What is the normality of 2.4M H2CO3?

Answer 1

These statements may be helpful for answering this question:

Normality is equal to the number of equivalent weights of solute per Liter of solution.

Molarity is equal to the number of moles of solute per Liter of solution, and to determine the number of moles, you take the weight of the solutes in solution divided by the weight of one of those solute molecule (the molecular weight).

How does one relate equivalent weights to moles. The equivalent weight of a compound is equal to its molecular weight divided by its valence. The valence in this context means the same thing as the number of substitutable groups (H+s or OH-s). Carbonic acid is a diprotic acid that dissociates to release 2 ionizable H+ s. So along those lines, a 1 M solution of H2CO3 is equivalent to a 2N solution of H2CO3. If 1 molar H2CO3 = 2N H2CO3 , a 2.4 M H2CO3 with 2 ionizable groups x 2.4, or 4.8N.

Sorry if you got my first answer and that confused you, the second answer (4.8) is the correct one. I confused normality with equivalent weight. The equivalent weight of an acid with a valence >1 like H2CO3 (valence = 2) is in fact less than its molecular weight, but the question was about normality, the number of equivalents present in a liter of solution which is not the same as the equivalent weight.

Answer 2

The normality of a solution is defined as the molarity multiplied by the number of equivalents per mole of solute. For H2CO3 (carbonic acid), there are 2 acidic protons per molecule. Therefore, the normality of a 2.4M H2CO3 solution would be 4.8N.

Answer 3

1.1 (g/L) / 100 (g/mol H2SO4) * 2 (equiv.H+/mol H2SO4) = 0.022 N