How to prepare 0.01 m sulfuric acid? Detailed steps and precautions

in laboratory chemistry, the preparation of solutions of different concentrations is a common task. As a strong acid, sulfuric acid is widely used in chemical experiments. This article will introduce in detail how to prepare 0.01 m sulfuric acid, and provide corresponding precautions to help you accurately complete the experimental operation.

What is 0.01 m sulfuric acid?

Before preparing 0.01 m sulfuric acid, it is first necessary to make it clear that "m" refers to the molar concentration (molarity), that is, the number of moles of solute per liter of solution. Thus, 0.01 m of sulfuric acid means that there are 0.01 moles of sulfuric acid molecules per liter of solution. In order to accurately prepare the sulfuric acid solution with this concentration, it is necessary to select the appropriate concentrated sulfuric acid for dilution according to the experimental requirements.

Select the appropriate concentrated sulfuric acid

normally, the concentration of concentrated sulfuric acid used in the laboratory is about 18 mol/L, so appropriate dilution is required to obtain the required 0.01 m sulfuric acid concentration. When selecting concentrated sulfuric acid, first confirm the concentration of concentrated sulfuric acid in order to correctly calculate the required volume and dilution ratio.

Calculate the required volume of concentrated sulfuric acid

to prepare 0.01 m of sulfuric acid, it is necessary to calculate the volume of concentrated sulfuric acid used. According to the concentration formula:

[ C1 V1 = C2 V2 ]

where (C1) is the concentration of concentrated sulfuric acid (18 mol/L),(V1) is the volume of concentrated sulfuric acid required,(C2) is the target concentration (0.01 mol/L), and (V2) is the volume of the final solution.

Assuming that we need to prepare 1 L(1000 mL) 0.01 m sulfuric acid solution, the volume of concentrated sulfuric acid required can be determined by the following calculation:

[ 18 \times V_1 = 0.01 \times 1000 ]

[ V_1 = \frac{0.01 \times 1000}{18} \approx 0.56 \, \text{mL} ]

therefore, to prepare 1 L of 0.01 m sulfuric acid solution, 0.56 mL of concentrated sulfuric acid is required.

Dilution step

1. prepare experimental equipment: A 1000 mL volumetric flask, pipette, distilled water, etc.
2. Take concentrated sulfuric acid: Use a pipette to accurately measure 0.56 mL of concentrated sulfuric acid.
3. Add water to dilute: After transferring the concentrated sulfuric acid to the volumetric flask, add a small amount of distilled water first, and then shake well. The addition of distilled water was then continued until the total amount of solution reached 1000 mL.
4. Mix the solution: In the process of adding water, pay attention to constantly shake the volumetric flask to ensure that the sulfuric acid and water are completely mixed and evenly.

Precautions

in the process of preparing 0.01 m sulfuric acid solution, there are several key points that require special attention:

• safety protection: Concentrated sulfuric acid is highly corrosive, so protective gloves, goggles and lab clothes must be worn during operation.
• Add acid, add water first: When adding acid, water should be added to the volumetric flask first, and then concentrated sulfuric acid should be added slowly. Do not pour water directly into concentrated sulfuric acid to avoid overheating and splashing.
• Accurate measurement: In order to ensure the accurate concentration of the solution, it is recommended to use high-precision pipettes and volumetric flasks for operation.
• Temperature change: Dilute concentrated sulfuric acid will release heat, so be careful to operate to avoid burns.

Summary

through the above steps, we can successfully prepare 0.01 m sulfuric acid solution. In the experiment, accurate measurement and safe operation are essential. Knowing how to prepare 0.01 m sulfuric acid solution can not only improve the accuracy of the experiment, but also ensure the safety of personnel in the experiment. I hope the analysis and steps of this article can help you with your experimental operation.