Chapter 11 Solutions and Colloids
Chapter 11 Key Terms
solid mixture of a metallic element and one or more additional elements
molecules possessing both hydrophobic (nonpolar) and a hydrophilic (polar) parts
elevation of the boiling point of a liquid by addition of a solute
boiling point elevation constant
the proportionality constant in the equation relating boiling point elevation to solute molality; also known as the ebullioscopic constant
property of a solution that depends only on the concentration of a solute species
(also, colloidal dispersion) mixture in which relatively large solid or liquid particles are dispersed uniformly throughout a gas, liquid, or solid
process whereby biological cells become shriveled due to loss of water by osmosis
substance present as relatively large solid or liquid particles in a colloid
solid, liquid, or gas in which colloidal particles are dispersed
physical process accompanying the dissolution of an ionic compound in which the compound’s constituent ions are solvated and dispersed throughout the solution
substance that produces ions when dissolved in water
amphiphilic substance used to stabilize the particles of some emulsions
colloid formed from immiscible liquids
lowering of the freezing point of a liquid by addition of a solute
freezing point depression constant
(also, cryoscopic constant) proportionality constant in the equation relating freezing point depression to solute molality
colloidal dispersion of a liquid in a solid
rupture of red blood cells due to the accumulation of excess water by osmosis
the proportional relationship between the concentration of dissolved gas in a solution and the partial pressure of the gas in contact with the solution
of greater osmotic pressure
of less osmotic pressure
solution that forms with no accompanying energy change
of negligible mutual solubility; typically refers to liquid substances
solvated anion/cation pair held together by moderate electrostatic attraction
electrostatic attraction between an ion and a polar molecule
of equal osmotic pressure
mutually soluble in all proportions; typically refers to liquid substances
a concentration unit defined as the ratio of the numbers of moles of solute to the mass of the solvent in kilograms
substance that does not produce ions when dissolved in water
diffusion of solvent molecules through a semipermeable membrane
opposing pressure required to prevent bulk transfer of solvent molecules through a semipermeable membrane
of moderate mutual solubility; typically refers to liquid substances
the relationship between a solution’s vapor pressure and the vapor pressures and concentrations of its components
of concentration equal to solubility; containing the maximum concentration of solute possible for a given temperature and pressure
a membrane that selectively permits passage of certain ions or molecules
extent to which a solute may be dissolved in water, or any solvent
exothermic process in which intermolecular attractive forces between the solute and solvent in a solution are established
physical or chemical change that occurs without the addition of energy from an external source
substance that dissociates or ionizes completely when dissolved in water
of concentration that exceeds solubility; a nonequilibrium state
heterogeneous mixture in which relatively large component particles are temporarily dispersed but settle out over time
scattering of visible light by a colloidal dispersion
of concentration less than solubility
the ratio of the number of moles of particles in a solution to the number of moles of formula units dissolved in the solution
substance that ionizes only partially when dissolved in water