Chemistry 112 - Study Guide - Test 1

Chemistry 112 - Study Guide - Test 1 - Chemistry 112 Exam 1...

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Chemistry 112 Exam 1 Review Sheet CHAPTER 12 Types of a Solution: - Gaseous - Liquid: rates of chemical reaction increase with the likelihood of collisions increasing. - Solid: Substitutional and interstitial. Solvent: The dissolving medium. Solute: The dissolving substance. Saturated: no more solute can be added to the solvent regularly. Supersaturated: By allowing for a raise in temperature, more of the solute can dissolve even if it’s already saturated. Solubility: Non-polar solutes interact with non-polar solvents because of LONDON FORCES and they are also temperature dependent. >> Pressure<< - Gas in a liquid is directly proportional to the partial pressure of the gas. o Henry’s law: S= K H P >>Temperature<< - For gases dissolved in liquid Temp increases and solubility decreases. - For solids dissolved in liquid Temp increases and solubility increases. Concentrations: Molarity (M) = moles/liters Molality ( m ) = moles solute/ kg solvent Mass Percent = (mass of solute/ mass solution) X 100 Mole Fraction = moles of substance A/ total moles Q: How do you prepare 72.5g of an aqueous solution that is .500% KI? A: 72.5 X .05 = 3.62g (KI) 72.5g-3.62g = 68.875 (H 2 O) Colligative Properties - Raoult’s Law: P solution = (mole fraction of solvent) x (Vapor pressure of pure solvent) - Boiling point elevation: ∆ T B = K B x Cm - Freezing point depression: ∆ T F = k f x Cm - Osmotic Pressure : TT = MRT or nRT/V
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Chemistry 112 - Study Guide - Test 1 - Chemistry 112 Exam 1...

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