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

1. 1.5 M

2. 1.66 M

3. 0.017 M

4. 1.59 M

At STP, the density of CCl₄ vapour in g/L will be closest to: 

1. 8.67

2. 6.87

3. 3.67

4. 4.26

Which of the following is dependent on temperature?

The molality of pure water is: 

1. 1 m

2. 18 m

3. 55.5 m

4. None of the above

20 g of sugar is dissolved in enough water to make a final volume of 2L. The concentration of sugar (C₁₂H₂₂O₁₁) in mol L^–1  will be:

1. 0.29 mol/L

2. 0.029 mol/L

3. 0.35 mol/L

4. 0.032 mol/L

1. $12.044\times {10}^{20}$ molecules

2. $6.022\times {10}^{23}$ molecules

3. $1\times {10}^{23}$ molecules

4. $12.044\times {10}^{23}$ molecules

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 volume occupied by one water molecule (density = 1 g cm^-3) is:

1. $9.0\times {10}^{-23}$ $$ ${\mathrm{cm}}^3$

2. $6.023\times {10}^{-23}$ $$ ${\mathrm{cm}}^3$

3. $3.0\times {10}^{-23}$ $$ ${\mathrm{cm}}^3$

4. $5.5\times {10}^{-23}$ $$ ${\mathrm{cm}}^3$