The mole fraction of the solute in a 1.00 molal aqueous solution is: 

If 500 mL of a 5 M solution is diluted to 1500 mL, the molarity of the resultant solution is: 

1. 1.5 M

2. 1.66 M

3. 0.017 M

4. 1.59 M

25.3 g of sodium carbonate, Na₂CO₃, is dissolved in enough water to make 250 mL of a solution. If sodium carbonate completely dissociates, the molar concentrations of sodium ion, Na⁺ and carbonate ion, $C{O}_3^{2-}$are respectively:
(molar mass of Na₂CO₃ = 106g mol^-1)

1. 0.955 M and 1.910 M
2. 1.910 M and 0.955 M
3. 1.90 M and 1.910 M
4. 0.477 M and 0.477 M

If 4 g of NaOH dissolves in 36 g of H₂O, the molarity of the solution is: (specific gravity of solution is 1 g mL^-1) : 

The density of a 2 M aqueous solution of NaOH is 1.28 g/$c{m}^3$. The molality of the solution is: 
[molecular mass of NaOH = 40 $gmo{l}^{-1}$]

The molality of a 20% (by mass) CaCO₃ solution is : 
(Given: Density of solution is 1.2 gm/ml)

The total molarity of all the ions present in  0.1 M of CuSO₄ and 0.1 M of Al₂(SO₄)₃ solution is:

1. 0.2M

2. 0.7M

3. 0.8M

4. 1.2M