8.1 Solutions and Other Mixtures Heterogenous Mixtures Does not have a fixed composition Each substance varies in amount Suspension - solid/liquid mixture where particles are large and settle out over time. (Italian salad dressing) Particles may be filtered out; bacteria, 1000nm Some liquid/liquid mixtures will settle out Immiscible liquids completely separate; Italian dressing Decanting – pouring a less dense liquid off a denser liquid; gravy from fats Particles in a Colloid are too small to settle out; stay suspended Particles are smaller than suspensions (1-1000nm) Pass through most filters, (latex paint) Particles small enough to scatter light (Tyndall Effect) Common foods; gelatin, egg whites, blood plasma (protein colloid) whipped cream and marshmallows, Fog/Smoke *Some immiscible liquids can form colloids Emulsions – liquid mixtures of two immiscible liquids held together by a protein(in eggs) binder, Oil/vinegar with egg white = Mayonnaise Homogenous Mixture Solutions - particles are evenly dispersed Solute is the substance being dissolved Solvent is the substance doing the dissolving Miscible liquids mix to form solutions; vinegar and water Liquid solutions sometimes contain no water Petroleum products –gasoline, diesel, kerosene, plastics fingernail polish remover, paint strippers **Other states of matter can also form solutions** o S-L-G combinations are all possible In Solids In Liquids In Gases Solids Metal Alloys(first melted then cooled) Italian Dressing Smoke Liquids amalgam Hg + Ag (second metal also melted first) water/acetic acid oil/vinegar (mayo) chocolate milk Gases Marshmallows Carbonated beverage; Whipped Cream Fog Atmosphere 8.2 How Substances Dissolve Water a Common Solvent – Universal Solvent Water can dissolved ionic compounds (ripping apart) Why??? Polar molecule- describes a molecule in which the positive and negative charges are separated (and those ends attract opposite charge particles) Dissolving depends on the force between the particles; strong bonds, not very soluble; sugar vs salt; Silver Nitrate – too strong to dissolve Water dissolves many molecular compounds (vitamins, sugars) Hydrogen bond is important in dissolving other polar molecular compounds Like dissolves Like- Polar dissolves other Polar compounds The Dissolving Process (think Kinetic Theory) Solutes with a larger surface area dissolve faster Stirring or shaking helps solids dissolve faster Solids dissolve faster when the solvent is hot Solutes affect the physical properties of solutions Boiling point in will increase due to more particles absorbing the thermal energy Freezing point will decrease 8.3 Solubility and Concentration Solubility - the ability of one substance to dissolve in another at a given temperature and pressure Different substances have different solubility’s Due to strength of forces acting between the solute particles and the strength of the force between the water molecules and solute particles How much substance is in a solution? General terms – Strong or weak Dilute – very little solute compared to amount of solvent Concentrated – a lot of solute compared to amount of solvent More specific. Based on ability of substance to dissolve in a given solvent Saturated - maximum about of solute at room temp; cannot dissolve any more; equilibrium Unsaturated – able to dissolve more solute in the solvent without separation occurring Supersaturated – able to “hold” more solute than normal due to heating solvent to increase solubility Concentrations of Solutions Molarity – quantitative measurement expressed as the number of moles of solute per liter of solution M solution is read as “one molar” solution Let practice – Molarity of a 1.0 L solution containing 25 grams of NaCl Number of moles(solute) divided by the liters of solvent used. Solute is NaCl = 58g/mol (23g/mol + 35g/mol) You have 25g of NaCl divide by 58g/mol = .43 moles Then divide moles of solute by liters of solvent .43 moles / 1 liter = .43 molar solution. Easy as that!!