Solutions Chapters 13 and 14

Solutions Solution Homogeneous mixture All looks the same Solute Being dissolved Solvent Doing the dissolving end

Solutions Polar Molecule: Do not share equally… Negative and Positive side Water (H2O) end

Solutions Nonpolar Molecule : Share equally No charge Carbon Dioxide (CO2) end

Solutions Polar Molecules ONLY dissolve Polar Molecules “Like Dissolves Like” Oil and Water don’t mix! Pen stains do not wash off with water end

Solutions Ionic Compounds Mixed with Water = Dissociation Cations and Anions separate and are surrounded by water NaCl(s) + H2O(l)  Na+(aq) + Cl-(aq) end

Solutions Molecular Compounds Mix with Water = Dispersion Each molecule surrounded by water C12H22O11(s) + H2O(l)  C12H22O11(aq) end

Solutions Acids Mix with Water = Ionization Create into H+ and anions HCl(g) + H2O(l)  H+(aq) + Cl-(aq) end

Properties of Solutions Solids/Liquids dissolve faster by: Add more solvent Increase surface area Grind solid into a powder Stir Increase Temperature Gases dissolve faster by: Decreasing Temperature Increasing Pressure end

Properties of Solutions Conductivity Ionic Compounds(aq) and Acids(aq) conduct electricity Electrolytes Covalent Molecules will NEVER conduct electricity Nonelectrolytes Pure water WILL NOT conduct electricity end

Pure Water= No Electricity Pure NaCl= No Electricity Water + NaCl= end

Properties of Solutions Electrolytes Conduct when dissolved Strong Electrolyte Completely Dissolves into IONS Weak Electrolyte Small Amount Dissolves into IONS Nonelectrolyte Does NOT Dissolve into IONS end

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Colligative Properties Vapor Pressure Amount of liquid particles that become a gas More Ions = Lower end

Colligative Properties B/c the V.P. changes… Freezing Point More Ions = Lower Salt put on icy roads Boiling Point More Ions = Higher Radiators have ethylene glycol dissolved in water end

Determining Solubility of a Substance Solubility Curve

Solubility Solubility Particles more attracted to solvent than each other Measured in: Changes with temperature At 50 °C, the solubility of KNO3 is 80 g. Can dissolve up to 80 g of KNO3 in 100 g of water end

Solubility Solubility Curve Solubility at different temps. What is the solubility of NH3 at 10 °C? ~ ___ g of NH3 / 100 g of H2O 60 g of NH4Cl can be dissolved in 100 g of water at what temperature? ___ °C How many grams of KClO3 can be dissolved in 200 g of water at 30 °C ~ 22 °C end

Solubility The amount of solute determines how a solution is classified: Unsaturated Saturated Supersaturated end

Solubility Unsaturated Solutions Can dissolve more solute BELOW the Line 60 g of KNO3 are dissolved in 100 g of water at 50 °C? Unsaturated Solution of KNO3 end

Solubility Saturated Solution Cannot dissolve any more ON the Line 80 g of KNO3 are dissolved in 100 g of water at 50 °C? Saturated Solution of KNO3 end

Solubility Supersaturated Solution Supersaturated Solution of KNO3 Supersaturated Solution Dissolved more than normally possible ABOVE the Line 130 g of KNO3 are dissolved in 100 g of H2O at 50 °C? end

Concentrations Concentration The amount of solute in a given amount of solvent Concentrated lots of solute Dilute little solute end

Concentrations Molarity (M) You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution contain? end

Concentrations You have 3.50 L of solution that contains 90.0 g of sodium chloride, NaCl. What is the molarity? end

Concentrations You need 23.4 g of potassium chromate in solution for a reaction. If you have a 6.0 M K2CrO4, what volume is needed for the reaction? end