Final answer:
The statement is false because the activity coefficient for hydrogen ions is likely smaller in 0.01 M FeSO4 than in 0.01 M NaCl, due to the higher ionic strength of FeSO4 resulting from its higher dissociation into ions with greater charges.
Step-by-step explanation:
The statement regarding the activity coefficient of hydrogen ions (H+) being smaller in 0.01 M NaCl than in 0.01 M FeSO4 pertains to the concept of ionic strength and its effect on the activity coefficients of ions in solution.
According to Debye-Hückel theory, activity coefficients are influenced by the ionic strength of the solution.
A solution with higher ionic strength, which depends on the concentrations and charges of all ions in the solution, will typically have lower activity coefficients for its ions.
FeSO4 is a salt that dissociates into three ions (Fe2+, SO42-), each with higher charges compared to NaCl, which dissociates into two ions with single charges (Na+, Cl-).
Therefore, 0.01 M FeSO4 would have a higher ionic strength than 0.01 M NaCl, leading to a smaller activity coefficient for hydrogen ions in FeSO4 than in NaCl. Thus, the initial statement is false.
Considering van't Hoff factors, which indicate the degree of dissociation of electrolytes in solution, also supports this concept.
The higher the factor (representing more dissociation and higher ionic charges), the greater the reduction in activity coefficient due to increased ionic strength.
Therefore, the activity coefficient for H+ is expected to be smaller in 0.01 M FeSO4 than in 0.01 M NaCl given its higher ionic strength.