(3.2) = ?
\+log(10) = ?
A 
\+log(1) = 0
\+log(3.2) = 0.5
\+log(10) = 1
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23
Q

What is the pH of an aqueous solution of HCl with an initial concentration of 3.2 x 10^-5 M?

A

pH = -log(3.2 10^-5 M)

-log(10^-5M) = 5
\+log(3.2) = 0.5

pH = 5 - 0.5 =4.5

NOTE: SUBTRACT log of the mantissa

24
Q

given the reaction below, what is the formula for the equilibrium constant (Kc)?

aA + bB –>/<– cC + dD

A

Kc = ( [C]^c [D]^d ) / ( [A]^a [B]^b )

25
Q

Changes in which of the following influence(s) the equilibrium constant? Select all that apply:

a) volume
b) pressure
c) temperature
d) catalyst

A

c) temperature

26
Q

TRUE OR FALSE: do NOT include pure liquids and gasses in the equilibrium constant calculation

A

TRUE

27
Q

What does amphoteric mean?

A

can act as both and acid and a base

28
Q

TRUE or FALSE: water is amphoteric

A

TRUE

29
Q

What is the equilibrium equation for the self-ionization/autoionization of water?

A

H2O (acid) + H2O (base) –>/<– HO- (conjugate base) + H3O+ (conjugate acid)

30
Q

What is the equilibrium constant for the self-ionization of water?

A

Kw = [H3O+][OH-] = 1.00 x 10^-14 ….at 25C and 1 atm

note: [H3O+] = [OH-] = 1.00 x 10^-7

31
Q

Ka x Kb = ?

A

Ka x Kb = Kw = 10^-14

32
Q

If Ka of a weak acid is greater than 10^-7 (e.g. 10^-6), its conjugate base will be __________.

a) stronger
b) weaker

hint: consider the value of Ka x Kb (or Kw)

A

b) weaker

33
Q

If Ka of a weak acid is less than 10^-7 (e.g. 10^-8), its conjugate base will be __________.

a) stronger
b) weaker

hint: consider the value of Ka x Kb (or Kw)

A

a) stronger

34
Q

What is the relationship between pKa and pKb? provide a formula/equation.

A

pKa + pKb = pKw = 14

35
Q

acid strength ___________ with an increase in Ka.

a) increases
b) decreases

A

a) increases

36
Q

acid strength ___________ with an increase in pKa.

a) increases
b) decreases

A

b) decreases

37
Q

base strength ___________ with an increase in Ka.

a) increases
b) decreases

A

b) decreases

38
Q

base strength ___________ with an increase in pKa.

a) increases
b) decreases

A

a) increases

39
Q

provide the products:

strong acid + strong base –>

A

water + neutral ions

40
Q

provide the products:

strong acid + weak base –>

A

water + acidic cation + neutral anion

41
Q

provide the products:

weak acid + strong base

A

water + neutral cation + basic anion

42
Q

provide the products:

weak acid + weak base

A

water + acidic cation + basic anion

43
Q

As atomic radius increases, acid strength and stability of conjugate base ____________.

a) increase
b) decrease

A

a) increase

44
Q

TRUE or FALSE: Acid strength increases to the right and down the periodic table (opposite of Zeff).

A

FALSE: SAME as Zeff

45
Q

Resonance ______________ conjugate bases.

a) stabilizes
b) destabilizes

A

a) stabilizes

46
Q

TRUE or FALSE: electronegativity increases with acid strength.

A

TRUE

47
Q

TRUE or FALSE: an increase in induction (EWG) causes a decrease in acidity.

A

FALSE: acidity increases with induction

48
Q

TRUE or FALSE: pKa increases as distance between the acidic proton and the electronegative atom increases.

A

TRUE

49
Q

What is a zwitterion?

A

ion that can be protonated or deprotonated

50
Q

For polyprotic acids, acid dissociation _____________ with sequential deprotonation.

a) increases
b) decreases

A

b) decreases

51
Q

At the equivalence/stoichiometric point (pH 7), number of moles of acid are _______________ number of moles of base.

a) greater than
b) less than
c) equal to

A

c) equal to

52
Q

What is the name of the chemical used to visualize the equivalence point?

A

indicator

53
Q

TRUE or FALSE: An indicator is usually a strong acid or strong base; whose conjugate form is a different colour.

A

FALSE: an indicator is usually a WEAK acid or base

54
Q

When does the indicator change colour?

A

at the end point

55
Q

TRUE or FALSE: A correct indicator will change colour at a pH that is far from the equivalence point, so that you can distinguish the end point from the equivalence point.

A

FALSE: A correct indicator will change colour at a pH that is very CLOSE tot he equivalence point.

56
Q

ADD QUESTION ABOUT TITRATION CURVES

A

CHEM/OCHEM (MCAT) (10 decks)

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