Study text: "Essential Mathematics and Statistics for Science", 2nd Edition,

G Currell & A A Dowman, Wiley-Blackwell, 2009

G Currell & A A Dowman, Wiley-Blackwell, 2009

A solution of NaOH contains 0.020 mol in a volume of 10 mL (= 10 cm ^{3}).

Calculate the concentration in moles per litre (mol L^{-1}, mol dm^{-3}or M).

(Note 1.0 L = 1.0 dm^{3}= 1000 mL = 1000 cm^{3}and 1.0 M = 1.0 mol L^{-1})- 0.20 mol L
^{-1}(= 0.20 mol dm^{-3}= 0.20 M) - 2.0 mol L
^{-1}(= 2.0 mol dm^{-3}= 2.0 M) - 0.0020 mol L
^{-1}(= 0.0020 mol dm^{-3}= 2.0 mM)

- 0.20 mol L
0.04 grams of a solute is dissolved in a solvent, giving a solution with a final volume of 25 mL (= 25 cm ^{3}). Calculate the concentration in g L^{-1}.

(Note 1.0 L = 1.0 dm^{3}= 1000 mL = 1000 cm^{3})- 0.625 g L
^{-1}(= 0.625 g dm^{-3}) - 0.16 g L
^{-1}(= 0.16 g dm^{-3}) - 1.6 g L
^{-1}(= 1.6 g dm^{-3})

- 0.625 g L
Calculate the mass (in g) of CuSO _{4}.5H_{2}O that must be dissolved in a final volume of 200 mL of solvent to obtain a concentration of 4.0 g L^{-1}.- 20 g
- 0.80 g
- 0.20 g

Calculate the mass (in g) of CuSO _{4}.5H_{2}O that must be dissolved in a final volume of 50 mL of solvent to obtain a molar concentration

of 0.04 mol L^{-1}.

Relative molecular mass of hydrated copper sulphate = 250.- 0.0080 g
- 0.20 g
- 0.50 g

A solution has a concentration of 8.0 g L ^{-1}.

Calculate the volume of solution (in mL) that will contain 0.50 g of solute.- 62.5 mL
- 16.0 mL
- Neither of the above

Calculate the mass (in g) of NaCl required to make up 500 mL of a 'saline' solution which has a concentration of 0.9 %w/v. - 1.8 g
- 180 g
- 4.5 g

The concentration of a solution is known to be 3.2 ppm. What mass (in g) of solute will there be in each millilitre (mL or cm ^{3}) of solution?- 3.2 × 10
^{-3 }g in each mL - 3.2 × 10
^{-6 }g in each mL - 3.2 × 10
^{-9 }g in each mL

- 3.2 × 10