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II III I II. The Nature of Solutions Ch. 13 – Liquids & Solids
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A. Solutions MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous MixtureCompoundElement MIXTUREPURE SUBSTANCE yesno Can it be chemically decomposed? noyes Is the composition uniform? noyes ColloidsSuspensions
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Separating Mixtures: 1.Evaporation 2.Filtration 3.Decanting 4.Centrifuge – spins rapidly and separates liquids with different densities 5.Chromatography – (color) separates dyes in ink 6.Distillation - separates liquids with different boiling points using vaporization & condensation
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A. Solutions Solution Homogeneous mixture very small particles no Tyndall effect Tyndall Effect particles don’t settle EX: salt water, hydrogen peroxide, 3 M (molar) HCl
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A. Definitions Solution: Solvent Solvent - present in greater amount- does the dissolving Solute Solute - substance being dissolved
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A. Definitions Types of solutions: Solid Solutions: gold jewelry (gold + copper, 18k (karot) is 18/24=75% gold); alloy- brass (copper + zinc) Gas Solutions: air (78% nitrogen, 21% oxygen, <1% argon and neon) Liquid Solutions: oxygen dissolved in lakes; soda pop-CO 2 in water
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A. Definitions Aqueous Solutions: water is the solvent (universal solvent) Salt + water Sugar + water 3% Hydrogen Peroxide NaOH (aq)
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B. Solvation Solvation the process of dissolving Increase rate by 3 things: stirring, increase temp. of solvent, smaller particle size. solute particles are separated and pulled into solution solute particles are surrounded by solvent particles
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B. Solvation 1. Dissociation separation of an ionic solid into aqueous ions NaCl(s) Na + (aq) + Cl – (aq) MgCl 2 (s) Mg +2 (aq) + 2Cl - (aq)
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B. Solvation 2. Ionization breaking apart of some polar molecules into aqueous ions HNO 3 (aq) + H 2 O(l) H 3 O + (aq) + NO 3 – (aq) (nitric acid)
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B. Solvation 3. Molecular Solvation Molecules Covalently bonded stay intact C 6 H 12 O 6 (s) C 6 H 12 O 6 (aq) (glucose, sugar)
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B. Solvation Strong Electrolyte Non- Electrolyte solute exists as ions only - + salt - + sugar solute exists as molecules only - + acetic acid Weak Electrolyte solute exists as ions and molecules
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B. Solvation NONPOLAR + NONPOLAR POLAR + POLAR Detergents - exception polar “head” with long nonpolar “tail” can dissolve nonpolar grease in polar water “Like Dissolves Like”
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C. Solubility Solubility maximum grams of solute that will dissolve in 100 g of solvent at a given temperature and pressure varies with temp. and pressure based on a saturated solution - (maximum of solute has been dissolved)
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C. Solubility Polar Substances Water Salt (ionic solids) ammonia Vinegar (acetic acid) Rubbing alcohol (isopropyl) acetone Nonpolar substance Vegetable oil Waxes Petroleum oil Gasoline Carbon tetrachloride Hexane
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C. Solubility SolutePolar Solvent Nonpolar solvent PolarSoluble (will mix together) insoluble NonpolarInsoluble- (Not Soluble) soluble Ionicsolubleinsoluble
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C. Solubility SATURATED SOLUTION no more solute can dissolve UNSATURATED SOLUTION more solute can dissolve SUPERSATURATED SOLUTION becomes unstable, crystals form concentration
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C. Solubility Solubility Curve shows the dependence of solubility on temperature
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C. Solubility Solids are more soluble at... high temperatures. Gases are more soluble at... low temperatures. high pressures EX: nitrogen narcosis, the “bends,” soda
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