Chapter 17, Problem 103RQ

Interpretation Introduction

Interpretation:

The equilibria that corresponds to ${\text{K}}_{\text{inst}}$ for each of the given complex ions and the equations for ${\text{K}}_{\text{inst}}$ are to be written.

Concept Introduction:

According to the law of chemical equilibrium, the equilibrium constant for an equilibrium reaction is the ratio of the product of the molar concentration of products to the product of the molar concentration of the reactants, each raised to the power of their stoichiometric coefficient in the overall balanced equilibrium reaction.

For a general equilibrium reaction, $\text{aA + bB }\underset{}{\overset{}{\rightleftarrows }}\text{cC+dD}$, the equilibrium constant will be represented as:

$K\text{ = }\frac{{\text{[C]}}^{\text{c}}{\text{[D]}}^{\text{d}}}{{\text{[A]}}^{\text{a}}{\text{[B]}}^{\text{b}}}$

The instability constant is reciprocal of the formation constant for an equilibrium reaction. The relation between these two is shown as follows:

$K_{\text{inst}}=\frac{1}{K_{\text{form}}}$

Here, $K_{\text{inst}}$ is the instability constant and $K_{\text{form}}$ is the formation constant.