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3-2 Subjects > TA3 Questions for Chemistry > Flashcards

TA3 Questions for Chemistry Flashcards

1
Q

Definition of an Acid

A

An acid is a substance that dissociates/ionises in water to form hydrogen ions

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2
Q

Definition of Basicity of an Acid

A

The basicity of an acid is the number of hydrogen ions, which can be produced by one molecule of the acid upon dissociation.

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3
Q

Acid reacts with a metal gives

A

salt and hydrogen

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4
Q

Acid reacts with metal carbonate gives

A

salt, water and carbon dioxide

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5
Q

Acid reacts with a base gives

A

salt and water

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6
Q

Why can only an acid react with other things when dissociated in only water instead of organic solvents?

A

Acids do not ionise in organic solvents because there are no hydrogen ions present.

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7
Q

Definition of Base

A

A base is any metal oxide or metal hydroxide that reacts with acids to produce salt and water only.

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8
Q

Definition of Alkali

A

An alkali is a soluble base that produces hydroxide ions in water.

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9
Q

Physical properties of alkalis

5 Properties

A
  1. Alkalis have bitter and soapy feel
  2. Alkalis have a pH greater than 7
  3. Alkalis turn damp red litmus paper blue
  4. Alkalis turn universal indicator blue
  5. Alkalis are good conductors of electricity because of mobile ions
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10
Q

Alkali reacts with acid gives

A

salt and water

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11
Q

Alkali reacts with Ammonium salt gives

A

ammonia, water and salt

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12
Q

Definition of strength of acid

A

The strength of an acid or alkali refers to the extent it ionises to produce H⁺ or OH⁻ when dissolved in water.

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13
Q

Definition of a strong acid

A

A strong acid is one that ionises completely in water to produce a high concentration of H⁺ ions.

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14
Q

Definition of a weak acid

A

A weak acid is one that ionises partially in water to produce a low concentration of H⁺ ions.

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15
Q

Definition of a strong alkali

A

A strong alkali is one that competely ionises in water to produce a high concentration of OH⁻ ions.

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16
Q

Definition of weak alkali

A

A weak alkali is one that partially ionises in water to produce a low concentration of OH⁻ ions.

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17
Q

For carbonates, what are soluble?

A

Group 1 cations and ammonium carbonates

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18
Q

For chlorides, what are soluble?

A

All besides Silver chloride, AgCl,
Lead(II) chloride, PbCl2

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19
Q

For hydroxides / oxide, what are soluble?

A

Group 1 oxide/hydroxide
Barium oxide/hydroxide
Calcium oxide/hydroxide

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20
Q

For nitrates, what are soluble?

A

All are soluble

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21
Q

For sulfates, what are soluble?

A

All except Barium sulfate, BaSO4
Calcium sulfate, CaSO4, (sparingly soluble)
Lead(II) sulfate, PbSO4

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22
Q

For carbonates, what are insoluble?

A

All besides Group 1 cations and ammonium salts.

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23
Q

For Chlorides, what are insoluble?

A

Silver chloride, AgCl,
Lead(II) chloride, PbCl2

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24
Q

For hydroxides / oxides, what are insoluble?

A

All besides group 1 cations, ammonium salts, calcium and magnesium (sparingly soluble)

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25
Q

For nitrates, what are insoluble?

A

None

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26
Q

For sulfates, what are insoluble?

A

Barium sulfate, BaSO4
Calcium sulfate, CaSO4,
Lead(II) sulfate, PbSO4

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27
Q

Reacting dilute acid with excess
solid base/carbonate/metal is reacting with which type of salts?

A

For all soluble salts beside Group 1 salts and ammonium salts

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28
Q

For titration, what type of salts is required?

A

For all group 1 salts and ammonium salts

29
Q

For precipitation test, what type of salts is required?

A

All insoluble salts only

30
Q

Why is excess solid added to reacting dilute acid with excess metal test?

A

To ensure that all the acid is completely reacted to produce a soluble salt.

31
Q

Why don’t we use excess acid to reacting dilute acid with excess metal test?

A

Both acid and the salt formed are in the aqueous state and impossible to separate

32
Q

Test for carbon dioxide.

A

Bubbling carbon dioxide into limewater (Calcium Hydroxide) to produce a white ppt.

33
Q

Test for ammonia gas.

A

Turns damp red litmus paper blue.

34
Q

Test for hydrogen gas.

A

Extinguishes a lighted splint with a “pop” sound.

35
Q

Test for oxygen gas.

A

Relights glowing splint.

36
Q

Test for sulfur dioxide.

A

Turns aqueous acidified potassium manganate(VII) from purple to colourless.

37
Q

Test for chlorine gas.

A

Turns damp blue litmus
paper red, and then
bleaches it.

38
Q

Test for Cation Aluminium (Al³⁺) in NaOH and NH3

A

NAOH : White precipitate of aluminium hydroxide
formed*, soluble in excess to form a
colourless solution

NH3 : White precipitate of aluminium hydroxide
formed*, insoluble in excess

39
Q

Test for Cation Zinc (Zn²⁺) in NaOH and NH3

A

NaOH : White precipitate of zinc hydroxide
formed*, soluble in excess to form a
colourless solution

NH3 : White precipitate of zinc hydroxide formed*, soluble in excess to form a colourless
solution

40
Q

Test for Cation Copper (II) (Cu²⁺) in NaOH and NH3

A

NaOH : Blue precipitate of copper(II) hydroxide formed*, insoluble in excess

NH3 : Blue precipitate of copper(II) hydroxide formed*, soluble in excess to form a dark
blue solution

41
Q

Test for Cation Calcium (Ca²⁺) in NaOH and NH3

A

NaOH : White precipitate of calcium hydroxide formed*, insoluble in excess

NH3 : No precipitate formed. (No visible change)

42
Q

Test for Cation Iron (II) (Fe²⁺) in NaOH and NH3

A

NaOH + NH3 : Green precipitate of iron(II) hydroxide formed*, insoluble in excess

43
Q

Test for Cation Iron (III) (Fe³⁺) in NaOH and NH3

A

NaOH + NH3 : Red-brown precipitate of iron(III) hydroxide formed*, insoluble in excess

44
Q

Test for Cation Ammonium (NH4⁺) in NaOH and NH3

A

NaOH : No precipitate formed.
On warming, a colourless and pungent
gas evolved turns damp red litmus paper
blue.*
Ammonia Gas is produced

45
Q

Test for Anion Carbonate,CO₃²⁻

A

Add any dilute acid.
(Acid + metal carbonate -> salt + water + carbon dioxide gas)

Effervescence of a
colourless and odourless
gas, gas forms white
precipitate with limewater.

46
Q

Test for Anion Sulfate, SO₄²⁻

A

Add dilute nitric acid, followed by aqueous barium nitrate (or barium chloride).
White precipitate formed.

47
Q

Test for Anion Chloride, Cl⁻

A

Add dilute nitric acid,
followed by aqueous
silver nitrate.

White precipitate formed.

48
Q

Test for Anion Iodide, I⁻

A

Add dilute nitric acid,
followed by aqueous
silver nitrate.

Yellow precipitate formed.

49
Q

Test for Nitrate, NO₃⁻

A

Add aqueous sodium
hydroxide. Add a small
piece of aluminium foil
and warm the mixture.

Effervescence of a
colourless and pungent
gas. Gas evolved turns
damp red litmus paper
blue. Aluminium foil
dissolves.

50
Q

Oxidation is the ______ of oxygen
Reduction is the ______ of oxygen

A

gain, loss

51
Q

Oxidation is the ______ of hydrogen
Reduction is the ______ of hydrogen

A

loss, gain

52
Q

Oxidation is the ______ of electron
Reduction is the ______ of electron

A

gain, loss

53
Q

Oxidation is the ______ of oxidation state
Reduction is the ______ of oxidation state

A

decrease, increase

54
Q

Oxidising agent: KMnO₄(aq) with H₂SO₄(aq)

A

Purple to colourless

MnO4 – (aq) + 8H+ (aq) + 5e- -> Mn2+(aq) + 4H2O(l)

55
Q

Oxidising agent: K₂Cr₂O₇(aq) with H₂SO4(aq)

A

Orange to green

Cr2O7 2- (aq) + 14H+ (aq) + 6e-  2Cr3+(aq) + 7H2O(l)

56
Q

Oxidising agent: H₂O₂

A

Remians colorless but causes other colour change of a reducing agent.

H2O2(aq) + 2H+ (aq) + 2e-  2H2O(l)

57
Q

Oxidising agent: Cl₂

A

Greenish-yellow solution turns colourless.

Cl2(aq) + 2e-  2Cl– (aq)

58
Q

Oxidising agent: I₂

A

Brown to colourless

I2(aq) + 2e-  2I– (aq)

59
Q

Oxidising agent: Fe³⁺

A

Yellow to light green.
Fe3+(aq) + e- -> Fe2+(aq)

60
Q

Reducing agent: KI

A

Colourless solution turns brown.
2I–(aq) -> I2(aq) + 2e-

61
Q

Reducing agent: H₂O₂

A

Effervescence of colourless, odourless gas which relights glowing splint. The gas is oxygen.

H2O2(aq) ->O2(g) + 2H+ (aq) + 2e-

62
Q

Reducing agent: SO₃²⁻, SO₂

A

Remains colorless
SO3 2– (aq) and SO2(g) are oxidised to
SO4 2– (aq)

63
Q

Reducing agent: Fe²⁺

A

Light green to yellow.
Fe2+(aq) -> Fe3+(aq) + e-

64
Q

Reducing agent:

A
65
Q

Reducing agent:

A
66
Q

Reducing agent:

A
67
Q
A
68
Q
A
69
Q
A

3-2 Subjects (1 decks)

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