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Question

2 litres of a 1 molar solution of a complex salt CrCl3.6H2O (molar mass 266.5g mol1) shows an osmotic pressure of 98.52 atm. The solution is now treated with 1 litre of 6 M AgNO3. Which of the following statements is/are correct?

A
Mass of AgCl precipitated is 861 g
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B
The clear solution will show an osmotic pressure of 98.52 atm
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C
The clear solution will show an osmotic pressure of 65.68 atm
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D
2 moles of [Cr(H2O)6](NO3)3 will be present in the solution
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Solution

The correct options are
A Mass of AgCl precipitated is 861 g
C The clear solution will show an osmotic pressure of 65.68 atm
D 2 moles of [Cr(H2O)6](NO3)3 will be present in the solution
π=C×R×T×i
As strong electrolyte then i = n.
π=C×R×T×n
98.52=1×0.0821×300×n
n = 4

CrCl3.6H2O can be written as:
[Cr(H2O)6]Cl3 [Cr(H2O)6]3++3Cl1
1
1- α α 3α

therefore
3 mole of AgNO3 will react with 1 mole of [Cr(H2O)6]Cl3

[Cr(H2O)6]Cl3+AgNO3[Cr(H2O)6](NO3)3+3AgCl
2 6
0 0 2 6
therefore
moles of AgCl formed = 6
mass of AgCl formed = 6× 143.5= 861g

[Cr(H2O)6](NO3)3 =23
π=23×0.0821×300×4
= 65.68 atm


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