1. Solubility Chapter 2 Ms. Mishriky & M. Moscoso

2. A solution is a mixture Review: Separation Techniques of Mixtures – Decantation – Magnetism – Evaporation – Distillation – Filtration – Sieving – Sedimentation – Hand removal

3. Solutions Definition: Definition: a solution is a homogeneous mixture whose component substances cannot be distinguished, even with the aid of a magnifying instrument. - can be solid, liquid or gas. The component substances are called solvent and solute. The solute is dissolved in the solvent. Solute molecules fit into “holes” of solvent. Aqueous solution: solution in which the solvent is water.

4. Solutions An aqueous solution is a solution in which the solvent is water. It is the polarity of the water molecule that makes it capable of dissolving a great number of substances. In general, water dissolves molecules made up of ionic bonds (like salt) and those that have a certain polarity (like sugar). Conversely, non-polar molecules are not very soluble in water.

5. How does that work?

6. Properties of Solutions Solubility Concentration Electrical conductivity pH

7. Solubility Solubility: it is the maximum amount of solute that can be dissolved in a certain amount of solvent, at a certain temperature. “Like dissolves like”: A solution forms when the attractive forces between the solute and the solvent are similar (polar & polar, non-polar with non-polar). – Solubility in water: solutes that are polar (Na + Cl - ) dissolve best in water. Solutes that are non polar (oil) almost never dissolve in water. – http://www.mhhe.com/physsci/chemistry/essentialchemistry/fl ash/molvie1.swf http://www.mhhe.com/physsci/chemistry/essentialchemistry/fl ash/molvie1.swf

8. Factors that influence solubility Nature of the solute Nature of the solvent Pressure (gas solutes) Temperature Solubility is expressed in mg/L.

9. Saturation of solutions Saturation: saturation is the point at which a solvent can dissolve no more of a solute and additional amounts of solute will appear as a precipitate. 36 grams of salt is fully saturated in 100 ml of water.

10. 36.0 Supersaturated solution

11. Undersaturation: is a state of a solvent that is capable of dissolving more solute (under certain conditions). Saturation: saturation is the point at which a solvent can dissolve no more of a solute and additional amounts of solute will appear as a precipitate. Supersaturation: To cause a solution to have more solute dissolved in the solvent than it can stably contain (under certain conditions).