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MCAT Gen. Chem Ch. 9
Term | Definition |
---|---|
Solutions: | Homogenous mixtures composed of two or more substances |
Solvent Particles Surround Solute Particles Via: | Electrostatic interactions in a process called solvation |
Hydration: | Solvation in water |
Solubility: Max amount of solute that can be dissolved in a given solvent at a given temp. | Max amount of solute that can be dissolved in a given solvent at a given temp. |
Molar Solubility: | The molarity of the solute at saturation |
Complex Ions / Coordination Compounds: | Composed of metallic ions bound to various neutral compounds and anions referred to as Ligands |
Formation Of Complex Ions Increases The Solubility Of: | Otherwise insoluble ions (opp of common ion effect) |
Process Of Forming A Complex Ion Involves: | Electron pair donors and electron pair acceptors such as those seen in coordinate covalent bonding |
Normality (Number of equivalents per liters of solution): | Molarity of the species of interest and is used for acid-base and oxidation-reduction reactions |
Solubility Product Constant, Ksp: | The equilibrium constant for a dissolution reaction. |
Comparison Of The Ion Product (IP) To Ksp Determines: | The level of saturation and behavior of the solution |
IP < Ksp: | The solution is unsaturated and if more solute is added, it will dissolve |
IP = Ksp: | The solution is saturated at equilibrium, and there will be no change in concentrations |
IP > Ksp: | The solution is supersaturated and a precipitate will form |
Formation / Stability Constant (Kt): | Equilibrium constant for complex formation. Its value is much greater than Ksp. |
Formation Of A Complex Increases The Solubility Of Other Salts Containing The Same Ions Because: | It uses up the products of these dissolution reactions, shifting the equilibrium to the right (opp of the common ion effect) |
Common Ion Effect: | Decreases the solubility of a compound in a solution that already contains one of the ions in the compound. The presence of that ion in solution shifts the dissolution reaction to the left, decreasing its dissociation. |
Colligative Properties: | Physical properties of solutions that depend on the conc. of dissolved particles but not on their chemical identity. |
Vapor Pressure Depressure Follows: | Raoult's Law |
Raoult's Law (First Part): | The presence of other solutes decreases the evaporation rate of a solvent without affecting its condensation rate, thus decreasing its vapor pressure. |
Raoult's Law (Second Part): | Vapor pressure depression also explains boiling point elevation: As the vapor pressure decreases, the temperature required to boil the liquid must be raised. |
Freezing Point Depression / Boiling Point Elevation: | Shifts in the phase equilibria dependent on the molality of the solution |
Osmotic Pressure: | Dependent on the molarity of the solution |
Van't Hoff Factor (i): | Used for solutes that dissociate in freezing point depression, boiling point elevation, and osmotic pressure calculations. |
Eq. 9.1: Percent Composition By Mass: | Mass of solute / Mass of solution * 100% |
Eq. 9.2: Mole Fraction: | XA = moles of A / total moles of all species |
Eq. 9.3: Molarity: | M = moles of solute / liters of solution |
Eq. 9.4: Molality: | m = moles of solute / kilograms of solvent |
Eq. 9.5: Dilution Formula: | MiVi = MfVf |
Eq. 9.6: Solubility Product Constant: | Ksp = [A^n+]^m*[B^m-]^n |
Eq. 9.7: Ion Product: | IP = [A^n+]^m*[B^m-]^n |
Eq. 9.8: Raoult's Law (Vapor Pressure Depression): | PA = XA*PA^0 |
Eq. 9.9: Boiling Point Elevation: | ΔTb = i*Kb*m |
Eq. 9.10: Freezing Point Depression: | ΔTf = i*Kf*m |
Eq. 9.11: Osmotic Pressure: | II = iMRT. II = Osmotic pressure. i = van't Hoff factor. M = Molarity of solution. R = ideal gas constant, 8.314 J/K*mol.T = temp. |