1. Identifying Halides

2. Testing for HALIDE ions – chloride, bromide and iodide ions
Most halides are soluble.
... so add dilute NITRIC ACID
Then add SILVER NITRATE solution
Chloride, bromide & iodide ions produce different coloured PRECIPITATES.

3. DESIGN your own table to record your results
Practical
15 minutes
DESIGN your own table to record your results
Halides
Use your method and observe the reaction between the three known halides with acid and silver nitrate to see the positive result.
Then determine which halide is in
A, B, C, D, E

4. Ag+ (aq) + X- (aq)  AgX (s)
Halides Test
Add dilute nitric acid THEN add silver nitrate
If a precipitate forms then a halide ion is present
The nitric acid is added first to remove any carbonate ions, as these would react with the silver nitrate and form a precipitate too.
Chlorides: White precipitate
Bromides: Cream Precipitate
Iodides: Pale yellow precipitate
Ionic equation (X- represents the halide ion):
Ag+ (aq) + X- (aq)  AgX (s)

5. Testing for HALIDE ions
Testing for ANIONS
Testing for HALIDE ions Cl - Br - I -
chloride , bromide & iodide
iodide ions
YELLOW precipitate
(of AgI)
bromide ions
CREAM precipitate
(of AgBr)
chloride ions
WHITE precipitate
(of AgCl)

6. Ionic equations Na Cl(aq) Ag NO3(aq) Cl(s) +
We aren’t interested in the sodium and nitrate
ions so we simplify the equation:
The state symbols
are crucial, as you need to show that the silver halides (AgCl etc) are formed as solids i.e. (s). This is why you see precipitates in the reactions!
Cl-(aq)
Ag+(aq) Ag
Cl(s) +
Br-(aq)
Ag+(aq) Ag
Br(s) +
I-(aq)
Ag+(aq) Ag
I(s) +