A `0.1M` solution of potassiu ferrocyanide is `46%` dissociated at `18^(@)C`. What will be its osmotic pressure?

An M/10 solution of potassium ferrocyanide is 46% dissociated at 300 K . What will be its osmotic pressure?

An M/10 solution of potassium ferrocyanide is 46% dissociated at 300 K . What will be its osmotic pressure?

An M/10 solution of potassium ferrocyanide is 46% dissociated at 300 K . What will be its osmotic pressure?

A decimolar solution of potassium ferrocyanide is 50% dissociated at 300K . Calculate osmotic pressure of the solution. (Given S = 8.341 JK^(-1) mol^(-1) )

A decimolar solution of potassium ferrocyanide is 50% dissociated at 300K . Calculate osmotic pressure of the solution. (Given S = 8.341 JK^(-1) mol^(-1) )

A decimolar solution of pottassium ferrocyanide is 50% dissociated at 300 K. The osmotic pressure of the solution is (Given R=8.314JK^-1mol^-1 )

A decimolar solution of potassium ferrocyanide is 50% dissociated at 300K. It's Osmotic pressure is 7.482 x10^(x) Nm^(-2) . Find x ?

2 millimolar solution of sodium ferrocyanide is 60% dissociated at 27^@C Osmotic pressure of the solution is