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Solutions and Solubility

Learn about solutions and solubility, including solubility curves, types of solutions, molarity, colligative properties, and more. Understand how temperature, pressure, and nature of solute/solvent affect solubility.

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Solutions and Solubility

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  1. Solutions and Solubility

  2. Solutions • Solution – a homogenous mixture of a solute dissolved in a solvent. The solubility (ability to dissolve) of a solute in a solvent is dependent on the • Temperature For solid solutes: as temperature increases, solubility increases. For gas solutes: as temperature increases, solubility decreases.

  3. Solutions con 2. Pressure For solid solutes: as pressure increases, solubility remains the same. For gas solutes: as pressure increases, solubility increases 3. Nature of Solute/Solvent “Like dissolves in like.”

  4. Solute/Solvents cont. Solubility Summary High solubility-soluble Low solubility-insoluble

  5. Solubility Curves • Shows the number of grams of solute that can be dissolved in 100.g of water at temperatures between 0 degrees C and 100 degrees C. • Each line represents the maximum amount of that substance that can be dissolved at a given temperature. • Lines that show an increase in solubility as temperatures increase represent solids being dissolved in water. • Lines that show a decrease in solubility as temperatures increase represent gases being dissolved in water. These are NH3, SO2, and HCl

  6. There are three types of solutions • 1. An unsaturated solution is a solution in which more solute can be dissolved at a given temperature. • 2. a saturated solution is a solution containing the maximum amount of solute that will dissolve at a given temperature. • 3. a supersaturated solution is a solution that contains more solute than would dissolve in a saturated solution at a given temperature.

  7. Solubility guidelines- reference table F • Recall that double-replacement reactions have the general formula: AB + CD AD +CB A reaction will take place if one or both of the products is listed as insoluble. Include the solubility's of the products. 2AgNO3 + Na2CrO4 Ag2CrO4 + Na NO3

  8. Concentrations of Solutions • Because solutions are homogeneous mixtures, their compositions can vary. Sometimes it is adequate to refer to a solution as dilute or concentrated. These are qualitative descriptions of concentration. It is more precise to describe the concentration of solutions in quantitative measures.

  9. Molarity • Molarity (M)- number of moles of solute in 1L of solution. Table T Molarity= moles of solute liters of solution • Parts per million (ppm)- ratio between the mass of a solute and the total mass of the solution (used for very dilute solutions) Table T ppm= grams of solute X 1,000,000 grams of solution

  10. Colligative Properties Freezing and boiling points of water change when nonvolatile solutes are added. 1. Freezing Point Depression: when any salt is added to water, the freezing point of the water decreases. Freezing point of pure water= 0 degrees C Freezing point of water solution= decreases One mole of any particles will have the same effect on the freezing point of water. One mole of particles lowers the freezing point of 1000g of water by 1.86 degrees C. Adding Salt Simulation

  11. Molecular vs. Ionic • When one mole of sugar is dissolved in water, one mole of particle is produced in solution: C12H22O11(s) C12H22O11(aq) • When one mole of an ionic substance is dissolved in water, the results are different. The ionic substance dissociates into individual ions: NaCl(s) Na(aq) + Cl (aq) • The greater number of ions, the greater the freezing point.

  12. Boiling Point Elevation • When any salt is added to water, the boiling point of the water increases. • Boiling point of pure water= 100 degrees C • Boiling point of water solution= increases • The situation is similar with the boiling point. One mole of particles will elevate the boiling of 1000.g of water by 0.52degrees C.

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