Chapter 19, Problem 96AP

Interpretation Introduction

Interpretation:

The solubility product constant for silver oxalate is to be determined, with given potential difference between the rod and the standard hydrogen potential.

Concept introduction:

The solubility product is the product of the equilibrium concentrations of the ions of a salt at saturation point

The stoichiometric coefficients are present as the raised power for each concentration of ions.

For a general reaction: $\text{AB}\left(s\right)\rightleftharpoons {\text{A}}^{+}\left(aq\right)+{\text{B}}^{-}\left(aq\right)$

The solubility product can be calculated by the expression as: $K_{\text{sp}}{\text{= [A}}^{\text{+}}{\text{][B}}^{-}\text{]}$

Here $K_{\text{sp}}$ is solubility product constant and $\text{sp}$ stands for solubility product.

For a general reaction: $a\text{A}\text{+}b\text{B}\rightleftarrows c\text{C}\text{+}d\text{D}$.

Reaction quotient is defined as the ratio of concentration of products and reactants of chemical species present in the reaction mixture at a given point of time. It is denoted with $\text{Q}$.

$\text{Reaction quotient, }{Q}_c=\frac{{\left[\text{C}\right]}^{\text{c}}{\left[\text{D}\right]}^{\text{d}}}{{\left[\text{A}\right]}^{\text{a}}{\left[\text{B}\right]}^{\text{b}}}$.

The Nernst equation is an important equation in electrochemistry. The equation is represented below:

$E=E^{\text{o}}-\frac{\text{R}T}{n\text{F}}\ln Q$

$E=E^{\text{o}}-\frac{0.0592\text{ V}}{n}\log Q$

Here, $E$ is the emf of the cell, $E_{cell}^{\circ }$ is the standard cell potential of the cell, $n$ is the number of electrons, and $Q$ is the reaction quotient.