Equimolal solutions of 'NaCl' and 'BaCl_2' are prepared in 'H_2 O'. Freezing point of 'NaCl' is found to be-` 2 C` . What is the freezing point of `BaCl_2` ?

The freezing point of equimolal aqueous solution will be highest for

Anhydrous 'BaO_2' is not used for preparing 'H_2 O_2 .' Why?

Give the correct order of initials T or F for the given statements. Use T for true statement and F for false statement: S1: Agl is less water soluble than AgF due to more polarisation of l ^(-) compared to F ^(-) S:2 Melting point of BaCl _(2) is higher than that of Be Cl _(2) due to higher ionic nature of BaCl _(2) S3: Order of lattice energy -NaF lt MgO lt AlN lt SiC : TTT, TTF, TFT, FTT,

A 5% solution (by mass) of cane sugar (C_12 H_22 O_11) in water has a freezing point of 271 K. Calculate the freezing point of 5%. (by mass) solution of glucose (C_6 H_12 O_6) In water. Freezingpoint of pure water is 273.15 K.

When 1 mole of a solute is dissolved in 1 kg of H_(2)O , boilling point of solution was found to be 100.5^(0)C . K_(b) for H_(2)O is

Assertion : Larges the value of cryoscopic constant of the solvent lesser will be the freezing point of the solution Reason : Depression in the freezing point depends on the nature of the solvent. a)If both (A) and (R) are correct and (R) is the correct explanation of(A). b)If both (A) and (R) are correct, but (R) is not the correct explanation of (A). c)If (A) is correct, but (R) is incorrect. d)If both (A) and (R) are incorrect.

What is false about 'H_2 O_2' ?

Assertion : Higher the value of molal depression constant of solvent (K) used to prepare the solution, lower will be the freezing point of the solution. Reason : Depression in freezing point depends upon the nature of the solvent. a)If both (A) and (R) are correct and (R) is the correct explanation of(A). b)If both (A) and (R) are correct, but (R) is not the correct explanation of (A). c)If (A) is correct, but (R) is incorrect. d)If both (A) and (R) are incorrect.

In the depression of freezing point experiment it is found that (i) The vapour pressure of the solution is less than that of pure solvent (ii) The vapour pressure of the solution is more than that of pure solvent (iii) Only solute molecules solidify at the freezing point (iv) Only solvent molecules solidify at the freezing point