How to Prepare 0.1 Molar Barium Nitrate Solution: A Comprehensive Guide

In the field of chemistry, the ability to prepare solutions of specific concentrations is crucial. Barium nitrate, a compound with the chemical formula Ba(NO?)?, is widely used in various applications. This article will guide you step-by-step through the process of preparing a 0.1 molar (M) aqueous solution of barium nitrate in a 100 mL volumetric flask.

Introduction to Barium Nitrate

Barium nitrate is a clear, colorless crystal that dissociates readily in water. It is soluble in water and is often used in the laboratory for the preparation of other compounds. Before we delve into the preparation process, it is essential to understand the basic definition of molarity and its relationship to solution concentration.

Molarity and Solution Concentration

Molarity (M) is defined as the number of moles of solute per liter of solution. The formula for calculating molarity is:

[ text{Molarity} frac{text{moles of solute}}{text{volume of solution in liters}} ]

Given the desired concentration of 0.1 M and a target volume of 100 mL, we can calculate the necessary moles of barium nitrate:

[ text{Moles of solute} text{Molarity} times text{Volume in liters} ]

[ text{Moles of Ba(NO?)?} 0.1 , text{M} times 0.1 , text{L} 0.01 , text{mol} ]

With the required moles known, we can proceed to the next step.

Preparing the Solution

To prepare 0.1 M barium nitrate, follow these detailed steps:

Calculate the required mass of barium nitrate. Using the molar mass of barium nitrate (261.34 g/mol), we can determine the mass needed:

[ text{Mass} text{Moles of solute} times text{Molar mass} ]

[ text{Mass} 0.01 , text{mol} times 261.34 , text{g/mol} 2.6134 , text{g} ]

Accurately weigh out 2.6134 grams of pure solid barium nitrate using a precision analytical balance. Ensure that the stopcock of the volumetric flask is closed during the weighing process to prevent any loss of powder.

Add the weighed barium nitrate to a 100 mL volumetric flask, then dissolve it in a small volume of distilled water. Swirl the flask gently to ensure complete dissolution.

Transfer the resulting solution to the volumetric flask and add distilled water until the bottom of the meniscus aligns with the calibration mark (100 mL) on the neck of the flask.

Close the stopcock tightly and shake the flask thoroughly to ensure the solution is well-mixed and free from any undissolved particles.

By following these steps, you will successfully prepare a 0.1 M barium nitrate solution in 100 mL of distilled water.

Note: Always handle chemicals with appropriate safety equipment and follow laboratory safety guidelines. Ensure that the solution is stored in a properly labeled container and kept away from incompatible materials.

Scaling the Solution Preparation

For preparing a different volume of solution, simply scale the required mass of barium nitrate based on the desired molarity and volume. The relationship can be expressed as:

[ text{Mass of solute} left( text{Molarity} times text{Volume in liters} right) times text{Molar mass} ]

This calculation will give you the precise amount of barium nitrate needed for any desired volume of solution.

Conclusion

Preparing a 0.1 M aqueous solution of barium nitrate in a 100 mL volumetric flask involves a few straightforward steps. By understanding the concepts of molarity and following the detailed procedures outlined, you can produce a highly concentrated and accurately measured solution suitable for various chemical applications.

Keywords

Barium nitrate, molar solution, volumetric flask, dilution