Question

Q6. A mixture named X contains 0.03 moles of [Co(NH3)5SO4]Br and 0.03 moles of [Co(NH3)5Br]SO4 the total volume of the mixture is 3 L. Calculate the number of moles of Y formed when 1 L of mixture of X is treated with excess of AgNO3 solution?

Answer 1

Answer:

0.01 mole of AgBr and 0.01 mol of AgSO4

Explanation:

Let's calculate the molarity of the complexes.

We have 0.03 moles in 3 L. So the molarity become 0.01 M solution [Co(NH3)5SO4]Br and  [Co(NH3)5Br]SO4  respectively.

There will be 0.01 moles of each complex in 1 L of solution. When the solution is treated with excess of AgNO3, AgBr and AgSO4 will precipitate out.

1 mole of AgNO3 forms 1 mole of AgBr

Similarly 1 mole of AgNO3 forms one mole of AgSO4

When 1 L solution is treated with the excess of AgNO3 solution 0.01 moles of AgBr and 0.01 moles of AgSO4 will be formed.