[" 10.A solution contains "0.8960g" of "K_(2)SO_(4)" in "500ml" solution .Its osmotic pressure is found to be "],[0.690atm" at "27^(@)C" .Calculate the value of van't hoff factor."(R=0.082atmmol^(-1)K^(-1))]

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 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 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) )

A decinormal solution of NaCl exerts an osmotic pressure of 4.6 atm. at 300 K. Calculate its degree of dissociation. (R=0.082Latm.K^(-1)mol^(-1))

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

What is meant by Vant Hoff's factor? The Osmotic pressure of 0.0103 molar Solution of an electrolyte is found to be 0.70 atm at 27 C. Calculate the Vant Hoff factor [R=0.082" liter "mol^(-1) K^(-1)] .