What is the normality of HNO3 when its molecular weight is 63.0 g?

To determine the normality of HNO3, it's essential to understand the concept of normality in relation to acids and their dissociation in water. Normality (N) is a measure of concentration equivalent to molarity (M) multiplied by the number of equivalents per mole of solute.

For HNO3, nitric acid is a strong acid that dissociates completely in solution, releasing one hydrogen ion (H+) per molecule. Since it donates one proton, the number of equivalents of HNO3 per mole is equal to 1.

The normality can be calculated using the formula:

Normality (N) = Molarity (M) × n

In this case, for HNO3, where n (the number of equivalents) is 1, the normality is equivalent to the molarity.

If you have 63.0 g of HNO3, this represents 1 mole because the molecular weight of HNO3 is 63.0 g/mol. When dissolved in 1 liter of solution, this gives a molarity of 1.0 M. Since the number of equivalents is 1 (because it donates one proton), the normality also becomes 1.0