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1 L, 0.02 M solution of [Co(NH3)5SO4]Br is mixed with 1 L, 0.02 M solution of [Co(NH3)5Br]SO4. The resulting solution is divided into two equal parts (X) and treated with excess of AgNO3 solution and BaCl2 solution respectively as shown below: 1 L Solution (X) + AgNO3 solution (excess) → Y 1 L Solution (X) + BaCl2 solution (excess) → Z The number of moles of Y and Z respectively are

1. 0.02, 0.02
2. 0.01, 0.01
3. 0.02, 0.01
4. 0.01, 0.02

Correct answer: 0.02, 0.01

Solution

In the mixed solution, both complexes contribute to the total concentration of cobalt ions. When treated with AgNO3, all the bromide ions from [Co(NH3)5Br]SO4 react, resulting in 0.02 moles of precipitate, while BaCl2 reacts with the sulfate ions from [Co(NH3)5SO4]Br, leading to 0.01 moles of precipitate due to the stoichiometry of the sulfate ions.

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