[Michael]

Hello again i have another problem,

It deals with identification tests of chlorides, bromides and iodides.

The materials are:
Silver nitrate solution
Dilute HNO₃
NaBr
NaCl
KI

From what i have researched i learnt that:

Chlorides give a white curdy ppt of silver chloride which dissolves in ammonia

Bromides give a creamy ppt of silver bromide which dissolve slightly in cold ammonia soultion.

Iodides gives a yellow ppt of silver iodide which does not dissolve in ammonia solution.

In each case a few drops of dilute HNO₃ was added first followed by the silver nitrate.

Why was HNO₃ added in each case.

What are the reactions taking place (equations)?

Why was "cold" ammonia solution needed?

What changes would be observered in each case other than the ones stated above like in colour or other wise. if any?

And for the quest for more knowledge what effects will concentrated sulphuric acid have on the bromides, chlorides and iodides (equations)?

I am limited to picturing what these reactions are like because i haven't the oppertunity to do them. So your help will be greatly appreciated.

Thanks in advance.

[AWK]

Why was HNO3 added in each case.

Many anions form precipitates with AgNO3. This is for check we are dealing with halides

What are the reactions taking place (equations)?

Ag(+) + X(-) = AgX(s)

Why was "cold" ammonia solution needed?

Only concentrated ammonia dissolves AgBr. Solubility of NH3 in water strongly depends on temperature.

What changes would be observered in each case other than the ones stated above like in colour or other wise. if any?

AgCl(s) + 2NH3 = [Ag(NH3)2]Cl - ppt disappears, colorless solution
AgBr(s) + 2NH3 (concentrated) = partiall dissolution of ppt

And for the quest for more knowledge what effects will concentrated sulphuric acid have on the bromides, chlorides and iodides (equations)?

2NaCl + H2SO4 = 2HCl + Na2SO4
For NaBr and NaI with conc. H2SO4 the same reaction take place follloved by
2HX + H2SO4 = X2 + SO2 + 2H2O