Question

Why is it more accurate to say that the concentration of a solution of acetic acid is 0.01 f rather than 0.01 m?

Answer 1

The formal concentration accounts for the moles of the original chemical formula into the solution rather than the concentration of the species that actually exist in solution which is accounted for by the molarity.

Step-by-step explanation:

Hello,

In this case, the difference between formal and molar units of concentration lies on the fact that the formal concentration accounts for the moles of the original chemical formula into the solution rather than the concentration of the species that actually exist in solution which is accounted for by the molarity. In such a way, since acetic acid is partially dissociated, formality better explains there are 0.01 moles of acetic acid added to the solution including both the non-dissociated and dissociated constituents. However, molarity just accounts for the 0.01 moles of acetic acid that could or could not have been dissociated into the solution.

As you see, this is just a by concept difference, as they lead to suitable calculations.

Best regards.

Answer 2

A 1 F solution stands 1 formula unit per litre and 0.01 F describes the concentration of solution with no deliberation for the real form of existence of species.

Molarity is defined as the ratio of moles of solute to the volume of solution in litres and it is used to describe formality. For accuracy, it is essential to expressed molarity of each species. In case of acetic acid, the molarity of acetic acid molecules is less than 0.01 M due to dissociation.

Thus, it is more precise to say that the concentration of a solution of acetic acid is 0.01 F instead of 0.01 M.