9 — salts

Question 1

Spectator ions

Answer 1

Spectator ions r substances that remain unchanged in their physical state or charge and do not take part in the reaction

Question 2

To evaporate to dryness vs to crystallise

Answer 2

D:
- crystals r anhydrous
C:
- crystals r hydrated

D:
- salt must be stable to heat
C:
- salt is decomposed by heat

D:
- solubility of salt does not vary much w hot tempt
C:
- solubility of salt s much greater in water at high temperature

Question 3

Spectator ions

Answer 3

Spectator ions r substances that remain unchanged in their physical state or charge n do not tk part in the reaction

Question 4

To prepare soluble salts

Answer 4

1. Titration
   - SPA + Group 1
2. Acid+ insoluble B.C.M.
   - non group 1 or SPA but soluble
   - insoluble B.C.M.in excess to use up the acid, preventing contamination of salt w acid

Both methods:
Acid containing anion of the salt + XCO3 (CO3 containing cation of the salt )

Question 5

Acid + B.C. M. Procedure

Answer 5

1. Fill half a beaker with x acid. Add excess y carbonate and stir continuously until no more y carbonate will dissolve or when no more effervescence observed (metal/carbonate + acid)
2. Filter to remove excess y carbonate, collect the filtrate which is the YX solution
3. Heat the filtrate till a hot saturated solution is obtained
4. Test for saturation by dipping a glass rod into filtrate, if filtrate is saturated, crystals will form on glass rod
5. Leave saturated solution to cool and crystallise
6. Filter to collect the residue. Wash the crystals with distilled water to remove impurities. Dry the crystals betw a few sheets of filter paper.

Question 6

Titration apparatus

Answer 6

1. Burette
2. Pipette and pipette filter
3. Conical flasks
4. Appropriate indicator

Question 7

Titration procedure

Answer 7

1. Fill up a burette with dilute nitric acid. Note the initial burette reading (V1, cm3).
2. Pipette 25.0cm of dilute sodium hydroxide solution into a conical flask.
3. Add 2-3 drops of methyl orange (indicator) to the sodium hydroxide solution. The solution turns yellow.
4. While swirling the conical flask, add dilute nitric acid from the burette slowly until the solution just turns orange permanently. This is the end-point.
5. Record the final burette reading as V2 cm3.

Volume of acid required = (V2 - V1) cm^3

Reaction is repeated without the addition of an indicator as the indicator would cause the salt to be impure.

6. Pipette 25.0cm of sodium hydroxide solution into a conical flask.
7. Add (V2 - V1) c m of dilute nitric acid from the burette.
8. Heat the solution to evaporate the water until a hot saturated solution is obtained.
9. Allow the saturated solution to cool and crystallise.
10. Filter to collect the residue.
11. Wash crystals with a little cold water to remove impurities.
12. Dry the crystals between sheets of filter paper.

Question 8

Precipitation

Answer 8

(Cation + NO3) + (SPA + anion)

1. Add and mix (SPA + anion) solution to (cation + NO3) solution and stir until no more precipitate forms
2. Filter to collect the side
3. Wash the residue w small amount of distilled water to remove impurities
4. Allow precipitate to dry on a piece of filter paper