Acid (aqueous): any species that produces
hydronium ions (H3O+) when dissolved in water, and
are proton donors.
Aliquot a sample, which is a fraction of a larger
known amount.
Analyte the species in the sample where analytical
information is focused.
Aqueous solution a solution in which water is the
solvent.
Base (aqueous): any species
that produces hydroxide ions when dissolved in water, and and are proton
acceptors..
Boiling point elevation the increase in the boiling
point of a solvent caused by the presence of dissolved solute.
Boiling Point The temperature where the vapor pressure
is equal to the external pressure.
Boules: large crystal mass
with the atomic structure of a single crystal used in the NIF; different
parts are used for optical switches or for frequency conversion.
Buffer Capacity a measure of the ability
of a buffer to resist a change in pH that is related to the concentrations
and relative proportions of buffer components.
Buffer range the pH range over which a buffer
acts effectively.
Buffer a solution that resists changes in
pH when a small amount of either strong acid or strong base is added.
Buret a graduated tube, where volumes of liquids maybe
accurately dispensed in titrations.
Clarify To make clear
by removing impurities or solid matter.
Colligative properties properties causing the number
of solute particles make a difference, not their chemical identity. Such
properties include: Vapor pressure lowering, boiling point elevation,
freezing point depression, and osmotic pressure.
Colloids a suspension in which a solute like
phase is being dispersed throughout a solvent like phase. Colloidal
particles in water have charged surfaces that keep them dispersed, but
they can be coagulated by heating or by the addition of ions.
Complex Ion a hydrated metal ion which has several
loosely bonded ionic or neutral species called ligands.
Concentrated Solution is a qualitative term for a
relatively large amount of solute dissolved.
Concentration the proportion of a substance
in a mixture, it is an intensive property, one that does not depend on
the total quantity of the mixture. Often expressed as the ratio of
the quantity of solute to the quantity of solution, sometimes it is the
ratio of solute to solvent. Concentrations may be expressed in a number
of ways. The simplest is in terms of a component's percentage by weight
or volume. Very low concentrations, such as those of various substances
in the atmosphere, are expressed in parts per million (ppm) or parts per
billion (ppb).
Crystalline solids: solids with a well-defined shape
because of the orderly arrangement of their atoms, molecules, or ions.
Crystallization a technique used to separate
and purify the components of a mixture through differences in solubility
in which a component comes out of solution as crystals.
Crystallography the scientific study of crystals dating
back to 18th century beginning with classification of the different geometric
patterns that were observed in crystals found in nature.
Diffusion the process of migration
of one species in high concentration to a lower concentration.
Dilute Solution is a qualitative term for a relatively
small amount of solute dissolved.
Dilution is the process of adding more solvent
to a solution.
Dipole-Dipole Forces important forces in solutions,
a special type of dipole-dipole forces known as the H bond, is a primary
factor in water’s ability to dissolve numerous O-containing and N-containing
organic and biological compounds, such as alkanes, sugars, amines, and
amino acids.
Dipole-induced dipole force a force resulting from
the distortion of the electron cloud of a nearby non-polar molecule by
the partial charges of a polar molecule.
Dispersion Forces principal attractive force in solutions
of non-polar substances; contributing to the solubility of all solutes
in all solvents.
Electrolyte a substance
that dissolves in water into ions which are capable of conducting an electrical
current.
Entropy: A measure of a system’s disorder, one
of the major factors to determine whether a substance dissolves is more
abstract than the change in heat. Entropy increases greatly when
pure substances mix and become dissolved.
Filtrate - Material, liquid,
that has passed through a filter.
Heat of hydration: the enthalpy
change for separating the water molecules (DHsolvent) and mixing the solute
with them (DHmixture). The heat of hydration is a crucial factor
in dissolving an ionic solid.
Heat of solution(D Hsolution): The total enthalpy
change that occurs when a solution forms from solute and solvent.
Henry’s Law: Expresses the quantitative relationship
between gas pressure and solubility: the solubilitty of a gas (S
gas) is directrly proportional to the partial pressure of the gas (P gas)
above the solution.
Homogeneous mixture (solution): a mixture that has
no visible boundaries among its components.
Hydration of an ion: The enthalpy change for the hydration
of 1 mol of separated gaseous ions. Hydration of ions is always an
exothermic process.
Hydration shells: The oriented cluster of water molecules
that surrounds an ion in aqueous solution.
Hydration: Solvation in water.
Ideal solution: a solution
whose vapor pressure equals the mole fraction of the solvent times the
vapor pressure of the pure solvent; approximated only by the very dilute
solutions.
Ion-dipole forces: A principal factor in the solubility
of ionic compounds in water. When a salt dissolves, each ion on the
surface of the crystal attracts the oppositely charged end of the water
dipole.
Ion-induced dipole force: The force resulting from
the distortion of the electron cloud of a nearby non-polar molecule by
an ion’s charge.
Ligand an ionic or neutral
species loosely bonded to a central metal ion.
Like dissolves Like: Substances with similar polarities
which relate to their attractive intermolecular forces dissolve in each
other.
Liquid crystal: is a substance that flows like a liquid
but packs like a crystalline solid at the molecular level.
Mass Percent (weight percent): A
way of describing a solution’s composition, which expresses the mass of
solute present in a given mass of solution; = (mass of solute / mass of
solution) * 100%
Metastable State: a state where a system that is being
perturbed briefly passes before becooming unstable. At this state, the
system may also return to stability when altered slightly. Example: if
water is super-cooled, then disturbed slightly, say by a speck of dust
or by having a single ice crystal put in, the super-cooled water will immediately
become a block of ice.
Miscible: liquids that are soluble in each other in any proportion.
Molality (m): The number of moles of solute dissolved
in 1000g of solvent.
Molar solubility: the solubility expressed in terms
of amount (mol) of dissolved solute.
Molarity (M): is the most commonly used expression
in chemistry of concentration, which describes the amount of solute in
moles and the volume; = moles of solute / liter of solution.
Mole fraction is the ratio of moles of solute
to the total number of moles in the solution.
Morphology - Shape of crystal; e.g., needlelike, hexagonal.
Neutralization reaction: an
acid-base reaction that gives water and a neutral solution of a salt; an
aqueous reaction between a strong acid and a strong base.
Nonelectrolyte: a substance whose aqueous solution
does not conduct an electric current.
Non-Linear crystals: Crystals that are used for harmonic
generation, including frequency doubling (SHG), or tripling (3HG), frequency
mixing, OPO (Optical Parametric Oscillation). eg. ZnGeP2, AgGaSe2, AgGaS2,
GaSe, Tl3AsSe3. They have middle and deep infrared applications
Osmosis: The process by which solvent
flows through a semi-permeable membrane from a dilute to a concentrated
solution.
Parts per million (ppm): number
of any unit present out of one million units.
Parts per billion (ppb): number of any unit present out of one billion
units.
Parts per trillion (ppt): number of any unit present out of one trillion
units.
Percent composition::[parts
by mass -> weight % = Mass of solute/Mass of
solution:x 100]; [parts by volume] -> volume
% = Volume of solute/Volume of solution]
pH: the negative base 10 logarithm of the hydronium ion concentration.
Pipet A tube which transfers known amounts of liquid from
one container to another
Pockels Cell: An electro-optical crystal used as a
Q-switch; part of an optical switch, which changes the frequency of a laser
beam
pOH: the negative logarithm of the hydroxide ion concentration.
Precipitation reaction: a reaction in which two water
soluble ionic compounds form an insoluble product, a precipitate.
Proof equals 2X the volume % of ethanol in alcoholic
beverages.
Qualitative analysis: the separation
and identification of the ions in an aqueous mixture.
Q-Switch: A device that has the effect of a shutter
to control the laser resonator's ability to oscillate. Control allows one
to spoil the resonator's "Q-factor," keeping it low to prevent
lasing action. When a high level of energy is stored, the laser can emit
a very high-peak-power pulse.
Raoult’s Law: States that the vapor
pressure of a solvent above a solution (Psolvent) equals the mole fraction
of a solvent in the solution (Xsolvent) times the vapor pressure of
the pure solvent.
Saturated: A solution
cntaining the maximum amount of dissolved solute at a given temperature.
Selective precipitation: the process of separating
ions through differences in the solubility of their compounds with a given
precipitating ion.
Semipermeable membrane: A membrane that allows
solvent, but not solute to pass through.
Single Crystal: a crystallite that has either been
found in nature, separated from a polycrystalline mass, or deliberately
prepared.
Slurry: A thin mixture of a liquid, especially water, and any of several
finely divided substances, such as cement, plaster of Paris, or clay particles.
Soap: The salt of an acid-base reaction between
a strong base (Metal Hydroxide), and a fatty acid, a molecule with a long
hydrocarbon chain bounded to an organic acid group.
Solubility: The maximum amount of solute that
dissolves in a fixed quantity of a particular solvent at a specified temperature.
Solute: The substance that dissolves in a solvent
in a solution.
Solutions: Homogenous mixtures consisting of
a solute dissolved in a solvent through the influence of intermolecular
forces.
Solvation: The process of surrounding a solute
particle with solvent particles.
Solvent The substance in which the solute dissolves,
which is the most abundant component of a given solution.
Standard Solution: is a solution whose concentration
is accurately known.
Supernatant : The clear fluid above a sediment or
precipitate.
Supersaturated: A solution containing more than
the equilibrium amount of dissolved salute. It is unstable relative
to the saturated solution.
Suspension: A heterogeneous mixture containing
particles large enough to be seen with the naked eye and clearly distinct
from the surrounding fluid.
Thermochemical solution cycle: Combining
the three enthalpy changes (DHsolute, DHsolvent, DHmixture) to find the
heat of solution.
Titration: a method of determining the concentration
of a solution by monitoring its reaction with a solution of known concentration.
Unsaturated: a solution
that has not reached the maximum limit of solute that will dissolve in
it. (and/or) A solution in which more solute can be dissolved at a give
temperature.
Viscosity The measure of resistance
in the flow of a fluid
