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chemistry > Acids, Bases and Salts > Flashcards

Acids, Bases and Salts Flashcards

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1
Q

Indicators

A

Substances which indicate whether compound is acidic or basic by change in colour

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2
Q

Natural Indicators

A

red cabbage extract, turmeric, hydrangea, litmus

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3
Q

Artificial Indicators

A

Mehtyl Orange, Phenopthalein

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4
Q

TURMERIC

A

yellow in color, remains yellow in acidic soln, turns red in basic soln

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5
Q

HYDRANGEA

A

blue in color, remains blue in acidic soln, turn pink in basic soln

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6
Q

METHYL ORANGE

A

red color in acidic soln, yellow color in basic soln

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7
Q

PHENOPTHALIEN

A

colorless, remains colorless in acidic soln, turns pink in basic soln

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8
Q

RED CABBAGE EXTRACT

A

red in color, remains red in acidic soln, turns green in basic soln

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9
Q

LITMUS

A

base- turns red litmus blue

acid- turns blue litmus red

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10
Q

OLFACTORY INDICATORS

A

indicate whether substance is acidic or basic in nature by changing odor or smell

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11
Q

VANILLA EXTRACT

A

characteristic smell remains as it is in acidic soln but cannot be detected in basic soln

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12
Q

Onion

A

characteristic smell remains as it is in acidic soln but cannot be detected in basic soln

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13
Q

EXAMPLES of OLFACTORY INDICATORS

A

vanilla extract, onion

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14
Q

ACIDS

A

sour in taste, conduct electricity

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15
Q

ORGANIC ACIDS

A

naturally occuring, weak in nature

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16
Q

EXAMPLES OF ORGANIC ACIDS (6)

A

Lactic Acid, Tartaric Acid, Oxalic Acid, Methanoic/formic, Acetic Acid, Citric Acid

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17
Q

LACTIC ACID

A

SOUR MILK/CURD

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18
Q

TARTARIC ACID

A

TAMARIND, UNRIPE GRAPES

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19
Q

OXALIC ACID

A

TOMATOES

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20
Q

methanoic acid is also known as

A

formic acid

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21
Q

Methanoic Acid

A

Ant’s sting, nettle leave sting

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22
Q

Citric Acid

A

citrus fruits like lemon, lime

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23
Q

Acetic Acid

A

Vinegar

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24
Q

MINERAL ACIDS

A

prepared from minerals of earth, man made, generally strong in nature

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25
Q

which mineral acid is not strong in nature

A

Carbonic acid (H2CO3)

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26
Q

three most used mineral acids

A

Sulphuric, Hydrochloric and Nitric

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27
Q

Acetic acid (in form of vinegar) is used in?

A

pickles, ketchup

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28
Q

Tartaric Acid is used in making

A

baking powder

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29
Q

carbonic acid is used in making

A

fizzy drinks

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30
Q

why should water be added gradually while diluting acid?

A

diluting acid is highly exothermic process–> lot of heat is produced
if water is added at once, large amount of heat would be evolved which would convert some of the water to steam, this might lead to acid splashing and causing burns

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31
Q

when acids react with metal

A

hydrogen gas is formed along with salt

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32
Q

example of metal reacting with acid

A

zinc + sulphuric acid —> zinc sulphate + hydrogen

Zn+H2SO4 —> ZnSO4+H2

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33
Q

why should food not be stored in metal containers?

A

because acid in food will react with metal to form harmful metal compounds

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34
Q

acid react with metal carbonate/hydrogen carbonate

A

to form salt, CO2, H2O

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35
Q

example of metal carbonate reacting with acid

A

sodium carbonate + hydrochloric acid—> sodium chloride + carbon dioxide+ water
Na2CO3 + 2HCl —> 2NaCl+ CO2+ H2O

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36
Q

metal carbonate/hydrogen carbonate + HCl (hydrochloric)

A

metal chloride+ CO2 + H2O

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37
Q

metal carbonate/hydrogen carbonate +H2SO4 (sulphuric)

A

metal sulphate + CO2 + H2O

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38
Q

example of metal hydrogen carbonate reacting with acid

A

sodium hydrogen carbonate + hydrochloric acid –> sodium chloride+ carbon dioxide + water
NaHCO3+HCl—> NaCl+CO2+H2O

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39
Q

lime water and carbon dioxide

A

Ca(OH)2 + CO2 —> CaCO3 + H2O

calcium hydroxide + carbon dioxide + calcium carbonate + water

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40
Q

lime water is

A

calcium hydroxide, Ca(OH)2

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41
Q

quicklime is

A

CaO, calcium oxide

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42
Q

slaked lime

A

Ca(OH)2

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43
Q

what can be observed when CO2 passes through lime water

A

lime water turns milky due to formation of white precipitate (CaCO3)

44
Q

what can be observed when excess CO2 passes through

A

when excess CO2 is passed, white precipitate (CaCO3) dissolves due to formation of calcium hydrogen carbonate and solution becomes clear
CaCO3+CO2+H20—> Ca(HCO3)2

45
Q

different forms of calcium carbonate (CaCO3)

A

egg shells, chalk, limestone, marble

46
Q

Acid react with base

A

to form salt and water, neutralization reaction

47
Q

example of acid reacting with base

A

NaOH (aq) +HCl (aq) —> NaCl (aq) +H2O (l)

]sodium hydroxide + hydrochloric acid –> sodium chloride + water

48
Q

acid react with metal oxide/hydroxide

A

to form salt and water

49
Q

example of acid reacting with metal oxide

A

CuO (s) + 2HCl (aq)—-> CuCl2 (aq) +H2O (l)

50
Q

what can be observed when copper oxide reacts with hydrochloric acid

A

change in color from black to blue-green

this reaction shows basic nature of metal oxide

51
Q

Acids and H+ ions

A

acids disassociate in water to produce H+ ions

52
Q

are all compounds having hydrogen acidic?

A

no because some compounds (like glucose) contain hydrogen but do not disassociate in water to form H+ ions

53
Q

why do aqueous acids conduct electricity

A

aqueous acids conduct electricity because of charged particles (ions) present in them

54
Q

why does rain water conduct electricity but distilled water doesn’t?

A

rain water dissolves with CO2 which is an acidic gas while falling through atmosphere to form carbonic acid (H2CO3). Due to presence of acid, electricity is conducted by rain water. Rain water also dissolves with other acidic gases like SO2, NO2 etc to form acid

55
Q

do acids show acidic behavior in absence of water?

A

no, because in absence of water acids cannot disassociate into H+ ions

56
Q

Strong acids

A

completely ionize in water to produce large amount of H+ ions
they react rapidly and are strong electrolytes due to large amount of ions

57
Q

what happens to H+ ions in water

A

H+ ions attach to polar water molecules to form hydronium ions
H+ ions + H2O—> H3O+ ions

58
Q

Weak Acids

A

partially ionize in water and produce small amount of H+ ions, react slowly and low electrical conductivity

59
Q

Example of strong acid

A

H2SO4 (sulphuric), HNO3 (Nitric)

60
Q

Example of weak acid

A

CH3COOH

61
Q

⇌ what does this double arrow indicate in a chem eqn

A

indicates partial ionization

62
Q

USES of sulphuric acid (9)

A

manufacture of fertilizers ( ammonia sulphate ), paints, dyes, chemicals, plastics, synthetic fibres, detergents, explosives, car batteries

63
Q

uses of nitric acid (4)

A

fertilizers (like ammonium nitrate), explosives ( TriNitro Toluene), dyes and plastic

64
Q

Uses of hydrochloric acid (5)

A

removing oxide film from steel objects

removing ‘scale’ from inside boilers, used in textile, food and leather industry

65
Q

ALKALI

A

water soluble bases

66
Q

examples of alkali

A

KOH, NH4OH, NaOH, Ca(OH)2, Mg(OH)2

67
Q

why are alkali more useful than bases

A

most chemical reactions take place in water, this is why alkali are more useful

68
Q

Bases and OH- ions

A

bases disassociate in water to form OH- ions

69
Q

Strong Bases

A

completely ionise in water and produce large amount og OH- ions

70
Q

Weak Bases

A

partially ionize in water and produce small amount of OH- ions

71
Q

Examples of strong bases

A

NaOH, KOH

72
Q

Examples of weak bases

A

NH4OH, Ca(OH)2, Mg(OH)2

73
Q

bases react with metal

A

for H2 gas

base + metal —> salt + H2

74
Q

example of metal reacting with base

A

sodium hydroxide + zinc —> sodium zincate + hydrogen

2NaOH (aq) + Zn(s) –> Na2ZnO2(aq) +H2 (g)

75
Q

base react with acid

A

to form salt and water

76
Q

example of base reacting with acid

A

2NaOH+ H2SO4 —> Na2SO4 + 2H2O

sodium hydroxide + sulphuric acid —> sodium sulphate + water

77
Q

Neutralization reaction in terms of ions

A

H+ (aq) + OH- (aq) —-> H20 (l)

H+ ion from acid and OH- ion from base

78
Q

Base react with non metal oxide

A

to form salt and water

79
Q

example of base + non metal oxide

A

Ca(OH)2+ CO2 —-> CaCO3 +H2O

80
Q

non metal oxides are ________ in nature

A

acidic

81
Q

use of sodium hydroxide

A

soap, paper, rayon (synthetic fibre)

82
Q

use of slaked lime

A

bleaching powder

83
Q

use of magnesium hydroxide

A

antacid

84
Q

use of sodium carbonate

A

washing soda, softening hard water

85
Q

use of sodium hydrogen carbonate

A

baking soda, making baking powder, antacid, soda-acid fire extinguisher

86
Q

when and who devised pH scale

A

1909, Sorenson

87
Q

what is pH scale

A

it is a scale that represents strength of acid and bases through concentration of H+ ions present
pH scale is inversely proportionate to concentration of H+ ions

88
Q

what is pH level of neutral substances

A

pH level of neutral substances is exactly 7

89
Q

pH level of acid?

A

acidic soln have pH less than 7
strong acid have pH 0 to 3
weak acid have pH 4 to 6

90
Q

pH level of bases?

A

more than 7
weak base have pH 8 to 10
strong base have pH 11 to 14

91
Q

Universal Indicator

A

mixture of many different indicators give different colors at different pH value, They indicate strength of acidic/basic solution

92
Q

what are different colors at different concentration of H+ ion in universal indicator

A 
strong acid---> red tones
weak acid ---> orange tones
neutral --> green
weak base --> blue tones
strong base ---> violet tones
93
Q

ACIDITY and its remedy

A

when excess of HCl is produced, it leads to indigestion

REMEDY - antacid, an antacid can neutralize excess acid and give relief

94
Q

Antacid and their examples

A

mild bases that dont have any toxic effect on body
examples- Mg(OH)2 - milk of magnesia/ magnesium hydroxide
NaHCO3 - sodium hydrogencarbonate

95
Q

Tooth Decay

A

bacteria in mouth break down sugar to form acid, when pH of acid falls below 5.6 it becomes strong enough to corrode enamel of teeth

96
Q

how to prevent tooth decay

A

toothpastes are basic in nature (generally have pH of 8) and they neutralize excess acid, we should clean our teeth with toothpaste regularly
eat less sugary food

97
Q

Plant growth and soil pH

A

plant grow best when pH of soil is around 7

98
Q

how can we treat soil that is too acidic

A

CaO (quicklime), Ca(OH)2 (lime water), CaCO3 (chalk) can be used to treat acidic soil as they are basic in nature and can neutralize excess acid

99
Q

how can we treat soil that is too basic

A

decaying organic matter (manure/compost)

100
Q

how does pH level affect aquatic animals

A

when rain water has pH of 5.6, it is considered acidic . Too much acid rain can lower pH level of lakes/rivers. Aquatic animals can only survive within narrow range of pH change, this is why, when lakes become too acidic, aquatic animals die

101
Q

how to prevent death of aquatic animals (caused by high acidity of lake)?

A

CaCO3 (calcium carbonate) can be added to lakes to raise their pH levels and neutralize excess acid

102
Q

why cant Venus support life

A

its atmosphere has thick white and yellow clouds of sulphuric acid, body can only work well in pH range around 7, this is why venus is inhabitable

103
Q

what is there in a bee’s sting? remedy for sting?

A

bees inject acidic liquid to protect themselves

remedy- mild base like baking soda

104
Q

what is there in a wasp’s sting? remedy for sting?

A

wasp inject alkaline liquid, remedy - mild acid like vinegar

105
Q

what is there in a ant’s sting? remedy for sting?

A

ants inject methanoic acid, remedy - mild base like baking soda

106
Q

what is there in a nettle leave’s sting? remedy for sting?

A

nettle leaves have stinging hair that inject methanoic acid into skin of animal that touches them
TRADITIONAL REMEDY - using leaves of dock plant (which grow near nettle plant). dock plant leaves have basic chemicals that neutralize the acid
other remedy - mild base like baking soda

chemistry (4 decks)

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