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Solution Homogeneous mixture in a single phase.
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Classification of Matter Matter Pure Substances ElementsCompounds Mixtures Homogeneous Mixtures Heterogeneous Mixtures Also called solutions Also called suspensions
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Solvent Substance you have the most of. Substance that retains its phase. Dispersing medium.
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Solute Substance you have the least of. Substance that dissolves.
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Dilute Solution Relatively small amount of solute.
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Concentrated Solution Relatively large amount of solute.
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Aqueous Solution Water is the solvent.
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NaCl(aq) Solution of NaCl dissolved in water!
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Soluble Capable of being dissolved.
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Solubility Maximum amount of 1 substance that will dissolve in a given amount of another substance.
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Factors that influence solubility Temperature for all systems & pressure for systems involving gases.
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Factors that influence the rate of dissolving. TemperatureTemperature Stirring or agitationStirring or agitation Surface Area of soluteSurface Area of solute Amount of solute already presentAmount of solute already present
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What kind of change is dissolving? Physical change
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How does a chemist represent the dissolving of a covalently bonded substance? C 6 H 12 O 6 (s) C 6 H 12 O 6 (aq)
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How does a chemist represent the dissolving of an ionically bonded substance? NaCl(s) Na +1 (aq) + Cl -1 (aq)
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What happens to an ionic substance when it dissolves? It separates into ions.
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What is the equation for the dissolving of CaBr 2 ? CaBr 2 (s) Ca +2 (aq) + 2Br -1 (aq)
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Molecule-Ion Attraction Interaction between water molecules and ions in solution.
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What kind of molecule is H 2 O? Polar – the O end is a bit negative & the H’s are a bit positive.
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Is the orange ion positive or negative & how do you know?
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Units of Solubility? Grams of solute per 100 grams of solvent
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What happens to the solubility of all gases as the temperature increases? The solubility of gases as the temperature
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What happens to the solubility of most solids as the temperature increases? The solubility of most solids as the temperature .
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What do you need to conduct electricity? Mobile charged particles!
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Electrolyte? A substance that dissolves in water to produce a solution that conducts an electric current!
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Nonelectrolyte? A substance that dissolves in water to produce a solution that does not conduct an electric current!
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Saturated solution Contains the maximum amount of dissolved solute at that temperature.
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Supersaturated solution Contains more than the maximum amount of dissolved solute at that temperature.
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Unsaturated solution Contains less than the maximum amount of dissolved solute at that temperature.
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Precipitation The opposite of dissolving. A solid comes out of solution.
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Dynamic Equilibrium Term used to describe a saturated solution. Precipitation & dissolving are ocurring at the same rates. No net change.
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How do you test a solution for saturation? Throw a crystal of the solute into the solution & observe what happens.
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What are 3 possible outcomes of the saturation test? Crystal dissolves – Soln was unsaturated.Crystal dissolves – Soln was unsaturated. No change in crystal – Soln was saturated.No change in crystal – Soln was saturated. Crystal gets larger – Soln was supersaturated.Crystal gets larger – Soln was supersaturated.
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What are 3 regions of a solubility curve? On the trace – saturated solution.On the trace – saturated solution. Above the trace – supersaturated solution.Above the trace – supersaturated solution. Below the trace – unsaturated solution.Below the trace – unsaturated solution.
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Concentration A number that describes how much solute compared to how much solution or how much solvent.A number that describes how much solute compared to how much solution or how much solvent.
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Percent Part over Whole X 100%
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Molarity (M) Molarity = # moles solute Liters of solution
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No. of Particles No. of Moles No. of Grams No. of Liters X formula mass X 22.4 L/mol X 6.02 X 10 23 by F.M. by 6.02 X 10 23 by 22.4 Mole Map
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Parts per Million (PPM) PPM = grams solute X 1000000 grams solution
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How much KCl will dissolve in 300 grams of water at 50 C? Use the graph to set up a proportion. Problem: 42 g KCl = X g KCl 100 g H 2 O300 g H 2 O X = 126 g KCl
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88 g KNO 3 in 100 g H2O at 50 C. 20 g KNO 3 in 100 g H 2 O at 10 C. 88 g – 20 g = 68 g KNO 3 precipitates. 50 to 10 - How much KNO 3 precipitates?
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source Measuring Heat of Solution If Temperature of H 2 O , dissolving was exothermic. If temperature of H 2 O , dissolving was endothermic.
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Factors affecting Solubility TemperatureTemperature PressurePressure Nature of the Solvent & SoluteNature of the Solvent & Solute
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Nature? IonicIonic Polar CovalentPolar Covalent Nonpolar CovalentNonpolar Covalent “Like Dissolves Like”
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Nature of Solute Nonpolar Solvent Polar Solvent NonpolarSolubleInsoluble PolarInsolubleSoluble IonicInsolubleSoluble
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Molarity C X Volume C = Molarity D X Volume D M C X V C = M D X V D Dilution Problems
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Colligative Property Depends on the concentration of the solute, NOT on the nature of the solute. Does not matter if ions or neutral particles are in solution.
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What are 2 colligative properties? Freezing Point Depression & Boiling Point Elevation
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Which solution has the most dissolved particles? a)1 mole of C 6 H 12 O 6 in 1 Liter H 2 O b)1 mole of NaCl in 1 Liter H 2 O c)1 mole of CaBr 2 in 1 Liter H 2 O
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