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MCAT Chemistry > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

Arrhenius acid

A

anything that produces hydrogen ions in aqueous solution

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2
Q

Arrhenius base

A

anything that produces hydroxide ions in aqueous solution

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3
Q

Bronsted and Lowry

A

acids - anything that donates a proton

bases - anything that accepts a proton

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4
Q

Lewis acids and bases

A

acids - anything that accepts a pair of electrons
bases - anything that donates a pair of electrons
*most general definition

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5
Q

pH =

A

pH = -log[H+]

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6
Q

log(1) =

A

0

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7
Q

log(10) =

A

1

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8
Q

log(AB) =

A

log(A) + log(B)

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9
Q

hydronium ion

A

H3O+

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10
Q

conjugate acid and base

A

the products that correspond to acid and base
HA is conjugate acid of base A-
A- is conjugate base of acid HA
*stronger the acid, weaker the conjugate base
stronger the base, weaker the conjugate acid
weak acid - strong or weak conjugate

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11
Q

amphoteric

A

act as acid or base,depending on their environment

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12
Q

strong acids

A 
hydroionic acid - HI
hydrobromic acid - HBr
hydrochloric acid -HCl
nitric acid - HNO3
perchloric acid - HClO4
chloric acid - HCLO3
sulfuric acid - H2SO4
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13
Q

strong bases

A 
sodium hydroxide - NaOH
potassium hydroxide - KOH
amide ion - NH2-
hydride ion - H-
calcium hydroxide - Ca(OH)2
sodium oxide - Na2O
calcium oxide - CaO
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14
Q

polyprotic acids

A

can donate more than 1 proton

diprotic- can donate 2 electrons

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15
Q

3 factors that deterime if molecule will release its hydrogen into solution and act as an acid

A

strength of bond holding hydrogen
polarity of bond
stability of conjugate base

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16
Q

with oxyacids, more oxygens means ….

A

stronger acid

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17
Q

hydrides

A

binary compounds containing hydrogen

basic, acid, or neutral

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18
Q

metal hydrides are…

A

basic or neutral

19
Q

nonmetal hydrides are…

A

acidic or neutral

increasing acidity to the right and down the table

20
Q

autoionization of water

A

H2O + H2O –> H3O+ + OH-

K(_w) is equilibrium constant

21
Q

K(_w)

A

equilibrium constant for autoionization of water
= [H+][OH-]
= 10^-14 at 25C

22
Q

pH + pOH =

A

pK(_w) = 14

23
Q

acid dissociation constant, K(_a)

base dissociation constant, K(_b)

A

acid/base’s equilibrium constant in water

K(_a)K(_b) = K(_w)q

24
Q

pK(_a) + pK(_b) =

A

pK(_w) = 14

25
Q

K_a and pK_a for strong acid

A

K_a great than 1

pK_a less than zero

26
Q

salts

A

ionic compounds that dissociate in water

27
Q

titration

A

drop by drop mixing of an acid and base

to find the concentration of an unknown by comparing it with the titrant (added drop by drop)

28
Q

titration curve

A

sigmoidal curve

29
Q

equivalence point/stoichiometric point of titration curve

A

midpoint of vertical part of titration curve, equal equivalents of acid and base in solution

30
Q

for equally strong acid-base titrations, equivalence point will be at pH _

A

pH 7

31
Q

titration curve of weak acid with strong base

A

2 flat parts, equivalence point not as predictable

32
Q

half equivalence point

A

point where exactly half of the acid has become base, concentration of acid is equal to concentration of its conjugate base
at midpoint of section of graph that is most like horizontal line
can add largest amount of base or acid with least change in pH
where solution is most buffered
pH of solution = pK_a of acid

33
Q

buffered

A

can add largest amount of base or acid with least change in pH

34
Q

Henderson-Hasselbalch equation

A

pH = pK_a + log([A-]/[HA])

pH of solution = pK_a of acid at half equivalence point (log1 = 0)

35
Q

to make buffer solution, start with acid whose pK_a is

A

closest to pH at which want the buffer solution

mix equal amount of acid with its conjugate base

36
Q

buffer solution is made from…

A

equal and copious amounts of weak acid and its conjugate base

37
Q

adding a small amount of water to and ideally dilute buffered solution will…

A

have no effect on the pH

38
Q

indicator used to find the ___

A

equivalence point

39
Q

indicator is usually…

A

weak acid whose conjugate base is a different color

40
Q

indicator range

A

pH values of the two points of color change

can be predicted from Henderson-hasselbalch

41
Q

point where indicator changes color is the ___

A

endpoint

42
Q

which indicator to use?

A

one with pK_a as close as possible to pH of the titrations equivalence point

43
Q

polyprotic titration

A

more than one equivalence point

first proton completely dissociates before 2nd begins to dissociate

MCAT Chemistry (7 decks)

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