Moles and concentration of solutions

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Moles and concentration of solutions

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Moles and concentration of solutions

  1. 1. Wednesday 12 September 2012
  2. 2. Using the Mole The mole is a conversion factor used in chemistry– this shows you how this is extended.Volume X 24 dm3 X 6 x 1023 Numberof a gas Moles of ÷ 24 dm3 (dm3) ÷ 6 x 1023 particles x formula ÷ mass formula mass Key fact – always Mass (g) multiply when working out of the mole box!
  3. 3. Concentration of a solutionA solution contains dissolved particles (the solute) in a solvent (the liquid).The concentration refers to the amount of dissolved solute in the solution.
  4. 4. More concentrated Less concentrated
  5. 5. Volume of solutionThe volume of a solution is measured in cm3 or dm3.Recall that: 1dm3 = 1000cm3.The volume of a solution is measured using: (a) Measuring cylinder (b) burette (c) pipette (d) standard flask
  6. 6. Formula for concentrationThe formula for concentration is:Concentration = number of moles ÷ volumeConcentration = mass ÷ volumeConcentration can be measured in: (a) moles/dm3 (b) grams/dm3
  7. 7. Calculations using concentration.Recall this triangle: n C V
  8. 8. Example(1) Calculate the concentration of a solution which has 160g of sodium hydroxide (NaOH) in 2dm3 solution.(2) Calculate the number of moles of sodium hydroxide in 500cm3 of the above sodium chloride solution.(3) Calculate the volume of this solution which will contain 0.1 moles of sodium hydroxide.
  9. 9. Diluting solutionsThe rule is: multiply the starting volume by the number of times the solution is to be dilutes and subtract the starting volume.So to dilute 20cm3 of 1mol/dm3 solution to 0.1mol/dm3:Add (1/0.1 x 20) – 20 = 180cm 3 water

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