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acid bases salts Flashcards

1
Q

acids & alkalis can dissociate to form

A

free mobile ions

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2
Q

ensuring acid is all used up to get ___________ yield

A

highest

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3
Q

bronsted-lowry theory
base def: substance that can ___________ a ________ (H+) from another substance

A

accept, proton

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3
Q

brontsted-lowry theory
acid def: is _________________ that can __________ a proton (____) to another ________________

A

substance, donate, H+, substance

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4
Q

when in same eqn/ paired with acid, water becomes _______

A

base

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5
Q

acids only behave like an acid when dissolved in ________; if in organic solvent —___ reaction

A

water, no

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5
Q

bases: ______ _________& ______ ________________

A

metal oxides, metal hydroxides

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6
Q

alkalis: ________ that are_________ in water & produces ______

A

bases, soluble, OH-

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7
Q

common acids:____,_____, CH3CO2H (____________ acid)

A

HCl, H2SO4, ethanoic

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8
Q

common alkalis: ______, _____ (aqueous ammonia)

A

NaOH, NH3

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9
Q

acids & bases can be classified as strong/weak in terms of their ________of ______________ to give ions in solution

A

extent, dissociation

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10
Q

STRONG ACID
def: one which _______________ _________ in solution to give _________ (H+)

A

dissociates fully, protons

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11
Q

STRONG ACID
degree of dissociation:

A

100%

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12
Q

STRONG ACID
type of arrow used in dissociation eqn:

A

single arrow (–>)

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13
Q

STRONG BASE
def:_____________ __________ in solution to give ____________ ions (OH-)

A

dissociates fully, hydroxide

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13
Q

strong & weak acids can be _____basic or ___basic

A

mono, di

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14
Q

STRONG BASE
degree of dissociation:

A

100%

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14
Q

WEAK ACID
def: _____________ ______________ in solution to give ________(H+)

A

dissociates partially, protons

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15
Q

WEAK ACID
degree of dissociation:

A

<100%

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15
Q

WEAK ACIDS
egs: __________ acids (containing ________) are generally weak acids

A

organic, -COOH

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16
Q

WEAK BASE
def: _______________ _____________ in solution to give ____________ ions (OH-)

A

dissociates partially, hydroxide

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16
Q

WEAK ACID
type of arrow used:

A

reversible arrow (⇌)

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17
Q

WEAK BASE
type of arrow:

A

reversible arrow (⇌)

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18
Q

WEAK BASE egs

A

ammonia (NH3)

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19
Q

strength of acid: ___________ of _________ (fully/partially) of dissociation of an acid in solution

A

measure, extent

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20
Q

conc. of acid: ______of ________ of __________________ acid per unit vol.

A

no., moles, undissociated

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21
Q

strength of acid/base is ________________ of its conc

A

INDEPENDENT

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21
Q

if a lot of H2O molecules means _____ conc of acid/base

A

low

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22
Q

HA is generic name for any ______

A

acid

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23
Q

Power of Hydrogen (pH)
def: ___________ ______ to the base ____ of the conc of hydrogen ions in ________

A

negative log, 10, mol/dm3

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24
Q

pH =

A

-log[H+]

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25
Q

[H+] =

A

10^-pH

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26
Q

[ ] means:

A

conc of thing inside [ ]

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27
Q

larger the pH value (more alkaline), _________ the [H+]

A

smaller

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28
Q

more acidic means ______ [H+]

A

more

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29
Q

at temps of 25 degree celsius,
NEUTRAL solution: [H+]___[OH-], pH__7

A

=, =

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30
Q

at temps of 25 degree celsius,
ACIDIC solution: [H+]___[OH-], pH__7

A

> , <

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31
Q

at temps of 25 degree celsius,
ALKALINE solution: [H+]___[OH-], pH__7

A

<, >

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32
Q

universal indicator: ____________ of dyes that can be used to estimate _____ of a solution by tallying ________ of solution with _______________________________

A

mixture, pH, colour, universal colour chart

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33
Q

COMMON INDICATORS USED IN TITRATION: SCREENED METHYL ORANGE
pH range for colour change: __-__
colour in acidic:
colour in alkaline:

A
  • 3, 5
  • magenta
  • green
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33
Q

COMMON INDICATORS: LITMUS
pH range at which indicator changes colour: __-__
colour in acidic solution: ____
colour in alkaline solution: ____

A
  • 5, 8
  • red
  • blue
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34
Q

COMMON INDICATORS USED IN TITRATION: METHYL ORANGE
pH range for colour change: __-___
colour in acidic: _____
colour in alkaline: _______

A
  • 3, 4.4
  • red
  • yellow
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34
Q

COMMON INDICATORS USED IN TITRATION: THYMOL BLUE
pH range for colour change: __-___
colour in acidic:
colour in alkaline:

A
  • 8, 9.6
  • yellow
  • blue
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35
Q

PROPERTIES OF ACIDS
pH:

A

less than 7

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35
Q

COMMON INDICATORS USED IN TITRATION: PHENOLPHTALEIN
pH range for colour change: __-___
colour in acidic:
colour in alkaline:

A
  • 8, 10
  • colourless
  • pink
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35
Q

PROPERTIES OF ACIDS
taste:

A

sour

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36
Q

PROPERTIES OF ACIDS
turns ______ blue _______ paper ____
turns ________________________ _________/____

A
  • damp, litmus, red
  • universal indicator, orange/red
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37
Q

PROPERTIES OF ACIDS
can ___________ ______________ (can act as charge carriers as they exist as ________________________ in _____________ solution)

A

conduct electricity, free mobile ions, acqueous

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38
Q

PROPERTIES OF ALKALIS
taste: ________ & feel ________

A

bitter, soapy

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39
Q

PROPERTIES OF ALKALIS
turn ______ red _______ paper _______
turn _____________________________ _____/________

A
  • damp, litmus, blue
  • universal indicator, blue/violet
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40
Q

PROPERTIES OF ALKALIS
pH:

A

more than 7

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41
Q

PROPERTIES OF ALKALIS
can ____________ _____________ (can act as ________ ___________ as they exist as ____________________________ in aqueous solution)

A

conduct electricity, charge carriers, free mobile ions

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42
Q

in organic solvent, acid exists as a simple molecular compound ( ________ dissociate in organic solvents) —> no ______________________________ to act as _________________ so ____ electrical conductivity

A

doesn’t, free mobile ions, charge carriers, no

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43
Q

neutralisation: reaction between acid and base to form _____ & _______

A

salt, water

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44
Q

Haber process: industrial method for ______________ of ______________ (a weak base in aqueous medium)

A

manufacture, ammonia

45
Q

Haber process is a ____________ reaction

A

reversible

46
Q

nature of OXIDE changes from _______ (metal oxides) to _____________ to ________ (non-metal oxides)

A

basic, amphoteric, acidic

47
Q

operating conditions for haber process:
- ______ pressure of ____ atm (atmospheric press. at sea level)
- _______________ temp of ____ °C
- _____ __________
- molar ratio of N2:H2 is __:__

A
  • high, 250
  • moderate, 450
  • iron catalyst
  • 1:3
48
Q

grp 13:___ (is _____________)

A

Al, amphoteric

49
Q

basic OXIDES can react with ______ to form ______ & _________

A

acids, salt, water

50
Q

amphoteric OXIDES can react with ______ ______ ___ ______ to form ______ & ________

A

both acids & bases, salt, water

51
Q

acidic OXIDES can react with _______ to form _____& ______

A

bases, salt, water

52
Q

grp 1 & 2 r ______ oxides & ______ in nature

A

metal, basic

53
Q

BASIC OXIDES: reaction with water
they’re usually __________ in water but ____________ (_____) & _______________ (_____) are _________ in water to give _________ solution with pH _7

A

insoluble, sodium oxide (Na2O), potassium oxide (K2O), soluble, alkaline, >

54
Q

BASIC OXIDES: reaction with water
Na2O + H2O —> ________
K2O + H2O —> ________

A
  • 2NaOH (sodium hydroxide)
  • 2KOH (potassium hydroxide)
55
Q

BASIC OXIDES: reaction with acids
______ basic oxides can react with acids to give _____ & _______
eg Na2O + 2HCl —> 2NaCl + H2O

A

metal, salt, water

56
Q

ACIDIC OXIDES
grp ___,___, & ____ r ____________ oxides dat are acidic in nature

A

14, 15, 16, non-metal

57
Q

ACIDIC OXIDES: reaction with water
non-metal oxides r ______ oxides
some acidic oxides _____ dissolve in _______ to form acidic solutions with pH__ 7

A
  • acidic
  • can, water, <
58
Q

ACIDIC OXIDES: reaction with water
egs: SO2 + H2O —>
SO3 + H2O —>

A
  • H2SO3 (sulfurous acid)
  • H2SO4 (sulfuric acid)
59
Q

AXIDIC OXIDES: reaction with bases
they react with bases to form ______ & _______

A

salt, water

60
Q

ACIDIC OXIDES : reaction with bases
egs:
P4O10 + 12 NaOH —>
SO2 + 2NaOH —>
SO3 + 2NaOH —>

A
  • 4Na3PO4 (sodium phosphate) + 6H2O
  • Na2SO3 (sodium sulfite)+ H2O
  • Na2SO4 (sodium sulfate)+ H2O
61
Q

ACIDIC OXIDES : reaction with bases
egs: silicon dioxide (_____), (giant ___________ struc. with _____________ strong ___________ bonds), reacts with ________________ ____/_________ NaOH at _____ temp to form ________________
SiO2 (s) + 2NaOH (l) ———> ??
molten 350 °C

A
  • SiO2, molecular, numerous, covalent, concentrated hot/molten, high, sodium silicate
  • Na2SiO3 (l) + H2O (g)
62
Q

AMPHOTERIC OXIDES: reaction with water
_____ react with water

A

DON’T

63
Q

AMPHOTERIC OXIDES: reaction with acids & bases
react to ______ (______ nature) to form ______ & _______

A

both, dual, salt, water

63
Q

AMPHOTERIC OXIDES: reaction with acids & bases
egs:

A
  • aluminium oxide
  • lead(II) oxide
  • zinc oxide
64
Q

AMPHOTERIC OXIDES: reaction with ACID
eg of reaction:

A

Al2O3 (acts as basic oxide) + 6HCl —> 2AlCl3 (aluminium chloride)+ 3H2O

65
Q

AMPHOTERIC OXIDES: reaction with BASE
eg of reaction:

A

Al2O3 (acts as acidic oxide) + 2NaOH + 3H2O —> 2NaAl(OH)4 (hydrated sodium aluminate)

65
Q

neutral oxides:
______ react with acids & bases
pH__7

A
  • don’t
  • =
66
Q

egs of neutral oxides

A
  • carbon monoxide (CO)
  • water
  • nitric oxide (NO)
  • nitrous oxide (N2O)
67
Q

salts r ______ ___________(eg NaCl)

A

ionic compounds

68
Q

salts contain _______ ________ & ___________ ________

A

metal cation & non-metal anion

68
Q

salts taht contain water of crystallisation are

A

hydrated

69
Q

naming of hydrated salts
eg: hydrated sodium carbonate (Na2Co3 · 10H2O)
LHS is _____
RHS is water of crystallisation, in this case there’s ___ moles of water of crystallisation for every mole of Na2CO3

A
  • salt
  • 10
69
Q

salts that don’t contain water of crystallisation are

A

anhydrous

69
Q

water molecules _____________ bind to ions in salt crystals —> water bonded _____________ within crystal known as ____________________________

A

chemically, chemically, water of crystallisation

70
Q

water of crystallisation can be driven off by __________ (energy to ______ chem bonds) crystals strongly to form _____________ salts
(might also have colour _________)

A

heating, break, anhydrous, change

71
Q

SOLUBILITY OF SALTS
salts with grp 1 cations: ____ soluble in water

A

ALL

71
Q

SOLUBILITY OF SALTS
ammonium salts:____ soluble in water

A

ALL

72
Q

SOLUBILITY OF SALTS
- chloride salts: ____________________, _____________________________ INSOLUBLE in water, all other r _____________
- btw their halides (grp ___) are insoluble except for _________

A
  • lead (II) chloride (PbCl2), silver chloride (AgCl), soluble
  • 17, flourides
72
Q

SOLUBILITY OF SALTS
nitrate salts: _____ soluble in water

A

ALL

73
Q

SOLUBILITY OF SALTS
sulfate salts: _____________________, _________________________, _____________________ INSOLUBLE in water, all other r ___________

A

calcium sulfate (CaSO4), lead (II) sulfate (PbSO4), barium sulfate (BaSO4), soluble

74
Q

SOLUBILITY OF SALTS
carbonate salts: _____________________, ______________________________ SOLUBLE, all others _______________

A

grp 1 carbonates, ammonium carbonate: (NH4)2CO3, insoluble

75
Q

SOLUBILITY OF SALTS
oxides & hydroxides: _____________ & ___________ __________, all others ____________

A

grp 1 oxides & hydroxides, soluble, insoluble

76
Q

ALL SOLUBLE SALTS

A
  • all grp 1 cations
  • all ammonium salts
  • all nitrate salts
  • chlorides except lead & silver chlorides
  • sulfates except Ca, Pb & Ba sulfates
  • grp 1 carbonates
  • ammonium carbonate, (NH4)2CO3
  • grp 1 oxides & hydroxides
77
Q

ALL INSOLUBLE SALTS

A
  • lead (II) & silver chloride
  • lead (II) & silver halides (except flourides)
  • calcium, lead (II) & barium sulfates
  • carbonates except grp 1 & ammonium carbonate
  • oxides & hydroxides except grp 1 oxides & hydroxides
78
Q

reactivity series
most ————————————>least reactive

A

K, Na, Ca, Mg, Al, Zn, Fe, Pb, H, Cu, Ag, Au

79
Q

reactivity series
everything above H:
everything after H:

A
  • reacts with acid
  • doesn’t react with acid
80
Q

reactivity series:
____, ____, ____ don’t react with acids
____ ain’t corrosive
____ & ____ r jewellery

A

Cu, Ag, Au
Cu,
Ag, Au

81
Q

reactivity series:
K vs Na
K has more _______ –>electrons ___________ _______ –> ___________________ forces of attraction ___________ –> electrons _________ _______ –> _______ __________

A

shells, further away, elecrostatic, weaker, easily lost, more reacive

82
Q

ACID-METAL reaction
when _________ metal (located above H in reactivity series) reacts with ________ acid, ______ & ________________ r formed

A

reactive, dilute, salt, hydrogen gas

83
Q

ACID-METAL reaction
less reactive metals _________ H in reactivity series eg _______, _________ & ______ metal ______ react with dilute acids

A

below, Cu, Ag, Au, don’t

83
Q

ACID-METAL reaction
simple formula:

A

acid + metal —> salt + hydrogen gas

84
Q

ACID-METAL reaction
extremely reactive metals eg _______ metals: __________, _____________ react ___________ & _____________ with dilute acids

A

grp 1, sodium, potassium, violently, explosively

85
Q

ACID-(HYDROGEN)CARBONATE reaction
when (hydrogen)/carbonate reacts with acid, _____, ________ & ________________ r formed

A

salt, water, carbon dioxide gas

86
Q

ACID-(HYDROGEN)CARBONATE reaction
simple formula

A

(hydrogen)/carbonate + acid —> salt + water + carbon dioxide gas

87
Q

ACID-BASE reaction (neutralisation)
simple formula

A

acid + base —> salt + water

87
Q

ACID-BASE reaction (________________)
egs of bases: ______ oxides & hydroxides, ____________
when acid reacts with base, _____ & ________ r formed

A
  • neutralisation
  • metal, ammonia
  • salt & water
88
Q

ACID-BASE reaction (neutralisation)
when ammonia (weak ______) reacts with acid, _____ ______ is formed

A

base, only salt

89
Q

ACID-AMMONIA reaction (_________________)
simple formula

A
  • neutralisation
  • acid + ammonia (NH3) —> salt ONLY
90
Q

ALKALI-AMMONIUM SALT reactions
when ammonium ______ warmed in presence of alkali, _____, _______ & ____________ _____ r formed

A

salt, salt, water, ammonia gas

91
Q

ALKALI-AMMONIUM SALT reactions
simple formula

A

ammonium salt(NH4+) + base (alkali) — (warmed)—> salt+ water + ammonia gas (NH3)

92
Q

PRECIPITATION reactions
forms ___________ salts (know from solubility table) thru _________ of 2 _________ (_____________) reagents

A

insoluble, mixing, soluble, aqueous

93
Q

PRECIPITATION reactions
when aqueous solution that contains ________ of an insoluble salt is _______ with an aqueous solution containing _______ of that salt, the _____________ salt will _______________ out of ___________

A

anion, mixed, cation, insoluble, precipitate, mixture

94
Q

PRECIPITATION reactions
to get the__________ salt: _______ _____ excess liquid into beaker, then the ___________ is the salt

A

insoluble, filter out, residue

95
Q

prep of salts
- soluble salt usually prepared from reactions with ______
- insoluble salt usually prepared by _________________________ ( _________ of 2 __________ salts)

A
  • acids
  • precipitation method, mixing, soluble
96
Q

reactions with acids: if salt to be prepared is ___________ in water while reactants ____________, salt can be prepared thru reaction of acid with excess _______/ ______ (insoluble)/ ______________ (insoluble)

A

insoluble, soluble, metal, base, carbonate

97
Q

reaction of ACID & EXCESS METAL
- metal + acid—> _____ + _____________ _____
- to produce salt that’s soluble in water, excess metal is use such that acid is _____________ used up (acid is ___________ reagent)
- ___________ _____ escapes so only soluble salt & excess metal remains & they can be separated thru ______________

A
  • salt, hydrogen gas
  • completely, limiting
  • hydrogen gas, filtration
97
Q

reaction of ACID & EXCESS METAL
(acid + metal —> salt + hydrogen gas)
this method unsuitable for:
- _____ ____________ metals eg Na & K cus they react ____________ with acids
- metals ________ ____ in reactivity series eg _______ & __________ as they don’t react with dilute acids

A
  • very reactive, violently
  • below H, copper, silver
98
Q

reaction of ACID & EXCESS METAL
experiment steps
- add ________ metal to ________ acid in beaker & _____ constantly till ____ ______ metal __________ in acid
- ______ to separate ________ metal —> salt collected as _________ & metal collected as __________
- heat _________ to evaporate water to _______________ salt solution to obtain ______________ solution of salt
- on __________, metal _________ will form
- ______ to get metal as _________ & wash it with abt __ _____ (cus salt is ___________—>can’t use too much water) of _____ distilled water to remove _____________
- dry ________ by pressing them between layers of ______ paper

A
  • excess, dilute, stir, no more, dissolves
  • filter, excess, filtrate, residue
  • filtrate, concentrate, saturated
  • cooling, crystals
  • filter, residue, 1 drop, soluble, cold, impurities
  • crystals, filter
99
Q

reaction of ACID + EXCESS INSOLUBLE BASE
reaction between base (metal ______/ ___________) and acid
acid + base (____________) —> _____ + _______

A

-oxides, hydroxides
- insoluble, salt, water

100
Q

reaction of ACID + EXCESS INSOLUBLE BASE
experiment steps
- add _______ base to acid in beaker & _____ constantly till ___ _____ base _________ in acid
- ______ to separate _______ base from ___________ solution of salt, which is collected as _________ & base collected as ___________
- _____ the _________ to _____________ water to _______________ salt solution to get _______________ solution of salt
- on __________, salt _________ forms
- ________ to obtain salt _________ as _________ & wash them with abt __ _____ (salt is _____________) of ______ distilled water to remove ______________
- dry _________ by pressing them between layers of _______ paper

A
  • excess, stir, no more, dissolves
  • filter, excess, aqueous, filtrate, residue
  • heat, filtrate, evaporate, concentrate, saturated
  • cooling, crystals
  • filter, crystals, residue, 1 drop, soluble, cold, impurities
  • crystals, filter
101
Q

reaction of ACID + EXCESS INSOLUBLE CARBONATE
carbonate (____________) + acid —> _____ + _________ + __________________

A

insoluble, salt, water, carbon dioxide gas

102
Q

reaction of ACID + EXCESS INSOLUBLE CARBONATE
experiment steps
- add ________ carbonate to acid & _____ constantly till ___ ______ carbonate __________ in acid
- ______ to separate ________ carbonate from ___________ solution of salt, which is collected as _________ & carbonate as ____________
- _____ the ________ to evaporate water to ______________ salt solution to get a ______________ solution of salt
- on _________, salt ________ forms
- ______ to obtain ________ as ____________ & wash them with abt __ _____ of ______ distilled water to remove ______________
- dry ________ by __________ them in between layers of _______ paper

A
  • excess, stir, no more, dissolves
  • filter, excess, aqueous, filtrate, residue
  • heat, filtrate, concentrate, saturated
  • cooling, crystals
  • filter, crystals, residue, 1 drop, cold, impurities
  • crystals, pressing, filter
103
Q

reaction of acid + SOLUBLE base/ carbonate
but since it’s soluble there won’t be any remaining ___________ residue to show that reaction is complete, so use ____________: determines _______ vol. of alkali that reacts with known amt of acid in presence of an _____________

A

insoluble, titration, exact, indicator

104
Q

alkalis are a

A

soluble base

105
Q

when acids react with metal, metal will be _______ –> ___________, so must be in _________

A

solid, insoluble, excess

106
Q

reaction of acid + SOLUBLE base/ carbonate
- part a: get the vol of base needed for __________________ with use of an _______________
- part b: prepare salt __________ use of an ____________ (cus it might _____________ salt —> salt not _____)

A
  • neutralisation, indicator
  • without, indicator, contaminate, pure
107
Q

reaction of acid + SOLUBLE base/ carbonate
TITRATION
- fill __________ with dilute _______ & record reading (1st reading)
- _________ ______cm3 of dilute ______ into a _____cm3 ________ _______
- add 1-2 drops of _____________ to acid & see og colour
- add dilute base from _________ (____________ near end-point), til end-point colour ________ observed
- record final _________ reading (2nd reading)
- record amt of base needed for __________ neutralisation (1st reading - 2nd reading)

A
  • burette, base
  • pipette, 25, acid, 250 conical flask
  • indicator
  • burette, drop-wise, change
  • burette
  • complete
108
Q

reaction of acid + SOLUBLE base/ carbonate
preparation of salt __________ use of indicator’
- _________ _____cm3 of dilute ______ into _____cm3 beaker
- add (_________________________)cm3 of dilute ______ (from __________) to acid
- ______ reaction mixture in beaker to evaporate off water —> get a ____________ solution
- let solution _____ ______ slowly & __________ of salt start to form (might need ice bath)
- _______ off _________ (as __________)
- wash them with ______ amt of ______ distilled water to remove ___________
- dry them between layers of ______ paper

A
  • without
  • pipette, 25, acid, 250
  • 1st reading - 2nd reading, base, burette
  • heat, saturated
  • cool down, crystals
  • filter crystals, residue
  • little, cold, impurities
  • filter
109
Q

IONIC PRECIPITATION REACTION (for insoluble salts)
have to choose 2 suitable _______ ____________ that when combined results in ______________ of wanted salt (need to ___________ any solid starting material to get __________ solution first)

A

ionic compounds, precipitate, dissolve, aqueous

110
Q

IONIC PRECIPITATION REACTION (for insoluble salts)
basically, take the salt, find ______ eqn of it, then choose 2 ______ ___________(each as 1 part of the salt) that can react with each other to give that salt & another compound but can ignore that

A

ionic, ionic compounds,

111
Q

IONIC PRECIPITATION REACTION (for insoluble salts)
experiment steps
- using ___________ ____________, add certain vol of 1 of the _______ ____________ into small beaker
- add ________ amts of the other ______ ___________ & _____ till ___ ______ ______________ forms
- ______ mixture to get insoluble salt as __________
- wash ______________ with ______ amt of ___________ water to remove any ______________
- dry it between layers of ______ paper

A
  • measuring cylinder, ionic compounds
  • excess, ionic compound, stir, no more precipitate
  • filter, residue
  • precipitate, small, de-ionised, impurities
  • filter
112
Q

IONIC PRECIPITATION REACTION (for insoluble salts)
BUT STARTING MATERIAL’S INSOLUBLE
- stage 1: convert it to a _________ ______
BY: adding ________ insoluble starting material to dilute ______ ______ (always convert to that) to form soluble salt & stir till ___ ______ insoluble starting material _____________. then _______ mixture to obtain ___________ _____ as filtrate
- stage 2: mix solutions of soluble salt (from stage 1 filtrate) & another ______ ___________ (basically the steps from b4: 2 soluble solutions)

A
  • soluble salt, excess, nitric acid, no more, dissolves, filter, soluble salt
  • ionic compound
113
Q

IONIC PRECIPITATION REACTION (for insoluble salts)
BUT STARTING MATERIAL’S INSOLUBLE

insoluble staring material can’t be added directly to other solution to make insoluble salt cus reaction would form an __________ compound that ______ surface of ____________ ____________ _____________, preventing it from __________ _________ with the other ionic compound in the other solution —> ____ ______ of insoluble salt

A

insoluble, coats, insoluble starting material, further reacting, low yield

114
Q
A

chemisty (6 decks)

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