dissolution

(noun)

Dissolving, or going into solution.

Related Terms

Examples of dissolution in the following topics:

  • Intermolecular Forces and Solutions

    • The nature of the solute (X) and solvent (Y) determines whether dissolution is energetically favorable or unfavorable.
    • On the other hand, dissolution is favorable when solute-solvent bonds (X-Y) are stronger than X-X or Y-Y bonds.
    • After dissolution occurs, solvation follows.
    • If solvation releases more energy than is consumed during dissolute, then solution formation is favored and the solute is soluble in the solvent.
    • Consider the dissolution of table salt (sodium chloride) in water:

  • Heat of Solution

    • The heat of solution, also referred to the enthalpy of solution or enthalpy of dissolution, is the enthalpy change associated with the dissolution of a solute in a solvent at constant pressure, resulting in infinite dilution.
    • Dissolution of sodium chloride (table salt) in water is endothermic.
    • Dissolution of sodium chloride in water is endothermic.

  • Solutions and Heats of Hydration

    • Solubility depends on dissolution of the solute into the solvent and, like all chemical reactions, is governed by the laws of thermodynamics.
    • The dissolution of an ionic solid MX in water can be thought of as a sequence of two processes:
    • As often happens for a quantity that is the sum of two large terms having opposite signs, the overall dissolution process can be either endothermic or exothermic.

  • Solutions and Entropy Changes

    • Consider, the dissolution of sodium sulfate,
    • If the energetics of dissolution are favorable, this increase in entropy means that the conditions for solubility will always be met.
    • Recall that entropy favors dissolution because the potential for randomness is increased

  • Solid Solubility and Temperature

    • This temperature dependence is sometimes referred to as retrograde or inverse solubility, and exists when a salt's dissolution is exothermic; this can be explained because, according to Le Chatelier's principle, extra heat will cause the equilibrium for an exothermic process to shift towards the reactants.

  • Metallurgy

    • In order to dissolve an ore in an aqueous solution, it is often necessary to break the large chunks into smaller pieces, thereby increasing the surface area and the rate of dissolution.
    • The most common hydrometallurgical process is leaching, which involves the dissolution of the valuable metals into the aqueous solution.

  • The Common Ion Effect

    • For a simple dissolution process, the addition of more of one of the ions (A+) from another compound will shift the composition to the left, reducing the concentration of the other ion (B-), effectively reducing the solubility of the solid (AB).

  • Carbon Oxides and Carbonates

    • Sodium carbonate is basic when dissolved in water (meaning it results in a basic solution upon dissolution), and sodium bicarbonate is weakly basic.
    • These effects can be explained by considering that upon dissolution and subsequent dissociation of the salt into its ions, the carbonate or bicarbonate ions will react with H+ in the solution to form H2CO3 (which has a low Ka value - i.e., is a weak acid).

  • Extractive Metallurgy

    • The most common hydrometallurgical process is leaching, which involves dissolution of the valuable metals into the aqueous solution.

  • Complex Ion Equilibria and Solubility

    • A well-known example is the addition of a concentrated solution of ammonia (NH3) to a suspension of silver chloride (AgCl), in which dissolution is favored by the formation of an ammine (NH3) complex.