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According to Debye-Hückel theory, activity coefficient depends directly on ionic strength. When ionic strength approaches zero, the activity coefficient approaches unity, indicating ideal behavior. As ionic strength increases from 0 to 0.1 mol/L, the activity coefficient decreases. Above 0.1 mol/L, the activity coefficient may increase, though the Debye-Hückel equation becomes less accurate at these higher concentrations.

Ion charge directly influences activity coefficient magnitude. With increased charge on an ion, the decrease in activity coefficient becomes more pronounced. For a given ionic strength, ions with higher charges show greater deviation from ideal behavior compared to singly charged ions. This relationship between charge and activity coefficient is fundamental to understanding ion behavior in solution.

Ion size, defined as the effective diameter of a hydrated ion, significantly affects activity coefficient. Ions with smaller size parameters deviate more from ideality, resulting in lower activity coefficients than similarly charged ions with larger size parameters. Even ions with identical charges can have different activity coefficients due to variations in hydration extent and resulting effective diameters.

For a particular ionic strength, ions with the same charge have approximately equal activity coefficients. However, differences in ion size parameters—the effective diameter of hydrated ions—can cause variations even among similarly charged ions. The dominant factor in these discrepancies is the extent of hydration, which determines the effective diameter and influences deviation from ideal behavior.

An activity coefficient approaching unity indicates that the ion behaves ideally in solution. This occurs when ionic strength approaches zero, meaning the solution contains very few dissolved ions. Under these conditions, ions experience minimal electrostatic interactions with other ions, so their actual concentration closely approximates their effective concentration, or activity.

The extended Debye-Hückel equation shows that activity coefficient depends on three partially interdependent properties: ionic strength, ion charge, and ion size parameter. Ionic strength and charge together determine the magnitude of electrostatic effects, while ion size modulates how strongly an ion responds to these effects. All three factors must be considered together to accurately predict activity coefficient values.

The Debye-Hückel equation accurately predicts activity coefficients at low to moderate ionic strengths, up to approximately 0.1 mol/L. At higher ionic strengths, the equation's assumptions break down, and activity coefficients may exceed unity rather than continuing to decrease. The extended Debye-Hückel equation provides better representation at these higher concentrations, though even it has limitations.