Select the correct statement. For association of a solute i=1 For complete dissociation of `K_(2)SO_(4)` i =2. For urea solution i=1 For dissociation of solute i=1

The pH of a solution of H_(2)SO_(4) is 1. Assuming complete ionisation, find the molarity of H_(2)SO_(4) solution :

Determine the osmotic pressure of a solution prepared by dissolving 25mg of K_(2)SO_(4) in 2L of water at 25^(@)C , assuming that it is completely dissociated.

Statement-I: 1M solution of Glauber's salt is isotonic with 1M solution of KNO_(3) . Because Statement-II: Solutions having same molar concentration of solute may or may not have same osmotic pressure.

Which relations are not correct for an aqueous dilute solution of K_(3)PO_(4) if its degree of dissociation is alpha ?

Molal depression constant for a solvent is 4.0 kg mol^(-1) . The depression in the freezing point of the solvent for 0.03 mol kg^(-1) solution of K_(2)SO_(4) is : (Assume complete dissociation of the electrolyte)

At 1000K , the pressure of iodine gas is found to be 0.1 atm due to partial dissociation of I_(2)(g) into I(g) . Had there been no dissociation, the pressure would have been 0.07 atm . Calculate the value of K_(p) for the reaction: I_(2)(g)hArr2I(g) .

The Van't Hoff factor for a solute which does not dissociate or associate in solution is

At 1000K, the pressure of iodine gas is found to be 0.112 atm due to partial dissociation of I_(2)(g) into I(g). Had there been no dissociation, the pressure would have been 0.074 atm. Calculate the value of K_(p) for the reaction: I_(2)(g) hArr 2I(g) .

If alpha is the degree of dissociation of Na_(2)SO_(4) the van't Hoff's factor (i) used for calculating the molecular mass is

Van't Hoff factor of 0.1 m aqueous solution of Al_2(SO_4)_3 which undergoes 80% dissociation is