The osmotic pressure of `0.010 M` potassium iodide solution `(KI)` at `25^(@)C` is `0.465 atm`. Calculate the van't hoff factor for `KI` at this concentration.
Strategy: Use the modified equation `(2.78)` to account for the effect of dissociation of KI in water.

Determining colligative properties of ionic solutions: Estimate the freezing point of a 0.010 m aqueous solution of aluminium sulphate, Al_(2)(SO_(4))_(3) . Assume the value of i based on the formula of the compound. Strategy: Use the modified equation (2.77) to account for the effect of dissociation of Al_(2)(SO_(4))_(3) in water. The van't hoff factor, i , is equal to the number of ions furnished per formula unit (assuming 100% dissociation.)

The osmotic pressures of 0.010 M solutions of KI and sucrose ( C_(12)H_(22)O_(11) ) are 0.432 atm and 0.24 atm respectively. The van't Hoff factor for KI is :

The osmotic pressures of 0.010 M solutions of KI and sucrose ( C_(12)H_(22)O_(11) ) are 0.432 atm and 0.24 atm respectively. The van't Hoff factor for KI is :

The osmotic pressures of 0.010 M solutions of KI and sucrose ( C_(12)H_(22)O_(11) ) are 0.432 atm and 0.24 atm respectively. The van't Hoff fector for KI is :

The osmotic pressures of 0.010 M solutions of KI and of sucrose (C_(12)H_(22)O_(11)) are 0.432 atm and 0.24 atm respectively. The vant's Hoff factor for KI is:

The osmotic pressure of 0.010 M solutions of Kl and of sucrose (C_(12)H_(22)O_(11)) are 0.432 atm and 0.24 atm respectively . The van't Hoff factor for Kl is :

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