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Equilibrium-constant expression

The acid dissociation constant has the same form m Brpnsted-Lowry as m the Arrhenius approach but is expressed m the concentration of H30" rather than The concentration terms [H30" ] and [H" ] are considered equivalent quantities m equilibrium constant expressions... [Pg.35]

Even though water is a reactant (a Brpnsted base) its concentration does not appear m the expression for because it is the solvent The convention for equilibrium constant expressions is to omit concentration terms for pure solids liquids and solvents... [Pg.35]

Several types of reactions are commonly used in analytical procedures, either in preparing samples for analysis or during the analysis itself. The most important of these are precipitation reactions, acid-base reactions, complexation reactions, and oxidation-reduction reactions. In this section we review these reactions and their equilibrium constant expressions. [Pg.139]

The equilibrium position for any reaction is defined by a fixed equilibrium constant, not by a fixed combination of concentrations for the reactants and products. This is easily appreciated by examining the equilibrium constant expression for the dissociation of acetic acid. [Pg.148]

Write all relevant equilibrium reactions and their equilibrium constant expressions. [Pg.159]

Count the number of species whose concentrations appear in the equilibrium constant expressions these are your unknowns. If the number of unknowns equals the number of equilibrium constant expressions, then you have enough information to solve the problem. If not, additional equations based on the conservation of mass and charge must be written. Continue to add equations until you have the same number of equations as you have unknowns. [Pg.159]

Substituting equations 6.39 and 6.40 into the equilibrium constant expression for the dissociation of HE (equation 6.35) and solving for the concentration of H3O4 gives us... [Pg.161]

Counting unknowns, we find that there are seven—[Ag+], [I ], [Ag(NH3)2 ], [NH3], [NH4+], [OH ], and [H3O+]. Four of the equations needed to solve this problem are given by the equilibrium constant expressions... [Pg.166]

Since the concentrations of Na+, A-, HA, H3O+, and OH- are unknown, five equations are needed to uniquely define the solution s composition. Two of these equations are given by the equilibrium constant expressions... [Pg.168]

You should be able to describe a system at equilibrium both qualitatively and quantitatively. Rigorous solutions to equilibrium problems can be developed by combining equilibrium constant expressions with appropriate mass balance and charge balance equations. Using this systematic approach, you can solve some quite complicated equilibrium problems. When a less rigorous an-... [Pg.176]

Write equilibrium constant expressions for the following reactions. Determine the value for the equilibrium constant for each reaction using appropriate equilibrium constants from Appendix 3. [Pg.176]

Substituting the equilibrium constant expressions for reactions 8.3-8.S into equation 8.6 defines the solubility of AgCl in terms of the equilibrium concentration of Ch. [Pg.236]

Starting with the equilibrium constant expressions for reactions 8.1, and 8.3-8.5, verify that equation 8.7 is correct. [Pg.267]

The change in the concentration of H3O+ is monitored with a pH ion-selective electrode, for which the cell potential is given by equation 11.9. The relationship between the concentration of H3O+ and CO2 is given by rearranging the equilibrium constant expression for reaction 11.10 thus... [Pg.484]

For every gaseous chemical system, an equilibrium constant expression can be written stating the condition that must be attained at equilibrium. For the general system involving only... [Pg.326]

At a given temperature, the pressure of iodine vapor is constant, independent of the amount of solid iodine or any other factor. The equilibrium constant expression is... [Pg.330]

Applying the reciprocal rule (page 327), we can deduce the equilibrium constant expression for the reverse reaction... [Pg.330]

Write equilibrium constant expressions (X) for die following reactions ... [Pg.345]

Given the following descriptions of reversible reactions, write a balanced equation (simplest whole-number coefficients) and the equilibrium constant expression (X) for each. [Pg.345]

Recall (page 331, Chapter 12) that in the equilibrium constant expression for reactions in solution—... [Pg.354]

Hence for the ionization of water, the equilibrium constant expression can be written ... [Pg.354]

For simplicity, throughout this chapter, we will use H+ rather than H3Q+ in equilibrium constant expressions. [Pg.354]

Substituting into the equilibrium-constant expression, we find... [Pg.369]

The equilibrium constant expression for the dissolving of SrCr04 can be written following the rules in Chapters 12 and 13. In particular, the solid does not appear in the expression the concentration of each ion is raised to a power equal to its coefficient in the chemical equation. [Pg.431]


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