If you have a 7.46 normal solution of carbonic acid, what would be its molarity?

To determine the molarity of a 7.46 normal solution of carbonic acid, it is important to understand the relationship between normality and molarity, particularly for acids and bases. Normality (N) is a measure of the concentration of equivalents of reactive species in a solution, while molarity (M) is a measure of the moles of solute per liter of solution.

For carbonic acid (H2CO3), which is a diprotic acid, it can donate two protons (H+) per molecule when it dissociates in water. This means that a one molar solution of carbonic acid would contribute two equivalents of protons, making the normality twice the molarity for carbonic acid.

The formula that relates molarity (M) to normality (N) for diprotic acids is:

[ \text{Normality} = 2 \times \text{Molarity} ]

Using this relationship, if the normality of the solution is 7.46 N, we can find the molarity by rearranging the equation:

[ \text{Molarity} = \frac{\text{Normality}}{2} ]

Substituting the given normal