ANALYTICAL CHEMISTRY (LECTURE) Flashcards
usually used to express concentration of commercial aqueous reagents
Weight percent
commonly used to specify the concentration of a pure liquid compound diluted with another liquid
Volume percent
used to indicate the concentration of solid reagent in a dilute aqueous solution
weight/volume percent
commonly used in unit operations to express concentrations of solute present in a stream of gas or liquid
Mole fraction (x)
temperature-independent concentration term used conveniently in physiochemical measurements of colligative properties of solutions
molality (m)
most commonly used in titration and denotes the amount of solute, in moles, dissolved in a solvent and diluting to a final volume of 1L in a volumetric flask
Molarity (M)
concentration term identical to molarity commonly used for solutions of ionic salts that do not exist as a molecule in a solid or in solution
formality (F)
once popular unit of concentration still used by some chemists
Normality (N)
weight percent formula
%wt/wt = weight of solute/ weight of solution x 100%
volume percent formula
%vol/vol = volume of solute/ volume of solution x 100%
weight/volume percent formula
%wt/vol = weight of solute (gram)/ volume of solution (mL) X 100%
Mole fraction formula
x = moles of solute/ mole of solute + mole of solvent
molality formula
m = mole of solute / kg of solvent
Molarity formula
M = mole of solute/volume of solution (L)
Normality formula
N = Equivalent of solute (eq)/ volume of solution (L)