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General Chemistry MCAT > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

arrhenius acid

A

Produces H+ ions when dissolved in water

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2
Q

arrhenius base

A

Produces OH- ions when dissolved in water

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3
Q

Bronsted-Lowry acid

A

proton donor

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4
Q

bronsted lowry base

A

proton acceptor

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5
Q

in the arrhenius definition, water is not considered an ____ bc it doesnt dissociate into H+ ions

A

Acid

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6
Q

lewis acid

A

electron pair acceptor

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7
Q

lewis base

A

electron pair donor

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8
Q

amphoteric species

A

is one that can act either as an acid or a base, depending on its chemical environment

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9
Q

amphiprotic

A

A species that can either accept or donate a proton.

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10
Q

when water reacts w a base, it behaves as a _____

A

acid

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11
Q

when water reacts w an acid, it behaves as a ____

A

base

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12
Q

complex amphoteric species

A

amino acids w zwitterion intermediates (both cationic and anionic character)

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13
Q

-ate ->

A

-ic

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14
Q

-ite ->

A

-ous

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15
Q

-ide ->

A

hydro-…-ic

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16
Q

autoionization

A

the process by which water acts as an acid and a base with itself

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17
Q

water dissociation constant

A

An expression of the auto-ionization of water into H+ and OH- at a certain temperature, given by the product of H+ and OH-‘s molar concentrations and is denoted by the equilibrium constant K_w., equal to 10^-14 at 25 degrees Celsius.

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18
Q

the concentration of each H3O+ and OH- in pure water at equilibrium at 298 K is..

A

10^-7 M

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19
Q

how can you change Kw?

A

change the temperature
NOTHING ELSE

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20
Q

at temperatures above 298 K, Kw will

A

increase

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21
Q

pH =

A

-log[H+]

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22
Q

pOH =

A

-log[OH-]

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23
Q

pH + pOH =

A

14

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24
Q

strong acids/bases

A

dissociate completely in water
- 1 M NaOH dissociates completely into 1 M Na+ and 1 M OH-

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25
Q

single headed arrows typically indicate

A

strong acids/bases

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26
Q

strong acids

A

HCl, HBr, HI, HNO3, H2SO4, HClO4

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27
Q

strong bases

A

LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

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28
Q

weak acids and bases

A

do not completely dissociate in solution and have corresponding dissociation constants (Ka and Kb)

29
Q

weak acid equation

A

HA + H2O <–> H3O+ + A-

30
Q

the smaller the Ka, the ____ the acid

A

weaker

31
Q

weak base equation

A

BOH -> B+ + OH-

32
Q

the smaller the Kb, the ____ the base

A

weaker

33
Q

conjugate acid-base pair

A

two substances that are related by the loss or gain of a single hydrogen ion

34
Q

if Ka or Kb is less than 1

A

it is a weak acid/base

35
Q

If Ka is large, then Kb is

A

small

36
Q

a strong acid produces a ___ conjugate base

A

very weak

37
Q

Ka x Kb

A

Kw

38
Q

acids that have EN elements nearer to acidic hydrogens are _____ than those that do not

A

stronger

39
Q

neutralization reaction

A

a reaction in which an acid and a base react in an aqueous solution to produce a salt and water

40
Q

Strong acid + Strong base = ______ solution

A

neutral
- salt + H2O

41
Q

Strong acid + Weak base = _________ solution

A

acidic salt

42
Q

Weak acid + Strong base = ________ solution

A

basic
- salt + H2O

43
Q

weak acid + weak base =

A

neutral salt

44
Q

neutralization reactions are often ______ reactions because they form bonds w a small molecule as a byproduct

A

condensation

45
Q

if Ka&raquo_space; water

A

strong acid
- if its closer to water, than its a weak acid

46
Q

if Kb&raquo_space; water

A

strong base

47
Q

what is the equivalent for acids

A

moles of H+

48
Q

what is the equivalent for bases

A

moles of OH-

49
Q

gram equivalent weight

A

-amount of a compound that produces 1 equivalent of the particle of interest

Gram Equivalent Weight= (molar mass)/n

n : # of particles produced or consumed per molecule

50
Q

titrant

A

A solution of known concentration that is used to titrate a solution of unknown concentration

51
Q

titrand

A

has an unknown concentration but a known volume

52
Q

equivalence point is reached when

A

number of acid equivalents in the original solution = number of base equivalents added
-or vv

53
Q

titration equation

A

VaNa=VbNb

54
Q

indicators

A
  • weak acids or bases that display different colors in their protonated and deprotonated forms
  • the indicator chosen for a titration should have a pKa close to the pH of the expected equivalence point
  • the endpoint of the titration is when the indicator reaches its final color
55
Q

equivalence point for strong acid + strong base

A

ph = 7

56
Q

equivalence point for weak acid + strong base

A

above 7 ( basic)

57
Q

difference between titration of weak acid/strong base and strong acid/strong base

A
  • initial pH of weak solution is higher
  • pH changes more gradually early on and has a less sudden rise at eq point
58
Q

equivalence point of strong acid and weak base

A

less than 7

59
Q

equivalence point of weak acid and weak base

A

Can have equivalence points above and below 7, depending on the relative strength of the acid and base.

60
Q

half-equivalence point

A

pH=pKa
[HA] = [A-]

61
Q

Polyvalent Titration Curve

A

region I = [A2-] predominates
region II = [HA-] = [A2-]
region III = [HA-] predominates
region IV = [H2A] = [HA-]
region V = [H2A] predominates

62
Q

buffer solution

A

a solution made from a weak acid and its conjugate base that neutralizes small amounts of acids or bases added to it

63
Q

acid buffer

A

Weak acid + conjugate base (salt)
acetic acid/sodium acetate
- when strong base is added, OH- ions interact w H3O+ present, so more acetic acid dissocates
- weak acid part of buffer neutralizes strong base
- when H+ is added, it makes acetic acid which is weak and doesn’t change pH that much

64
Q

base buffer

A

Weak base + conjugate acid (salt)
- ammonium chloride/ammonia solution

65
Q

bicarbonate buffer system

A

CO2 (g)+ H2O(l)↔H2 CO3 (aq)↔H+ (aq)+HCO3- (aq)

-Blowing off CO2 (hyperventilation) decreases levels of CO2 which causes reaction to shift left consuming H+ and reducing H+ in the blood making pH less acidic

66
Q

Henderson-Hasselbalch equation

A

pH = pKa + log [A-]/[HA]

67
Q

pOH =

A

pKb + log[B+]/[BOH]

68
Q

buffering capacity

A

the ability of a buffered solution to absorb protons or hydroxide ions without a significant change in pH; determined by the magnitudes of [HA] and [A-] in the solution
- maintained within 1 pH unit of the pKa value

69
Q

buffering region

A

[HA] ~ [A-]
flattest point
resistant to pH changes

General Chemistry MCAT (12 decks)

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