Preparation of 0.1 N H2SO4 Solution from a 1.8g/mL Density and 98 mL Volume Solution

In this article, we will discuss the step-by-step process to prepare a 0.1 N H2SO4 solution given its density and the initial volume and concentration. This process involves understanding the principles of normality, density, and dilution, and applying them to accurately prepare the desired solution.

Understanding the Problem

We need to prepare 0.1 N H2SO4 using a solution with a density of 1.8 g/mL and a volume of 98 mL. This solution initially has a specific normality and molarity that we need to calculate and then use to determine the exact volume of this concentrated solution required to prepare the 0.1 N solution.

Calculating the Normality of the Initial Solution

The normality (N) of the initial solution can be calculated using the formula:

N C / Z

where C is the molarity (M) of the solution and Z is the number of equivalents per mole. For H2SO4, Z 2 (since it produces 2 H ions per mole).

Step 1: Determining the Mass of H2SO4

First, we calculate the mass of H2SO4 in the given volume using the density:

Mass Density × Volume

M 1.8 g/mL × 98 mL 176.4 g

Step 2: Calculating Molarity (M)

The molarity (M) of H2SO4 can be calculated using the formula:

M Mass of solute / Molar mass × Volume of solution in liters

M 176.4 g / 98.079 g/mol × 0.098 L

M 1.80 M

Therefore, the normality (N) of the initial solution:

N M / 2 1.80 M / 2 0.9 N

Step 3: Determining the Volume Required for the 0.1 N Solution

Now, we need to determine the volume of the 0.9 N solution required to prepare the 0.1 N solution. The dilution formula is:

V1N1 V2N2

Where V1 is the initial volume, N1 is the initial normality, V2 is the final volume, and N2 is the desired normality.

V1 × 0.9 N V2 × 0.1 N

V2 V1 × 0.9 N / 0.1 N

V2 0.098 L × 9 N

V2 0.882 L 882 mL

Step 4: Preparing the Solution

To prepare 0.1 N H2SO4, take 98 mL of the initial solution and dilute it to a final volume of 882 mL with distilled water. This ensures that the concentration is accurately diluted to the desired 0.1 N.

Conclusion

Preparing an accurately diluted solution like 0.1 N H2SO4 from a concentrated solution requires careful calculation and precise measurement. By understanding the principles of normality, density, and dilution, we can ensure that the final solution meets the required specifications.

Related Keywords

This article addresses several important keywords in chemistry and laboratory operations:

H2SO4 solution preparation normality calculation dilution process acid solutions chemical preparation

FAQs

What is normality (N) and how is it calculated?

Normality (N) is a measure of concentration defined as the number of equivalents of solute per liter of solution. It is calculated using the formula N C / Z, where C is the molarity (M) and Z is the number of equivalents per mole.

What is the difference between molarity and normality?

Molarity (M) is the number of moles of solute per liter of solution, while normality (N) is the concentration in equivalents per liter of solution. For monoprotic acids (like HCl), molarity and normality are the same, but for diprotic acids (like H2SO4), normality is twice the molarity.

How do you convert molarity to normality?

To convert molarity to normality, divide the molarity by the number of equivalents per mole (Z). For H2SO4, Z 2, so N M / 2.

Conclusion

Mastering the art of preparing accurate chemical solutions is a crucial skill for chemists and researchers alike. By understanding and applying the principles of normality, density, and dilution, one can ensure that the final solution is precisely as intended.