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It is usually indicated by the Greek symbol α. More accurately, degree of dissociation refers to the amount of solute dissociated into ions or radicals per mole. In case of very strong acids and bases, degree of dissociation will be close to 1. Less powerful acids and bases will have lesser degree of dissociation.
The degree of dissociation is the fraction of the original solute molecules that have dissociated. It is usually indicated by the Greek symbol α {\displaystyle \alpha } . There is a simple relationship between this parameter and the van 't Hoff factor.
Thus, the degree of dissociation of a weak electrolyte is proportional to the inverse square root of the concentration, or the square root of the dilution. The concentration of any one ionic species is given by the root of the product of the dissociation constant and the concentration of the electrolyte.
With the formula below, freezing-point depression can be used to measure the degree of dissociation or the molar mass of the solute. This kind of measurement is called cryoscopy (Greek cryo = cold, scopos = observe; "observe the cold" [7]) and relies on exact measurement of the freezing point.
The degree of dissociation α (also known as degree of ionization), is a way of representing the strength of an acid. It is defined as the ratio of the number of ionized molecules and the number of molecules dissolved in water.
The general formula for such (non-cyclic) polyphosphate anions, linear or branched, is [H n+2−k P n O 3n+1] k−, where the charge k may vary from 1 to n + 2. Generally in an aqueous solution, the degree or percentage of dissociation depends on the pH of the solution.
Complete dissociation. Ion association may take place, particularly with ions of higher charge. This was followed up in detail by Niels Bjerrum. The Bjerrum length is the separation at which the electrostatic interaction between two ions is comparable in magnitude to k B T. Weak electrolytes. A weak electrolyte is one that is not fully dissociated.
Acid strength is the tendency of an acid, symbolised by the chemical formula, to dissociate into a proton, +, and an anion, .The dissociation or ionization of a strong acid in solution is effectively complete, except in its most concentrated solutions.