The gas librated , on heating a mixture of two salts with `NaOH` give sa reddish brown precipitate with an alkline solution of `K_(2)HgI_(4)` the aqeous solution of the mixture on treatment with `BaCI_(2)` gives awhite precipitate which is sparingly soluble with `K_(2)Cr_(2)O_(7)` and concentrated `H_(2)SO_(4)`red vapour of A are produced .The aqueous solution of the mixture gives a deep -blue colouration B with potassium ferrcyanide soluble identify the redicals in the gives mixture and write the balanced equation in the gives mixture and write the balanced equations for the formation of A and B

Explanation

To solve the given question, we need to identify the radicals in the mixture of salts and write balanced equations for the reactions described. Let's break down the information step by step:

### Step 1: Identify the gas liberated on heating with NaOH
When a mixture of salts is heated with NaOH, the gas liberated is ammonia (NH₃). This indicates that one of the salts must contain ammonium ions (NH₄⁺).

### Step 2: Identify the reddish-brown precipitate with K₂HgI₄
The reddish-brown precipitate formed when the gas (NH₃) is treated with K₂HgI₄ suggests the presence of ammonium ions. The reaction can be represented as:
\[ \text{NH}_3 + \text{K}_2\text{HgI}_4 \rightarrow \text{Hg}_2\text{I}_2 \text{(s)} + \text{other products} \]
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