Chemical Equilibrium Theory - An Introduction
Chemical equilibria are found everywhere in nature and are an important part of many industrial processes. There are several "types" of chemical equilibria which include; 1) Slightly soluble ionic compounds, 2) Weak acid & weak base equilibria, 3) gas-phase processes, and 4) Buffer Systems.Equilibrium Constant Equations
The equilibrium constant equation is the mathematical representation of equilibrium position. Several important solution properties can be determined by analysis and algebraic manipulation of the equilibrium constant equation. Among these properties are 1) compound solubility, 2) acid strength, 3) buffer pH, and 4) gas-phase theoretical yield.
The following table describes the symbols used in Equilibrium Constant Calculations for a monoprotic weak acid, such as acetic acid.
The following table describes the symbols used in Equilibrium Constant Calculations for a monoprotic weak acid, such as acetic acid.
Definition of Equilibrium Constant Equation Terms
The following document explains how to do a typical weak acid problem.
From the initial acid-dissociation constant equation, mx equals hydrogen ion molar concentration because m * H+ moles are produced for each mole of original acid dissociated.
Notice that we have also created a formula by working with the general chemical equation.
That's all for now. Thank you for reading!
A Publication of http://ExcellenceInLearning.bizFrom the initial acid-dissociation constant equation, mx equals hydrogen ion molar concentration because m * H+ moles are produced for each mole of original acid dissociated.
Notice that we have also created a formula by working with the general chemical equation.
That's all for now. Thank you for reading!