Concentration of Aqueous Solution (2)

Chemistry

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I easily remember

Unit to measure the quantity of solute dissolved (1)

Gram

Unit to measure the concentration of a solution (1)

g dm–3

The unit for molarity

Is mol dm–3 or molar (M)

Mole

Is the unit for measuring matter

Molar

Is the number of moles of solute in a given volume of solution

Example of calculation of concentration of solution of 40 g of solid copper(II) sulphate, CuSO4 is dissolved in water to produce 20 dm3 solution

Concentration of copper(II) sulphate, CuSO4 = Mass of solute (g)/Volume of solution (dm3) = 40 g/20 dm3 = 2.0 g dm–3

Example of calculation of concentration of solution of 18 g of sodium hydroxide pellets, NaOH is dissolved in water to produce 750 cm3 solution

Concentration of sodium hydroxide, NaOH = Mass of solute (g)/Volume of solution(dm3) = 18 g/0.75 dm3 = 24.0 g dm–3

Example of calculation of molarity of solution of 10 mol of solid zinc chloride, ZnCl2 dissolved in water to produce 5 dm3 of solution

Molarity of zinc chloride solution, ZnCl2 = Number of moles of solute (mol)/Volume of solution(dm3) = 10 mol/5 dm3 = 2.0 mol dm–3

Example of calculation of molarity of solution of 0.1 mol of solid calcium chloride, CaCl2 is dissolved in 500 cm3 of distilled water

Molarity of calcium chloride solution, CaCl2 = Number of moles of solute (mol)/Volume of solution(dm3) = 0.1 mol/0.5 dm3 = 0.2 mol dm–3

Example of calculation of concentration of nitric acid, HNO3 with a molarity of 0.5 mol dm–3 in unit g dm–3

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