Mixture X of 0.02 mole of [Co(NH3)5SO4]Br and 0.02 mole of [Co(NH3)5Br]SO4 was prepared in 2 litre of solution :
1 litre of mixture X + excess of AgNO3 Y
1 litre of mixture X + excess of BaCl2 Z

Question

Mixture X of 0.02 mole of [Co(NH3)5SO4]Br and 0.02 mole of [Co(NH3)5Br]SO4 was prepared in 2 litre of solution :
1 litre of mixture X + excess of AgNO3 $\rightarrow$ Y
1 litre of mixture X + excess of BaCl2 $\rightarrow$ Z
Number of moles of Y and Z respectively are :

Prashant Kotian · Accepted Answer

Correct answer: C. Step 1: Calculate the concentration of each complex in the 2-liter mixture: both [Co(NH3)5SO4]Br and [Co(NH3)5Br]SO4 have a concentration of 0.02 mol / 2 L = 0.01 M. Step 2: In 1 liter of this mixture, there is exactly 0.01 mol of Br^- ions from [Co(NH3)5SO4]Br and 0.01 mol of SO4^2- ions from [Co(NH3)5Br]SO4. When treated with excess AgNO3, 0.01 mol of Br^- reacts to form 0.01 mol of AgBr precipitate (Y). Step 3: When treated with excess BaCl2, 0.01 mol of SO4^2- reacts to form 0.01 mol of BaSO4 precipitate (Z). Thus, Y = 0.01 and Z = 0.01, which matches option (c).

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