Concentration Based Problem

Concentrated aqueous sulphuric acid is 98% H₂SO₄ by mass and has a density of 1.80 g mL^-1. The volume of acid required to make one litre of 0.1 M H₂SO₄ solution is:

1. 11.10 mL

2. 16.65 mL

3. 22.20 mL

4. 5.55 mL

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

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

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

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

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

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

Mole fraction of solute in a 1.00 molal aqueous solution is:
1. 0.0177
2. 0.0344
3. 1.770
4. 0.1770

The weight of 70% HNO₃ concentrated nitric acid solution that should be used to prepare 250 mL of 2.0 M HNO₃ is:

1. 90.0 g conc. HNO₃
2. 70.0 g conc. HNO₃
3. 54.0 g conc. HNO₃
4. 45.0 g conc. HNO₃

6.02 \times 10²⁰ molecules of urea are present in 100 mL of its solution. The concentration of the solution is:

1.	0.01 M	2.	0.001 M
3.	0.1 M	4.	0.02 M

Calculate the mole fraction of the solute in a 1.00 m aqueous solution.

1.	0.177	2.	0.771
3.	0.0534	4.	0.0177

Which of the following is dependent on temperature?

1.	Molarity	2.	Mole fraction
3.	Weight percentage	4.	Molality