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

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

A 0.1M solution of potassiu ferrocyanide is 46% dissociated at 18^(@)C . 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 ?

A 0.1 M solution of potassium sulphate, K_2SO_4 is dissolved to the extent of 90%. What would be its osmotic pressure at 27^@C ?