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chemistry 1102 > chapter 13: Acids and Bases > Flashcards

chapter 13: Acids and Bases Flashcards

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1
Q

what are some descriptions of an acid

A
  • sour taste

- ability to dissolve metals

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2
Q

what are some descriptions of a base

A
  • bitter taste

- slippery to the touch

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3
Q

what are some common acids?

A
  • HCL (hydrochloric acid)
  • H2SO4(sulfuric acid)
  • HNO3(nitric acid)
  • HC2H3O2 ( acetic acid)
  • H3C6H5O7(citric acid)
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4
Q

what are some common bases?

A 
NaOH (sodium hydroxide)
KOH ( potassium hydroxide)
Sodium Bicarbonate( NaHCO3)
Sodium Carbonate(Na2CO3)
Ammonia (NH3)
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5
Q

who developed the Arrhenius theory?

A

swedish chemist svante arrhenius

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6
Q

what was the Arrhenius theory?

A

acids are substances that increase the concentration of H+ when added to water
- bases increase concentration of OH- when dissolved in water

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7
Q

what is the neutralization reaction in the Arrhenius Acid-Base reaction

A

solution of acid and solution of base are mixed

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8
Q

what does the neutralization of an acid and metal hydroxide produce

A

H2O + OH (hydroxide and water)

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9
Q

what is an example of a neutralization reaction?

A

HCL(aq) + NaOH = H2O + NaCl

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10
Q

who developed the bronsted lowry theory?

A

danish chemist: bronsted

English chemist lowry

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11
Q

what was the Bronsted Lowry theory?

A

-acids are proton donors (Removeable H+)
-bases are proton acceptors
pair of nonbonding electrons

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12
Q

which acid-base theory do we use/ rely on

A

bronsted and lowry

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13
Q

what is an amphoteric substance

A

can act as either an acid or a base

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14
Q

what is a common example of a amphoteric substance

A

hydronium

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15
Q

what is the hydronium ion

A

H+ ions are so reactive that they can’t be in water

- small positive charged particles interacts with the nonbonding electron

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16
Q

what is an H+ ion

A

proton with no valence electron

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17
Q

what are some interchangeable terms

A

H+ and H3O+

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18
Q

which acid-base theory allows for reversible reactions

A

bronsted and lowry

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19
Q

how do bronsted and lowry reversible reactions work

A
  • original base has an extra H+ after the reaction

- original acid has a lone pair (acts as base in reverse process)

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20
Q

what does conjugate mean

A

come together

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21
Q

what is a conjugate base

A

formed by removing a proton from acid

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22
Q

what is a conjugate acid

A

formed by adding a proton

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23
Q

what are some common strong bases

A
  • sulfuric acid (H2SO4)
  • hydrochloric acid (HCL)
  • hydrobromic acid( HBr)
  • Perchloric acid ( HCLO4)
  • chloric acid (HCLO3)
  • Nitric acid(HNO3)
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24
Q

what is monoprotic

A

acids with only one ionizable hydrogen

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25
Q

what is a polyprotuc acid

A

molecules with more than 1 ionizable hydrogen

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26
Q

what is the relationship between a strong polyprotic and the conjugate base

A

one polyprotic is strong and its amphoteric conjugate base is weak acid

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27
Q

organic acids contain what backbone

A

carbon that contains the carboxyl group

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28
Q

are organic acids weak or strong and why

A

weak because most of the H atoms are not ionizable

C-H

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29
Q

what is K used for in ionization

A

express the extent to which a weak acid ionizes

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30
Q

what is not included in the acid constant

A

liquids or solid

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31
Q

what does a greater K value indicate

A

the stronger acid

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32
Q

what factors can affect acid strength

A
  • polarity and strength of the H-Y bond
  • stability of the H-Y conjugate base
  • bond strength
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33
Q

when will H transfer in a bond

A

if the H-Y bond is polarized

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34
Q

how does bond strength affect acid strength

A

strong bonds = easily dissociated (short bond length)

weak acids and bases = long bond length

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35
Q

how does the conjugate base affect acid strength

A

strong acid = more stable conj base (more stable = more strong)
stronger acid = weaker conj base

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36
Q

what is the strength of binary acids

A

more polar H-Y or weaker the bond = the more acidic compound

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37
Q

what is the trend for acidity

A

increases from left to right across a row and from top to bottom down a group

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38
Q

what is an oxyacid

A

OH groups and oxygen atoms are bound to a central atom

39
Q

in an oxyacid group what happens when Y is a nonmetal

A

Y-O-H

  • the bond to O is covalent = does not readily lose OH-
  • electronegativity of Y increases = acidity of the substance
40
Q

what is the rule of thumb for oxyacids that have the same number of O atoms and OH groups

A

acid strength increases with increasing EN of the central atom

41
Q

oxyacids that have the same central atom

A

acid strength increases as the number of oxygen atoms attached to the central atom increases

42
Q

what is the most important chemical property of water

A

it can act as either a bronsted lowry acid or base (ionization)

43
Q

what is Kw

A

the ion product constant

44
Q

at 25 degrees celsius what does Kw =

A

1.0 x 10-14

45
Q

as [H3O]+ increases what happens to [OH]

A

OH has to decrease

46
Q

what happens to H3O and OH in a neutral solution

A

they are equal to each toher

[H3O] =OH = 1.x10-7

47
Q

acidic solutions have a larger H3O or OH

A

H3O

48
Q

Basic solutions have a larger H3O or OH

A

OH

49
Q

what is pH

A

acidity and bascity of a solutoin

50
Q

how do do you calculate pH

A

-log (H3O)

51
Q

how do you calculate H3O from pH

A

10^-pH

52
Q

what is the pH of a neutral solution

A

7.00

53
Q

lower pH means what

A

acidic solution

54
Q

higher pH means that

A

more basic solution

55
Q

what is the normal pH range

A

0-14

56
Q

what is the rule of sig figs when calculating pH

A

number of decimal places in the log equals the # of sig figs in the O.G number

57
Q

how do you find poH given oH

A

-log(OH)

58
Q

how do you find POH from [oH]

A

10^-POH

59
Q

what does POH + pH =

A

14

60
Q

in an aqueous solution of a strong acid what is the source of H+ ions

A

the strong acid

61
Q

what is H3O interchangable with

A

an acid

62
Q

calculating the Ka for weak acids

A

when given the problem the weak acid is always mixed with water to produce another H3O + another aqueous solution that has one less H (use ice table)

63
Q

how to calculate % ionization

A

[H3O]+eq/[Ha]initial x 100 = 10^-ph/[Ha}

64
Q

why do we use percent ionization

A

since a weak acid ionizes partially we use it just to know how much has ionized

65
Q

why do we sometimes exclude x from the ice table

A

because the ka is small

66
Q

what happens when the concentration of an acid increases

A

strength increases and so does the pH

67
Q

as the concentration of an acid increases, the percent ionization of the acid increases why

A

an acid is diluted by adding water to it which shifts the equilibrium to the left

68
Q

what must the acid do to reach equilibrium

A

ionize more and shift to the right

69
Q

most weak bases contain what

A

nitrogen because the lone pair on N makes it an excellent proton acceptor

70
Q

what happens when a weak base interacts with water

A

produces a conjugate acid and OH ion

71
Q

what is Kb

A

the base-dissociation constant

72
Q

Kb can be used to find what directly

A

OH

73
Q

greater value of Kb =

A

stronger the base

74
Q

what is a polyprotic acid

A

acid and molecules with more than one ionizable H

75
Q

polyprotic acids do what

A

ionize in steps

76
Q

what does removing the first H automatically do to the second H

A

makes it harder to remove that is why the Ka value goes down

77
Q

what do the Ka values for successive losses of protons differ by a factor of

A

10^3

78
Q

what happens with ionization if the equlibrium lies to the righ

A

complete ionization

79
Q

what does Kw equal

A

[H3O] + [OH] so Ka X Kb = 1.0x-14

80
Q

pKa +pKb = p Kw = what

A

14.00

81
Q

if you have a stronger acid what happens to the value of pKa

A

Larger Ka = smaller pKa because it is the -log

82
Q

what is an oxide

A

molecule that contains the HOX group where X can be any element

83
Q

If X is a nonmetal, in HOX

A

compound is a covalent oxide and when it is dissolved in water an acidic solution forms

84
Q

what is an acidic oxide

A

when dissolved in water, an acidic solution forms

85
Q

what happens if X is a metal

A

compound is an ionic oxide

86
Q

who came up with the lewis theory

A

G.N lewis

87
Q

what does the lewis theory say about acids

A

acids are electron pair acceptors and they must have an atom with an empty valence orbital

88
Q

what does the lewis theory say about bases

A

bases are electron pair donors they must have lone pair electrons

89
Q

anything that can be a bronsted lowry base

A

is a lewis base but not all lewis base are B-L bases

90
Q

what is the arrhenius acid

A

substance produces H+ in water

91
Q

what is the arrhenius base

A

substance produces OH in water

92
Q

what is the bronsted lowry acid

A

proton donar

93
Q

what is the bronsted base

A

proton accpetor

chemistry 1102 (6 decks)

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