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Chemistry (Inorganic) > Reactions Of Ions In Aqueous Solution > Flashcards

Reactions Of Ions In Aqueous Solution Flashcards

1
Q

What is the equation for pH

A

-log10[H+]

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2
Q

When are metal aqua complexes formed

A

When we add a transition metal compound to water

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3
Q

Draw the structure of (Cu(H2O)6)2+

A
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4
Q

Draw the structure of (Fe(H2O)6)2+

A
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5
Q

Draw the structure of (Fe(H2O)6)3+

A
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6
Q

Draw the structure of (Al(H2O)6)3+

A
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7
Q

What is the pH of metal-aqua ions

A

Below 7, they are acidic in solution

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8
Q

What affects how acidic a metal aqua ion is in solution

A

The charge of the ion

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9
Q

What is the equation for when (Fe(H2O)6)2+ reacts with water

A

(Fe(H2O)6)2+(aq) + H2O(l) ⇌ (Fe(H2O)5(OH))+(aq) + H3O+(aq)

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10
Q

What is H3O+ ion called

A

Hydroxonium ion

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11
Q

What is the term for using water to break a portion of a complex off using water

A

Hydrolysis

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12
Q

What is the equation for when (Fe(H2O)6)3+ reacts with water

A

(Fe(H2O)6)3+(aq) + H2O(l) ⇌ (Fe(H2O)5(OH))2+(aq) + H3O+(aq)

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13
Q

Why do more positively charged ions form more acidic solutions

A

More positively charged ions have a greater charger density
and are more polarising
And so attract electrons in the O-H bond in water ligands more strongly, weakening the bond
Therefore more likely that H+ will be released

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14
Q

What do we form from further hydrolysis of metal-aqua ions

A

Insoluble metal hydroxides

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15
Q

What is the state of the neutral complex formed after repeated hydrolysis using OH- of metal aqua ions

A

Further hydrolysis leads to the formation of a neutral complex that is solid and forms precipitate in solution

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16
Q

Write the equations for the 3 stages for the formation of a solid metal hydroxide precipitate from the hydrolysis of (M(H2O)6)3+(aq)
M = Al3+ and Fe3+

A

(M(H2O)6)3+(aq) + H2O(l) ⇌ (M(H2O)5(OH))2+(aq) + H3O+(aq)
(M(H2O)5(OH))2+(aq) + H2O(l) ⇌ (M(H2O)4(OH)2)+(aq) + H3O+(aq)
(M(H2O)4(OH)2)+(aq) + H2O(l) ⇌ M(H2O)3(OH)3(s) + H3O+(aq)

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17
Q

Why are there only two steps to form an insoluble solid from metal aqua 2+ ions rather than 3 for metal aqua 3+ ions

A

Only two water ligands need to be deprotonated to form a neutral complex

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18
Q

Write the equations for the 2 stages for the formation of a solid metal hydroxide precipitate from the hydrolysis of (M(H2O)6)2+(aq)
M = Cu2+ and Fe2+

A

(M(H2O)6)2+(aq) + H2O(l) ⇌ (M(H2O)5(OH))+(aq) + H3O+(aq)
(M(H2O)5(OH))+(aq) + H2O(l) ⇌ M(H2O)4(OH)2(s) + H3O+(aq)

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19
Q

Which way does equilibrium shift when we add OH- ions to the reaction between a metal aqua ion and water

A

Equilibrium shifts right

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20
Q

Metal hydroxides can act as an acid or base meaning they are….

A

Amphoteric

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21
Q

What is a Bronsted lowry base

A

H+ acceptor

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22
Q

What is a Bronsted lowry acid

A

H+ donor

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23
Q

Give an example of an amphoteric metal hydroxide

A

Al(H2O)3(OH)3

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24
Q

What is the equation for when aluminium hydroxide reacts with a excess base

A

Al(H2O)3(OH)3(s) + OH-(aq) —> (Al(H2O)2(OH)4)-(aq) + H2O(aq)

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25
Q

How does aluminium hydroxide act when we add a base

A

Acts as a Bronsted lowry acid to react with the OH- and therefore it dissolves

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26
Q

How does aluminium hydroxide act when we add an acid

A

Acts as a Bronsted lowry base by accepting H+ ions to form H3O+ in solution and therefore it dissolves

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27
Q

What is the equation for when aluminium hydroxide reacts with an acid

A

Al(H2O)3(OH)3(s) + 3H3O+(aq) —> (Al(H2O)6)3+(aq) + 3H2O(aq)

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28
Q

What do we form when we add small amounts of ammonia to metal aqua ions

A

Metal hydroxide precipitates

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29
Q

Write the equation showing the equilibrium as to how ammonia exists in solution

A

NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH-(aq)

30
Q

What sometimes occurs when we add excess ammonia to metal aqua ions

A

A partial ligand substitution

31
Q

What is the equation for when copper hydroxide reacts with excess ammonia

A

Cu(OH)2(H2O)4(aq) + 4NH3(aq) —> (Cu(NH3)4(H2O)2)2+(aq) + 2OH-(aq) + 2H2O(l)

32
Q

What do we form when we add sodium carbonate to 2+ metal aqua ions

A

Insoluble metal carbonate precipitates

33
Q

What is the general equation for when we add a carbonate to 2+ metal aqua ions

A

(M(H2O)6)2+(aq) + CO32-(aq) ⇌ MCO3(s) + 6H2O(l)

34
Q

Why do we not form a carbonate when we add sodium carbonate to 3+ metal aqua ions

A

3+ metal ions are more acidic than 2+ and there is more H3O+ ions in solution
Carbonate ions react with the free H3O+ ions instead of displacing water ligands like 2+ ions

35
Q

What is the general equation for when we add a carbonate to 3+ metal aqua ions

A

2(M(H2O)6)3+(aq) + 3CO2-(aq )⇌ 2M(OH)3(H2O)3(s) + 3CO2(g) + 3H2O(l)

36
Q

What is observed when we add sodium carbonate to 3+ metal aqua ions

A

Fizzing
(due to CO2 produced)

37
Q

What is observed when we add NaOH to Fe2+ Cu2+ Al3+ and Fe3+

A

All react to form precipitates

38
Q

State and explain what is observed when we add excess NaOH to an aluminium hydroxide precipitate

A

It dissolves as it is amphoteric
White precipitate to a colourless solution

39
Q

What is observed when we add NH3 to Fe2+ Cu2+ Al3+ and Fe3+

A

All react to form precipitates

40
Q

When adding NaOH to Fe2+ Cu2+ Al3+ and Fe3+, a precipitate is formed. Which is the only precipitate that dissolves in excess NaOH

A

Aluminium hydroxide

41
Q

When adding NH3to Fe2+ Cu2+ Al3+ and Fe3+, a precipitate is formed. Which is the only precipitate that dissolves in excess NH3

A

Copper Hydroxide

42
Q

State and explain what is observed when we add excess NH3 to a Copper Hydroxide precipitate

A

Dissolves as there is a ligand substitution
Colour goes from pale blue precipitate to dark blue solution
(pale blue precipitate dissolves to form a dark blue solution)

43
Q

What is observed when we add Na2CO3 to Fe2+ Cu2+ Al3+ and Fe3+

A

All react to form precipitates

44
Q

What is observed when Al3+ and Fe3+ react with sodium carbonate

A

A precipitate and bubbles (CO2 formed)

45
Q

Do we produce a gas when Cu2+ and Fe2+ react with sodium carbonate

A

No, only a precipitate is formed

46
Q

Why must any Fe2+ solution being tested be made fresh

A

Fe2+ oxidises readily with air to form Fe3+

47
Q

What colour is Cu2+(aq)

A

Blue

48
Q

What colour is observed when we add small amounts of OH-(aq) or NH3(aq) to Cu2+(aq)

A

Pale blue precipitate

49
Q

What colour is observed when we add excess OH-(aq) to the precipitate formed from adding small amounts of OH-(aq) to Cu2+(aq)

A

No change
Insoluble in excess NaoH

50
Q

What colour is observed when we add excess NH3(aq) to the precipitate formed from adding small amounts of NH3(aq) to Cu2+(aq)

A

Dark blue solution

51
Q

What colour is observed when we add Na2CO3(aq) to Cu2+(aq)

A

Green - Blue precipitate

52
Q

What colour is Fe2+(aq)

A

Pale green

53
Q

What colour is observed when we add small amounts of OH-(aq) or NH3(aq) to Fe2+(aq)

A

Dirty green precipitate

54
Q

What colour is observed when we add excess OH-(aq) to the precipitate formed from adding small amounts of OH-(aq) to Fe2+(aq)

A

No change
Insoluble in excess NaoH

55
Q

What colour is observed when we add excess NH3(aq) to the precipitate formed from adding small amounts of NH3(aq) to Fe2+(aq)

A

No change
Insoluble in excess NH3

56
Q

What colour is observed when we add Na2CO3(aq) to Fe2+(aq)

A

Green precipitate

57
Q

What colour is Fe3+(aq)

A

Yellow

58
Q

What colour is observed when we add small amounts of OH-(aq) or NH3(aq) to Fe3+(aq)

A

Orange precipitate

59
Q

What colour is observed when we add excess OH-(aq) to the precipitate formed from adding small amounts of OH-(aq) to Fe3+(aq)

A

No change
Insoluble in excess NaoH

60
Q

What colour is observed when we add excess NH3(aq) to the precipitate formed from adding small amounts of NH3(aq) to Fe3+(aq)

A

No change
Insoluble in excess NH3

61
Q

What colour is observed when we add Na2CO3(aq) to Fe3+(aq)

A

Brown precipitate

62
Q

What colour is Al3+(aq)

A

Colourless

63
Q

What colour is observed when we add small amounts of OH-(aq) or NH3(aq) to Al3+(aq)

A

White precipitate

64
Q

What colour is observed when we add excess OH-(aq) to the precipitate formed from adding small amounts of OH-(aq) to Al3+(aq)

A

Colourless solution

65
Q

What colour is observed when we add excess NH3(aq) to the precipitate formed from adding small amounts of NH3(aq) to Al3+(aq)

A

No change

66
Q

What colour is observed when we add Na2CO3(aq) to Al3+(aq)

A

White precipitate

67
Q

Draw the table for colours of the ions Cu2+, Fe2+, Fe3+, Al3+

A
68
Q

What is the the equation for adding drops (not excess) of OH- to (Al(H2O)6)3+

A
69
Q

What ion does NH3 form

A

NH4+

70
Q
A
71
Q

Write the colour observed, final species and equation when (Cu(H2O)6)2+ reacts with concentrated HCl

A

Chemistry (Inorganic) (7 decks)

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