Question

2 litres of a 1 molar solution of a complex salt CrCl3.6H2O (molar mass 266.5g molâˆ’1) 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
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
B
The clear solution will show an osmotic pressure of 98.52 atm
No worries! Weâ€˜ve got your back. Try BYJUâ€˜S free classes today!
C
The clear solution will show an osmotic pressure of 65.68 atm
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
D
2 moles of [Cr(H2O)6](NO3)3 will be present in the solution
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
Open in App
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 solutionπ=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++3Cl−1 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

Suggest Corrections
5
Join BYJU'S Learning Program
Related Videos
Van't Hoff Factor
CHEMISTRY
Watch in App
Explore more
Join BYJU'S Learning Program