Chemistry Chapter 9: Solutions (4 Stars) Flashcards
______ are homogenous mixtures composed of two or more substances.
Solutions
Solutions combine to form a single phase, generally the _____ phase.
liquid
Solvent particles surround solute particles via ______ interactions in a process called solvation or dissolution.
electrostatic
Aqueous solutions are most important for the MCAT; solvation in water can also be called ______
hydration.
Most dissolutions are ______, although the dissolution of gas into liquid is ______
endothermic
exothermic.
_______ is the maximum amount of a solute that can be dissolved in a given solvent at a given temperature; it is often expressed as molar solubility—the molarity of the solute at saturation.
Solubility
Complex ions or coordination compounds are composed of metallic ions bonded to various neutral compounds and anions, referred to as _______
ligands.
Formation of complex ions increases the _____ of otherwise insoluble ions (the opposite of the common ion effect).
solubility
The process of forming a complex ion involves electron pair donors and electron pair acceptors such as those seen in __________ bonding.
coordinate covalent
Percent composition by mass (mass of solute per mass of solution times 100%) is used for ______ solutions and solid-in-solid solutions.
aqueous
The mole fraction (moles of solute per total moles) is used for calculating vapor pressure depression and _______ of gases in a system.
partial pressures
______ (moles of solute per liters of solution) is the most common unit for concentration and is used for rate laws, the law of mass action, osmotic pressure, pH and pOH, and the Nernst equation.
Molarity
_____ (moles of solute per kilograms of solvent) is used for boiling point elevation and freezing point depression.
Molality
_______ (number of equivalents per liters of solution) is the molarity of the species of interest and is used for acid–base and oxidation–reduction reactions.
Normality
______ solutions are in equilibrium at that particular temperature.
Saturated
The solubility product constant (Ksp) is simply the equilibrium constant for a _____ reaction.
dissociation
Comparison of the ion product (IP) to ____ determines the level of saturation and behavior of the solution:
Ksp
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 ____ change in concentrations
no
IP > Ksp: the solution is supersaturated, and a _____ will form
precipitate
Formation of a complex ion in solution greatly ______ solubility.
increases
The formation or stability constant (Kf ) is the equilibrium constant for complex formation. Its value is usually much _____ than Ksp.
greater
The formation of a complex _____ the solubility of other salts containing the same ions because it uses up the products of those dissolution reactions, shifting the equilibrium to the right (the opposite of the common ion effect).
increases
The _______ 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.
common ion
______ properties are physical properties of solutions that depend on the concentration of dissolved particles but not on their chemical identity.
Colligative
_____ pressure depression follows Raoult’s law.
Vapor
The presence of other solutes ______ the evaporation rate of a solvent without affecting its condensation rate, thus decreasing its vapor pressure.
decreases
____ pressure depression also explains boiling point elevation—as the vapor pressure decreases, the temperature (energy) required to boil the liquid must be raised.
Vapor
Freezing point depression and boiling point elevation are ____ in the phase equilibria dependent on the molality of the solution.
shifts
_____ pressure is primarily dependent on the molarity of the solution.
Osmotic
For _____ that dissociate, the van ’t Hoff factor (i) is used in freezing point depression, boiling point elevation, and osmotic pressure calculations.
solutes