COLLIGATIVENATURE SOLUTION

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1 COLLIGATIVENATURE SOLUTION
CLASS XI SEMESTER 1 SMKN 7 BANDUNG

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Colligative nature of the solution is the solution that nature does not depend on the type of solute but solely determined only by the number of solute (solute concentration). When a solvent with little solute, then a solution will be the: 1) Decrease saturated vapor pressure 2) The increase in boiling point 3) A decrease in freezing point 4) The pressure osmosis Hal.: 2 Isi dengan Judul Halaman Terkait

3 Decrease in Saturated Vapor Pressure
The addition of a substance in the liquid causes a decrease in pressure. This is because the dissolved oxygen is reduced or the faction of the solvent, so that the speed of evaporation is reduced (Figure 5.3). Hal.: 3 Isi dengan Judul Halaman Terkait

4 Decrease in Saturated Vapor Pressure
According to Roult: description: p: vapor pressure of saturated solution po: saturated vapor pressure of pure solvent XB: faction mol solvent Hal.: 4 Isi dengan Judul Halaman Terkait

5 Decrease in Saturated Vapor Pressure
Because xa + xb= 1, then the equation above can be expanded to: P = Po (1 - xa) P = Po - Po. Xa Po - P = Po. Xa So that: ΔP = po. Xa description: ΔP: a decrease in saturated solvent vapor pressure po: vapor pressure of pure solvent Xa: faction mol oxygen terlarut Hal.: 5 Isi dengan Judul Halaman Terkait

6 Decrease in Saturated Vapor Pressure
Example: Count decrease saturated water vapor pressure, when 45 grams of glucose (Mr = 180) dissolved in 90 grams of water! Known saturated water vapor pressure 20oC is purely on the 18 mmHg. Hal.: 6 Isi dengan Judul Halaman Terkait

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Answer: mole glucose = mole H2O = mole faction glucose = = Decrease in saturated water vapor pressure: ΔP = Po. Xa = 18 x = 0864 mmHg Hal.: 7 Isi dengan Judul Halaman Terkait

8 Increase in Boiling Point
A decrease in saturated vapor pressure boiling point solvents lead to higher boiling point of pure solvent. Non-electrolyte solution for the increase in boiling point is expressed with: description: ΔTb = increase in boiling point (oC) m = molality solution Kb = constant increase in boiling point molal Hal.: 8 Isi dengan Judul Halaman Terkait

9 Decrease in Freezing Point
To a decrease in freezing point similarity stated as: description: ΔTf = decrease in freezing point m = molality solution KF = constant point reduction molal freezing W = mass substances solute Mr = relative molecular mass substances terlarut p = solvent mass When the solvent is water and 1 atm air pressure, the freezing point of solution expressed as: Tf = (O - ΔTf) oC Hal.: 9 Isi dengan Judul Halaman Terkait

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Osmosis Pressure osmosis pressure is given to the solution that can stop the transfer of molecule-solvent in solution through a semi permeable membrane (osmosis process). According to Van't hoff osmosis pressure following the ideal gas law: PV = nRT Hal.: 10 Isi dengan Judul Halaman Terkait

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Osmosis Pressure Because the pressure osmosis = th description: = osmosis pressure (atmosphere) C = solution concentration (M) R = universal gas constant = L.atm / mol K T = absolute temperature (K) Hal.: 11 Isi dengan Judul Halaman Terkait

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Osmosis Pressure Solvents that have osmosis pressure is lower than the other solvents mentioned Hypotonic. Solvents that have a pressure higher than the other solvents mentioned Hypertonic. Solvents that have the same pressure is called osmosis Isotonic. Hal.: 12 Isi dengan Judul Halaman Terkait