Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry: Inorganic > 6: Reaction of Ions in Aqueous Solution > Flashcards

6: Reaction of Ions in Aqueous Solution Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

How many H2O molecules bind to a metal ion?

A

6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

How do we name metal aqua ions?

A

Hexaaqua for the 6 H2O
Then the metal name
Eg: Hexaaquacopper

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What type of bonds are found in metal aqua ions?

A

Coordinate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Give 2 hydrolysis equations, starting with [Fe(H2O)6]2+, that show the acidity. The final product should be [Fe(OH)2(H2O)4]

A

[Fe(H2O)6]2+ + H2O = [Fe(H2O)5(OH)]+ + H3O+
[Fe(H2O)5(OH)]+ + H2O = [Fe(OH)2(H2O)4] + H3O+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Give 3 hydrolysis equations, starting with [Al(H2O)6]3+, that show the acidity of 3+ ions. The final product should be [Al(OH)3(H2O)3]

A

[Al(H2O)6]3+ + H2O = [Al(H2O)5(OH)]2+ + H3O+
[Al(H2O)5(OH)]2+ + H2O = [Al(OH)2(H2O)4]+ + H3O+
[Al(OH)2(H2O)4]+ + H2O = [Al(OH)3(H2O)3] + H3O+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Give 2 reasons why 3+ ions are more acidic.

A

They have a larger charger and are therefore smaller
3+ Ions are more polarising

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What does it mean to say that 3+ ions are more polarising to water ligands?

A

They have a higher charge and therefore attract more electrons from the oxygen in the water molecule, in the coordinate bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

When OH- is added during hydrolysis, how does this affect equilibrium?

A

This removes H3O+ ions, so equilibrium shifts right to try and raise concentration of these ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Give an overall hydrolysis equation for [Fe(H2O)6]3+ with NH3

A

[Fe(H2O)6]3+ + 3NH3 = [Fe(OH)3(H2O)3] + 3NH4+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Give an overall hydrolysis equation for [Cu(OH)6]4- with NH3

A

[Cu(OH)6]4- + 4NH3 = [Cu(NH3)4(H2O)2]2+ + 6OH-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Give a general overall ionic equation for the hydrolysis of metal aqua ion [M(H2O)6]2+ using Na2CO3

A

[M(H2O)6]2+ + CO3 2- = MCO3 + 6H2O

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What colour will the precipitate produced be when NaOH is added to a solution of Fe3+ ions?

A

Brown precipitate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Give the overall reverse hydrolysis equation for the formation of [Fe(H2O)6]3+ from Fe(OH)3(H2O)3

A

Fe(OH)3(H2O)3 + 3H+ =[Fe(H2O)6]3+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What does amphoteric mean?

A

Where a substance can act as both an acid or a base.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Give an equation for Al(OH)3(H2O)3 to form [Al(OH)4(H2O)2]- where it acts as a Bronsted Lowry acid.

A

Al(OH)3(H2O)3 + OH- = [Al(OH)4(H2O)2]- + H2O

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Give an equation showing Al(OH)3(H2O)3 acting as Bronsted Lowry base.

A

Al(OH)3(H2O)3 + 3H+ = [Al(H2O)6]3+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

If you add some OH- to [Fe(H2O)6]2+, what will you observe before and after?
What will you observe if OH- is added in excess?

A

Green solution to turns to green precipitate
No visible change

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

If you add some OH- to [Cu(H2O)6]2+, what will you observe before and after?
What will you observe if OH- is added in excess?

A

Blue solution to blue precipitate
No visible observation

19
Q

If you add some OH- to [Fe(H2O)6]3+, what will you observe before and after?
What will you observe if OH- is added in excess?

A

Orange solution to brown precipitate
No visible observation

20
Q

If you add some OH- to [Al(H2O)6]3+, what will you observe before and after?
What will you observe if OH- is added in excess?

A

Colourless solution to white precipitate
No visible reaction

21
Q

If you add some NH3 to [Fe(H2O)6]2+, what will you observe before and after?
What will you observe if NH3 is added in excess?

A

Green solution to green precipitate
No visible change

22
Q

If you add some NH3 to [Cu(H2O)6]2+, what will you observe before and after?
What will you observe if NH3 is added in excess?

A

Blue solution to blue precipitate
Deep blue precipitate

23
Q

If you add some NH3 to [Fe(H2O)6]3+, what will you observe before and after?
What will you observe if NH3 is added in excess?

A

Orange solution to brown precipitate
No visible change

24
Q

If you add some NH3 to [Al(H2O)6]3+, what will you observe before and after?
What will you observe if NH3 is added in excess?

A

Colourless solution to white precipitate

25
Q

If you add some CO3 2- to [Fe(H2O)6]2+, what will you observe before and after?

A

Green solution to green precipitate

26
Q

If you add some CO3 2- to [Cu(H2O)6]2+, what will you observe before and after?

A

Blue solution to blue/green precipitate

27
Q

If you add some CO3 2- to [Fe(H2O)6]3+, what will you observe before and after?

A

Orange solution to brown precipitate with bubbles

28
Q

If you add some CO3 2- to [Al(H2O)6]3+, what will you observe before and after?

A

Colourless solution to white precipitate and gentle bubbling

29
Q

If you add excess acid to [Fe(H2O)4(OH)2], what will you observe before and after?

A

Green precipitate to green solution

30
Q

If you add excess acid to [Cu(H2O)4(OH)2], what will you observe before and after?

A

Blue precipitate to blue solution

31
Q

If you add excess acid to [Fe(H2O)3(OH)3], what will you observe before and after?

A

Brown precipitate to pale violet solution

32
Q

If you add excess acid to [Al(H2O)3(OH)3], what will you observe before and after?

A

White precipitate to colourless solution

33
Q

If you add excess alkali to [Fe(H2O)3(OH)3], [Fe(H2O)4(OH)2] and [Cu(H2O)4(OH)2] what will you observe before and after?

A

No visible change

34
Q

If you add excess alkali to [Al(H2O)3(OH)3], what will you observe?

A

White precipitate to colourless solution

35
Q

What is an acidic hydroxide?

A

A hydroxide that reacts with bases only.

36
Q

What is a basic hydroxide?

A

A hydroxide that reacts with acids only.

37
Q

Name the 3 basic hydroxides.

A

[Cu(H2O)4(OH)2]
[Fe(H2O)4(OH)2]
[Cu(H2O)3(OH)3]

38
Q

State the observations you would see before and after adding excess Cl- to [Fe(H2O)6]2+

A

Green solution to yellow solution

39
Q

State the observations you would see before and after adding excess Cl- to [Cu(H2O)6]2+

A

Blue solution changes to yellow

40
Q

State the observations you would see before and after adding excess Cl- to [Fe(H2O)6]3+

A

Orange solution changes to yellow

41
Q

State the observations you would see before and after adding excess Cl- to [Al(H2O)6]3+

A

Solution remains colourless

42
Q

What is formed when you add Na2CO3 to [Al(H2O)6]3+?
What do you observe?
Give an equation.

A

Al(CO3)3(OH)3
Bubbles
2 [Al(H2O)6]3++ 3CO3 2–
-> 2 Al(H2O)3(OH)3 + 3H2O + 3CO2

43
Q

Give a condition needed for the formation of [Al(OH)4]- from [Al(H2O)6}3+ and NaOH.
Give an equation.

A

Excess NaOH
[Al(H2O)6]3+ + 4 OH- ->[Al(OH)4]– + 6 H2O

44
Q

Explain, with the use of an equation, why a solution containing [Al(H2O)6]3+ has a pH below 7.

A

[Al(H2O)6]3+ + H2O ⇌ [Al(H2O)5(OH)]2++ H3O+
Al3+ has a small size and high charge
This weakens the OH bond in water, releasing H+ ions

Chemistry: Inorganic (8 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions