Nature of Solutions.

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Presentation transcript:

Nature of Solutions

Parts of a Solution Solvent: dissolving medium water Solute: dissolved particles Solvent and Solute particles can be solid, liquid, or gas

Electrolytes and Nonelectrolytes Electrolytes: conducts electrical current Ionic compounds Separate in solution NaCl  Na+ + Cl- Nonelectrolytes: don’t conduct electrical current Molecular compounds Sugar and alcohol

Electrolytes Strong Electrolyte: ~ all separate into ions Good conductor of electricity NaCl Weak Electrolytes: only a fraction separate into ions Poor conductor of electricity HgCl2

Types of Solution Hydrate: compound that contains water molecules CuSO4 ·H2O Deliquescent Compounds: remove water from the air Silica gel used in packaging NaOH (lye)

Heterogeneous Mixtures Suspension: contains larger particles that don’t stay suspended forever > 1000 nm Muddy Water Colloids: particle larger than solution and smaller than suspension 1 nm to 1000 nm Whipped cream, blood

Tyndall Effect Passing a beam of light through a liquid Passes clear through a solution Cloudy through colloid and suspension Particles scatter the light

Solvation Solvation: formation of a solution Rate Affected By: Agitation (stirring) Increases rate Temperature Hi Temp  Hi KE Inc Collision of Particles  increase rate Surface Area of the solute particles Inc surface area  Inc Collisions  Inc rate

Solubility Solubility: amount of solute that will dissolves in a given quantity of solvent at specific temperature and pressure g of solute/100g of solvent g/L Unsaturated S0lution: contains less than the maximum amount of solute Saturated Solution: contains the maximum amount solute

Solubility Supersaturated solution: contains more solute than is can theoretically hold at a given temperature Crystals form

Solubility Miscible: two liquids that dissolve in each other in all proportions Alc0hol and Water Immiscible: liquids that are insoluble Oil and vinegar Like dissolves Like Polar and Polar Nonpolar and nonpolar

Factors Affecting Solubility Temperature and Pressure affect Solubility Solubility Increases with Temperature Pressure: gas solubility increases as the partial pressure of the gas above the solution increase Carbonated beverages Henry’s Law:

Solubility Curves

Henry’s Law If the solubility of a gas in water is 0.77 g/L at 3.5 atm of pressure, what is its solubility at 1.0 atm of pressure? P1 = 3.5 atm S1 = 0.77 g/L P2 = 1.0 atm S2 = ?