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General Chemistry > Acids/Bases > Flashcards

Acids/Bases Flashcards

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1
Q

bicarbonate

A

base HCO3-

when added to something that is acidic, will increase pH to become more basic because HCO3- consumes H+

H+ + HCO3- H2CO3 H2O + CO2

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2
Q

ksp

A

solubility product constant

the products are multiplied together. If that concentration exceeds the ksp, they will also form a precipitate because ksp represents the limit of solubility. Everything under ksp value will be dissolved, everything over becomes solid

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3
Q

How does the stability of the conjugate base affect acidity?

A

conjugate bases made from smaller halogens will be less stables because a smaller radius has less surface area to spread out the charge (thus stabilize)

therefore while fluorine is the most electronegative, it will form a short, strong bond with H that is not acidic (wants to keep H)

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4
Q

What determines acidity of functional group?

A

more electronegative atoms are more acidic

ability to stabilize negative charge through charge distribution (atom size) or delocalization (resonance)

more acidic protons will be the first to deprotonate as pH increases

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5
Q

What is more acidic alkene, alkane, or ketone?

A

ketones are less acidic than alcohols, but more acidic than hydrocarbons. The negative charge in the conjugate base of a ketone is delocalized by resonance across the alpha carbon and carbonyl oxygen atoms, which helps stabilize the charge

alkene proteins (sp2 C-H) are more acidic than alkane proteins (sp3 C-H)

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6
Q

What is more acidic, primary or secondary alcohol?

A

a primary alcohol is more acidic which contributes to their enhanced ability to react because deprotonation by a base makes the alcohol a better nucleophile

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7
Q

nucleophile

A

Needs a New Boy

  • super negative and has a lot of baggage (electrons)
  • looking for positive charge to balance her out
  • she is a lewis base because will provide electrons to the positive electrophile
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8
Q

electrophile

A

Electron loving
positive - wants to accept electrons
Lewis acid

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9
Q

How do acids affect nucleophiles?

A

nucleophiles are out looking for protons to make her happy because she is so negative.
acids come along and donate their H+ to nucleophile which is a bronsted base (accepts protons)

because already has a proton, will not actively search for more, reducing the nucleophilicity of the molecule

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10
Q

indicators

A

determine endpoint by changing color during titration to signal close to equivalence point (when the acid and base are equal amounts)

one color represents low pH and another color represents high pH

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11
Q

buffers

A

region that will not have a large change in pH
weak acid + conjugate base or weak base + conjugate acid (or salt)

need weak acid or base so it doesn’t completely dissociate. acids donate protons and bases accept them so work together to resist changes in pH

buffering zones are horizontal on a titration curve - point of inflection

buffering zone = 1/2 [weak acid/base]

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12
Q

NH3

A

ammonium

weak base

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13
Q

strong acids

A 
HClO4
HI
HBr
H2SO4
HCl
HNO3
H3O+ or H+
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14
Q

perchloric acid

A

HClO4

strong acid

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15
Q

hydrochloric acid

A

HCl

strong acid

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16
Q

sulfuric acid

A

H2SO4

strong acid

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17
Q

nitric acid

A

HNO3

strong acid

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18
Q

acidic in nature

A

the more oxidated something is, the more acidic

ex: CO2 is surrounded by oxygen and is like breaking pure acid

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19
Q

strong bases

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

strong bases completely dissociate in solutions because the conjugate acid cation is very stable

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20
Q

weak acids

A 
HCOOH (formic acid)
CH3COOH (acetic acid)
HF (hydrofluoric acid)
HCN (cyanide)
H2S (hydrogen sulfide)
H2O (water)
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21
Q

weak bases

A 
NH3 (ammonium)
NR3 (amine)
C5H5N (pyridine)
NH4OH (ammonium hydroxide)
H2O (water)
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22
Q

neutralization

A

acid + base –> salt + water

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23
Q

equivalence point

A

vertical line where [base]=[acid] - neutralized

amount of equivalence points is dependent on number of acidic protons (H+) - polyprotic acids have multiple pKas

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24
Q

strong base + strong acid

A

equivalence point is pH 7

25
Q

strong base + weak acid

A

equivalence point at higher pH than 7

26
Q

strong acid + weak base

A

equivalence point lower than pH 7

27
Q

titration

A

technique to determine the concentration of an unknown solution

use a known concentration and slowly add to unknown solution with known volume and use indicator to see change

28
Q

polyprotic acids

A

have more than one acidic proton
the number of acidic protons will be the number of equivalence points

adding strong base will neutralize and remove protons in stepwise fashion

29
Q

How to tell acidic protons

A

acidic protons are attached to functional groups with low pKa values

acidic --> basic
H-X
R-H-O-H+
R-NH3+
carboxylic acid
phenol
alcohol
SP
amine
SP2
SP3

look for protons on electronegative atoms first –> O, N, S

30
Q

the most stable conjugate base will be

A

the strongest acid

31
Q

oxyacid

A

acid that contains a hydrogen, oxygen, and another element

HClO

dissolves in water and creates acidic solution
ex: HClO + H2O –> H30+ + ClO-

32
Q

oxides

A

oxygen and another element

ex: SO2

33
Q

arrhenius acid

A

H+ donor

HA –> H+ + A-

34
Q

arrhenius base

A

OH- donor

BOH –> B+ + OH-

35
Q

Bronsted-Lowry acid

A

H+ donor

36
Q

Bronsted-Lowry base

A

H+ acceptor

37
Q

Lewis acid

A

electron acceptor aka electrophile

38
Q

Lewis base

A

electron donor aka nucleophile

39
Q

water as an acid or base

A

water is amphoteric - can act as either acid or base

will act a certain way depending on conditions
in basic conditions acts a s a base

40
Q

ionization

A

complete loss of electrons
left with just an ion

M –> M+ + e-

41
Q

NO2-

A

nitrite

42
Q

NO3-

A

nitrate

43
Q

NO4-

A

peroxynitrate

44
Q

NO

A

nitroxide

45
Q

SO3^(2-)

A

sulfite

46
Q

SO4^(2-)

A

sulfate

47
Q

PO4(3-)

A

phosphate

48
Q

PO3(3-)

A

phosphite

49
Q

ClO3-

A

chlorate

50
Q

ClO2-

A

chlorite

51
Q

HCO3-

A

bicarbonate

bi = single Hydrogen atom

52
Q

HSO4-

A

bisulfate

53
Q

H2PO4-

A

dihydrogen phosphate

di = two hydrogen atoms

54
Q

ferrous

A

Fe2+

ous = lower charge for metal

55
Q

ferric

A

Fe3+

ic = higher charge for metal

56
Q

neutralization

A

acid + base –> salt + H20

can figure out how much is needed by using NacidVacid=NbaseVbase
N= normalities = number of grams/volume
V=volume

so this can be thought of as moles acid = moles base

57
Q

What makes a strong Lewis acid?

A

smaller ionic radius and strong positive charge

58
Q

Why is the conjugate base a better nucleophile than the acid?

A

because the conjugate base has more electron density due to the negative charge

General Chemistry (10 decks)

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