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40 Cards in this Set
- Front
- Back
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Solute
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Smallest amount - dissolved
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Solvent
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Largest amount - does the dissolving
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Soluble / Miscible
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Solute dissolves easily
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Insoluble / Immiscible
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Solute does not dissolve
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Solvation
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Process of surrounding solute particles with solvent particles to form a solution (solvation in water is called hydration)
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What is the Rule of Solubility?
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"Like dissolves like"
-Polar solvent dissolves polar solute -Nonpolar solvent dissolves nonpolar solute |
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What are the factors that affect solvation rate?
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1. agitation
2. increase surface area 3. increase temperature |
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Heat of Solution
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The overall energy change that occurs during the solution formation process
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Solubility
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The maximum amount of solute that will dissolve in a given amount of solvent at a specified temperature and pressure
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What unit is solubility expressed in?
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g solute/100g solvent
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Saturated Solution
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Contains the maximum amount of solute that can dissolve in a given amount of solvent
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Unsaturated Solution
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Contains less solute than what can be dissolved in a given amount of solvent
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Supersaturated Solution
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Contains more dissolved solute than a saturated solution at the same temperature
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What factors affect solubility and how?
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1. temperature - ⬆temp, ⬆solubility, ⬆KE - more collisions
2. pressure - ⬆pressure, ⬆solubility |
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Henry's Law
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S1/P1 = S2/P2
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Concentration
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Measure of how much solute is dissolved in a specific amount of solvent or solution
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Percent by mass
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mass solute/mass solution x 100
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Percent by volume
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volume solute/volume solution x 100
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Molarity
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moles solute/liter solution
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Molality
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moles solute/kilogram solvent
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Mole fraction
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moles solute/moles of solute + moles of solvent
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What is equation for molarity when diluting solutions?
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M1V1 = M2V2
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What is the mole fraction for the solvent?
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moles solvent/moles solvent + moles solute
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What is the mole fraction for the solute?
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moles solute/moles solute + moles solvent
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Colligative Properties
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Physical properties of solutions that are affected by the number of particles but not the identity of dissolved solute particles
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What are the colligative properties?
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1. vapor pressure lowering
2. boiling point elevation 3. freezing point depression 4. osmotic pressure |
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Vapor pressure lowering
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The greater the number of solute particles in a solvent, the lower the resulting vapor pressure
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Boiling point elevation
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The temperature difference between a solution's boiling point and a pure solvent's boiling point
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What is the boiling point constant for water?
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0.512 °C kg/mol
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What is the boiling point equation?
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ΔTb = Kbm
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Freezing point depression
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The difference in temperature between its freezing point and the freezing point of its pure solvent
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What is the freezing point constant for water?
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1.86 °C kg/mol
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What is the freezing point equation?
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ΔTf = Kfm
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Osmosis
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The diffusion of solvent particles across a semipermeable membrane from an area of higher solvent concentration to an area of lower solvent concentration
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Osmotic Pressure
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The amount of additional pressure caused by the water molecules that moved into the solution
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What are the three types of heterogeneous mixtures?
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1. true solution - smallest solute
2. colloids - medium size solute 3. suspension - largest size solute |
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Suspension
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A mixture containing particles that settle out if left undisturbed
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Colloid
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A heterogeneous mixture of intermediate size particles
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Tyndall Effect
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Way to to tell the difference between colloid and true solution. Light cannot be seen in true solution because the solute is too small to scatter light. Light does scatter in colloid because particles big enough..
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Brownian Motion
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The random, constant movement of solvent particles keep solute particles dispersed
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