The mean ionic activity coefficient of 0.1 molar HCl(aq) at 25^∘ C is 0.796 . What is the activi

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The mean ionic activity coefficient of 0.1 molar HCl(aq) at...

The mean ionic activity coefficient of 0.1 molar $\mathrm{HCl}(\mathrm{aq})$ at $25^{\circ} \mathrm{C}$ is $0.796 .$ What is the activity of $\mathrm{HCl}$ in this solution? (b) The mean ionic activity coefficient of $0.1 \mathrm{mo}$ $\operatorname{lar} \mathrm{H}_{2} \mathrm{SO}_{4}$ is $0.265 .$ What is the activity of $\mathrm{H}_{2} \mathrm{SO}_{4}$ in this solution?

The mean ionic activity coefficient of 0.1 molar $\mathrm{HCl}(\mathrm{aq})$ at $25^{\circ} \mathrm{C}$ is $0.796 .$ What is the activity of $\mathrm{HCl}$ in this solution?
(b) The mean ionic activity coefficient of $0.1 \mathrm{mo}$ $\operatorname{lar} \mathrm{H}_{2} \mathrm{SO}_{4}$ is $0.265 .$ What is the activity of $\mathrm{H}_{2} \mathrm{SO}_{4}$ in this
solution?

Key Concepts

Electrolyte Dissociation

Electrolyte dissociation refers to the process by which an ionic compound, when dissolved in a solvent, separates into its individual ions. The degree of dissociation and the interactions among the ions in solution influence both the concentrations of the ions and their corresponding activity coefficients, thereby affecting the overall reaction behavior and equilibrium conditions.

Activity

Activity is a measure of the effective concentration of a chemical species in a solution that takes into account non-ideal interactions. It is obtained by multiplying the molar concentration by the activity coefficient. In equilibrium and thermodynamic equations, the activity is used rather than the pure concentration in order to precisely represent the chemical potential of the species.

Ionic Activity Coefficient

This factor quantifies the deviation from ideal behavior of ions in solution. In an ideal solution, the activity (or effective concentration) of an ion would equal its actual molar concentration. In real solutions, however, electrostatic interactions between ions cause these activities to differ, and the ionic activity coefficient is used to bridge this gap.

Mean Ionic Activity Coefficient

For electrolytes that dissociate into multiple ions, the mean ionic activity coefficient is defined as the geometric average of the individual ionic activity coefficients, weighted by the number of ions produced upon dissociation. This single coefficient is particularly useful when expressing equilibrium constants since it allows one to combine the effects of all dissociating ions into one effective parameter.

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