A solution contains `0.8133 g` of `K_(2)SO_(4)` in `500 mL`. If osmotic pressure is found to be `0.69 atm` at `27^(circ)C`. Calculate the value of van't Hoff's factor.

A solution cantains 0.8960 g of K_(2)SO_(4) in 500 mL. Its osmotic pressure is found to be 0.69 atm at 27^(@)C . Calculate the value of Van't Hoff factor.

A solution contins 0 .860 g of K_(2)SO_(4) in 500 mL solution . Its osmotic pressure is found to be 0.690 atm at 27^(@)C . Calculate the value of Van't Hoff factor . (At mass K = 39.0 , S = 32, O = 16 R = 0.082 atm mol^(-1) K^(-1) )

What is the value of Van't Hoff's factor (i) for K_2SO_4 ?

The osmotic pressure of a solution containing 5 g of substance (molar mass =100) in 308 m L of solution was found to be 4.0 atm at 300 K . Calculate the value of solution constant (R)

The osmotic pressure of a solution containing 5 g of substance (molar mass =100) in 308 m L of solution was found to be 4.0 atm at 300 K . Calculate the value of solution constant (R)

The osmotic pressure of a solution containing 5 g of substance (molar mass =100) in 308 m L of solution was found to be 4.0 atm at 300 K . Calculate the value of solution constant (R)

Osmotic pressure of a 0.01 M solution is 0.7 atm at 27^(@)C , its van't Hoff factor will be

Osmotic pressure of a 0.01 M solution is 0.7 atm at 27^(@)C , its van't Hoff factor will be