Brainscape's Knowledge GenomeTM

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


See full index

chemistry > Solubility and salt preparation > Flashcards

Solubility and salt preparation Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q
  1. What is a solvent?
A

A liquid that a solute dissolves in

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
1
Q
  1. What is a solute?
A

A solid that dissolves in a solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q
  1. What is a solution?
A

The mixture produced when a solute is dissolved in a solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q
  1. What is a saturated solution?
A

The maximum mass of solute that can dissolve in a solvent for a given temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q
  1. How does solubility increase with temperature?
A

Solubility increases with temperature, the higher the temperature, the more solute can be dissolved

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

How is solubility measured?

A

In [mass] (g)/100g [liquid solute is dissolving in]

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

Solubility rules

A

Halides (iodides, chlorides, bromides) Soluble except lead (Pb) and silver (Ag) halides
Hydroxides and oxides (OH) Insoluble except group 1 and ammonium
Sulfates (SO4) Soluble except barium (Ba) and calcium (Ca)
Group 1 and ammonium (NH4) Always soluble
Carbonates (CO3) Insoluble except group 1 and ammonium (calcium carbonate is slightly soluble in water)
Nitrates Always soluble

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

Formulae of sulphate ions

A

SO4 2-

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

Formulae of nitrate ions

A

NO3 -

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

Formulae of carbonate ions

A

CO3 2-

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

Formulae of hydroxide ions

A

OH-

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

Formulae of sulphuric acid

A

H2SO4

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

Formulae of nitric acid

A

HNO3

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

Formulae of Hydrochloric acid

A

HCL

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

Formulae of ammonia

A

NH3

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

Formulae of ammonium

A

NH4+

16
Q

Formulae of lead ion

A

Pb 2+

17
Q

Formulae of hydrogen ion

A

H +

18
Q

Formulae of silver ion

A

Ag +

19
Q

Formulae of zinc ion

A

Zn 2+

20
Q

What is an acid?

A

A donor of H+ ions (HCl, HNO3, H2SO4)(CH3COOH – ethanoic acid)

21
Q

What is a base?

A

A source of OH- ions that reacts with an acid

22
Q

What is a salt made up of?

A

A metal bromide/nitrate/sulfate/iodide/chloride

23
Q

What happens when two salt solutions are mixed together that produce soluble salts ?

A

There is no reaction as the products of the reaction are both soluble, so ions diffuse around the solution

24
Q

What is a precipitate?

A

An insoluble solid that is produced in a precipitation reaction

25
Q

How are precipitates formed?

A

By precipitation reactions
Two soluble salts react to make an insoluble salt and a soluble salt

26
Q

What can and cannot be made using a precipitation reaction?

A

Soluble salts cannot be made using the precipitation reaction
They would be made using the copper(II)sulfate method that starts from an acid and an alkali
Example: copper(II)oxide + sulfuric acid —> copper(II)sulfate + water
Insoluble salts can be made using the precipitation reaction
Soluble salt + soluble salt —> insoluble salt + soluble salt

27
Q

How is a pure, dry sample of an insoluble salt prepared?

A
  • Mix solution of two soluble reactants
  • Filter mixture (insoluble salt will remain on filter paper)
  • Wash the salt with distilled water (makes sure the sample is pure)
  • Leave the salt to dry
28
Q

Rules when writing ionic equations

A

Write out a balanced symbol equation
Ionic compounds (soluble), acids and bases dissociate (split up)
Cancel out terms that appear on both sides of the equation (spectator ions)
Substances that do not dissociate do not become charged (eg H2)

29
Q

What types of compounds are usually coloured?

A

Transition metal compounds

30
Q

Copper(II)sulfate colour

A

Light blue solution

31
Q

Lead(II)nitrate colour

A

Colourless solution

32
Q

Iron(III)chloride colour

A

Yellow solution

33
Q

Table recording results of precipitation reactions practical with colour changes

A

Copper(II)sulfate + potassium iodide
Light blue solution to red-brown precipitate

Copper(II)sulfate + sodium hydroxide
Bright blue precipitate (gelatinous appearance) formed in light blue solution

Copper(II)sulfate + potassium sulfate
No change - stayed a light blue solution

Lead(II)nitrate + potassium iodide
Colourless to opaque bright yellow precipitate

Lead(II)nitrate + sodium hydroxide
White preciptate formed from colourless solution

Lead(II)nitrate + potassium sulfate
No colour change – stayed a colourless solution

Iron(III)chloride + potassium iodide
No colour change – stayed a yellow solution

Iron(III)chloride + sodium hydroxide

Iron(III)chloride + potassium sulfate
No colour change – stayed a yellow solution

chemistry (2 decks)

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