Slightly soluble solute

Slightly Soluble Solute Silver Chloride. For AgCl we can add the following equations ... [Pg.483]

An insoluble solid formed by mixing in solution the constituent ions of a slightly soluble solution. [Pg.36]

The driving force for stripping operations involving slightly soluble solutes is considered in terms of liquid-phase composition minus the composition of a liquid in equilibrium with the gas phase. Thus, the driving force is X X or X — p/H where Henry s Law applies. For practical purposes, again we have resorted to overall terms. The overall liquid-phase mass transfer coefficient in volumetric terms (KLa) is represented by the equation ... [Pg.52]

EXAMPLE 18-1 Writing Solubility Product Constant Expressions for Slightly Soluble Solutes... [Pg.832]

The equation for the solubility equilibrium is written for one mole of the slightly soluble solute. That is, the coefficient "1" is understood for the slightly soluble solute. The coefficients for the ions in solution are whatever is needed to balance the equation. The coefficients then establish the powers to which the ion concentrations are raised in the K p expression. [Pg.832]

PRACTICE EXAMPLE B A handbook lists K p = 1 X 10 for calcium hydrogen phosphate, a substance used in dentifrices and as an animal feed supplement. Write (a) the equation for the solubility equilibrium and (b) the solubility product constant expression for this slightly soluble solute. [Pg.832]

EXAMPLE 18-2 Calculating of a Slightly Soluble Solute from Its Solubility... [Pg.833]

Calculating the Solubility of a Slightly Soluble Solute in the Presence of a Common Ion... [Pg.836]

EXAMPLE 18-5 Applying the Criteria for Precipitation of a Slightly Soluble Solute... [Pg.840]

Other slightly soluble solutes having basic anions (such as ZnCOs, MgF2, and CaC204) also dissolve to a greater extent in acidic solutions. For these solutes, we can write overall net ionic equations for solubility equilibria and corresponding K values based on for the solutes and for the conjugate acids of the anions. [Pg.844]

Criteria for Precipitation and Its Completeness—To determine whether a slightly soluble solute will precipitate from a solution, the ion product, Qsp, is compared with the solubility product constant, K p. Q p is based on the initial ion concentrations in a solution. K p, on the other hand, is based on the equilibrium ion concentrations in a saturated solution. If Qgp > K p, precipitation will... [Pg.856]

Solubility and pH— The solubility of a slightly soluble solute is affected by pH if the anion is OH or derived from a weak acid. The solubility increases as the pH is lowered or decreases as the pH is raised. This can be illustrated through Le Chatelier s principle. Also, an equilibrium constant for the dissolution reaction can be obtained by combining the solubility equihbrium equation and the ionization equilibrium equation of the weak electrolyte. Some shghtly soluble solutions form suspensions, which are heterogeneous fluids containing solid particles that will eventually settle. [Pg.856]

The slightly soluble solute Ag2Cr04 is most soluble in (a) pure water (b) 0.10MK2CrO4 (c) O.25MKNO3 ... [Pg.863]

Appendix E describes a useful study aid known as concept mapping. Using the methods presented in Appendix E, construct a concept map that links the various factors affecting the solubility of slightly soluble solutes. [Pg.864]

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