How many milliliters of HNO3 are needed to prepare 1.0 L of a 2.0 N solution?

To determine how many milliliters of HNO3 (Nitric Acid) are required to prepare a 1.0 L solution at a concentration of 2.0 N (Normal), it's essential to understand the relationship between normality, volume, and molarity of the solution.

Normality is a measure of concentration equivalent to the molarity multiplied by the number of equivalence factors. For HNO3, which is a strong acid, it has one acidic proton available for reaction, making its normality equivalent to its molarity for typical acid-base reactions. Therefore, a 2.0 N solution of HNO3 is also a 2.0 M solution.

To calculate the volume of concentrated HNO3 needed, we can use the formula:

[ \text{C}_1 \times \text{V}_1 = \text{C}_2 \times \text{V}_2 ]

Where:

• ( C_1 ) is the concentration of the concentrated solution (about 15.7 M for concentrated HNO3),

• ( V_1 ) is the volume of the concentrated solution we need to find,

• ( C_2 ) is the desired concentration (2.0 M