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Concentration of solutions (notes p. 27)

Concentration of solutions (notes p. 27). 10 g HCl in 100 cm 3 water 12 g HNO 3 in 100 cm 3 water?. Why of the following solutions is more concentrated?. Ö.

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Concentration of solutions (notes p. 27)

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  1. Concentration of solutions (notes p. 27)

  2. 10 g HCl in 100 cm3 water 12 g HNO3 in 100 cm3 water? Why of the following solutions is more concentrated? Ö

  3. The molarity (or molar concentration) of a solution is the number of moles of solute per dm3 of the solution. The unit of molarity is mol dm–3 or M. Learning tip • Concentration of a solution is the amount of solute in a unit volume of the solution. mole • Amount of substance is expressed in

  4. contains 1 mole of solute per dm3 of solution 1 M (one molar solution)

  5. contains 2 mole of solute per dm3 of solution 2 M (two molar solution) Class practice 15.1

  6. Fig.15.1 The concentrations of aqueous bench reagents are usually stated in terms of molarity.

  7. number of moles of solute (mol) Molarity of solution (mol dm−3) / (M) = It follows that: volume of solution (dm3)

  8. mass of solute (g) Number of moles of solute (mol) = molar mass of solute (g mol−1) number of moles of solute (mol) Molarity of a solution (mol dm−3) / (M) = volume of solution (dm3) The two formula:

  9. Class practice 15.3 Class practice 15.4 Class practice 15.5 Class practice 15.6 Class practice 15.7 • In the laboratory, the concentration of aqueous reagents is usually stated in molarity (mol dm–3), rather than in g dm–3. Do Q. 34, 33

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