Experiment Report: Concentration – Dilution of NaCl

1. Purpose

The purpose of this experiment is to ensure the proper execution of a basic laboratory procedure. Precision in measurement and calculation, as well as attention to detail, are crucial aspects of laboratory work. This experiment serves as a learning opportunity for students and aspiring scientists to develop precision and meticulousness in their work.

2. Abstract

Accurate execution of laboratory experiments is essential to obtain reliable results. This basic laboratory experiment involves the preparation of a 1 M solution of NaCl by mixing 100 ml of the solution with water.

Additionally, a 0.1 M MgS solution is prepared. The experiment includes both mass and volume measurements, utilizing equipment such as burettes, volumetric flasks, and pipettes. The aim is to teach students the importance of precision and accuracy in laboratory procedures.

3. Tools and Materials

• Volumetric flasks: 100 mL, 25 mL
• Beaker glass: 250 mL (2 pieces)
• Erlenmeyer flask: 100 mL
• Burette: 50 mL
• Burette stand
• Magnetic stirrer
• Balance
• Graduated pipette with pump: 10 mL
• Funnel
• Water
• NaCl

4. Procedure

Before commencing the experiment, the mass of NaCl (0.

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5 M NaCl, 100 ml) is determined. The mass of MgS (0.1 M MgS, 25 ml) is also calculated using the following equations:

M1V1 = M2V2

Where:

• M1 = Initial molarity (mol/L)
• V1 = Initial volume (L)
• M2 = Final molarity (mol/L)
• V2 = Final volume (L)

The result of the NaCl mass is 2.922019 g.

For the first part of the experiment:

1. Measure 2.922019 g of solid sodium chloride (NaCl) using a balance.
2. Place the NaCl into a 250 ml beaker and add approximately 75 ml of water.
3. Dissolve the NaCl in water using a magnetic stirrer at 400 rpm.
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4. Transfer 1 ml of the NaCl solution to a 25 ml volumetric flask.
5. Add 25 ml of water to the volumetric flask.

The result of the NaCl volume is 5 ml.

For the second part of the experiment, involving the burette:

1. Add water to a 250 ml beaker until it reaches the 0 ml mark on the burette.
2. Position an Erlenmeyer flask beneath the burette.
3. Dispense water from the burette until it reaches the 8.10 ml mark.
4. Deliver water from the burette until it reaches the 7.05 ml mark.
5. The final volume of the delivered water is 15.15 ml.

The proper technique for measuring solutions with a burette and volumetric flask is to read the volume from the bottom of the meniscus.

5. Discussion

Sodium chloride (NaCl) is composed of positive sodium ions bonded to negative chloride ions. Water can dissolve salt because the positive part of water molecules attracts the negative chloride ions, and the negative part of water molecules attracts the positive sodium ions.

Molarity (M), also known as molar concentration, represents the number of moles of a substance per liter of solution. The relationship between concentration, volume, and moles is described by the equation:

M = n / V

Where:

• M = Molarity (mol/L)
• n = Moles (mol)
• V = Volume (L)

Dilution is the process of reducing the concentration of a solution by adding solvent. The formula for dilution is:

M1V1 = M2V2

Where:

• M1 = Initial molarity
• V1 = Initial volume
• M2 = Final molarity
• V2 = Final volume

Dilution can be achieved by adding a less concentrated solution to a more concentrated one or by adding solvent to decrease the concentration while keeping the amount of solute constant.

6. Conclusion

From the experiment conducted, it is evident that precision in measurement is essential in laboratory work. While human errors are inevitable, accuracy is crucial, especially in the initial calculations. Any mistakes during the experiment require repeating the entire procedure from the beginning to ensure reliable results.