COLLIGATIVENATURE SOLUTION CLASS XI SEMESTER 1 SMKN 7 BANDUNG

Isi dengan Judul Halaman Terkait 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

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

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

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

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

Isi dengan Judul Halaman Terkait Answer: mole glucose = mole H2O = mole faction glucose = = Decrease in saturated water vapor pressure: ΔP = Po. Xa = 18 x 0048 = 0864 mmHg Hal.: 7 Isi dengan Judul Halaman Terkait

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

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

Isi dengan Judul Halaman Terkait 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

Isi dengan Judul Halaman Terkait Osmosis Pressure Because the pressure osmosis = th description: = osmosis pressure (atmosphere) C = solution concentration (M) R = universal gas constant = 0.082 L.atm / mol K T = absolute temperature (K) Hal.: 11 Isi dengan Judul Halaman Terkait

Isi dengan Judul Halaman Terkait 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