How Many Gm of Conc. Nitric Acid Solution should be used to Prepare 250ml of 2m HNO3, Given

Introduction

Nitric acid, also known as HNO3, is a strong acid commonly used in laboratories and industrial settings. It is a highly corrosive and reactive substance and must be handled with care. When preparing a solution of HNO3, it is important to accurately measure the amount of concentrated acid needed in order to obtain the desired concentration. Concentrated nitric acid is typically sold as a solution containing a certain percentage of HNO3 by weight. For example, a bottle of concentrated nitric acid may be labelled as "70 per cent HNO3".Therefore for every 100 grams of solution, 70 grams is pure HNO3, and the remaining 30 grams is made up of water and other impurities.

In order to prepare a solution of HNO3 with a specific concentration, it is necessary to calculate the volume of concentrated nitric acid needed based on the desired concentration and volume of the final solution. This can be done using the formula:

C1V1 = C2V2

Where C1 is the concentration of the concentrated acid, V1 is the volume of the concentrated acid needed, C2 is the desired concentration of the final solution, and V2 is the quantity of the final solution.

Example

To prepare 250 millilitres of 2 molar HNO3 solutions using a bottle of concentrated nitric acid labelled as "70 per cent HNO3", we can use the following steps:

Use the following formula to calculate the volume of concentrated nitric acid needed.

C1V1 = C2V2

In this case, C1 is 0.7 (since the concentrated acid is 70 per cent HNO3), V1 is the unknown quantity, C2 is 2, and V2 is 250 millilitres. Plugging in the values, we get:

0.7 X V = 2 X 250

Solving for V1, we find that we need approximately 178.57 millilitres of concentrated nitric acid to prepare 250 millilitres of 2 molar HNO3 solutions.

1. Determine the density of the concentrated nitric acid solution. For this example, we will assume a density of 1.5 grams per millilitre for the concentrated nitric acid solution.

2. Use the density of the concentrated nitric acid solution to calculate the Mass of concentrated acid needed. Given the density of 1.5 grams per millilitre, we can calculate the Mass of concentrated nitric acid needed to prepare 250 millilitres of 2 molar HNO3 solutions as follows:

Mass = Density X Volume

where Mass is the Mass of concentrated nitric acid needed, density is the density of the concentrated acid solution, and Volume is the volume of concentrated acid needed (as calculated earlier). Plugging in the values, we get:

Mass = 1.5 X 178.57

Solving for Mass, we need approximately 267.85 grams of concentrated nitric acid to prepare 250 millilitres of 2 molar HNO3 solutions.

Conclusion

In order to prepare 250 millilitres of 2 molar HNO3 solutions, we need to use approximately 178.57 millilitres of concentrated nitric acid. It is important to carefully measure the amount of concentrated acid used in order to obtain the desired concentration of the final solution.