Chem Lab Report 2

Objective: To prepare a 0.
1 mol sodium hydroxide solution by dissolving 2g of

sodium hydroxide in distilled water.
Theory: Sodium Hydroxide (NaOH) is a strong base, and it is commonly used in

laboratories to create basic solutions. To create a 0.1 mol NaOH solution, the
required amount of NaOH solid needs to be dissolved in a specific volume of
water. The molarity (M) of a solution is the number of moles of solute (NaOH in
this case) per litre of solution. In this experiment, 2 grams of NaOH is used to
prepare a 0.1 mol solution in a 500ml volumetric flask.
Apparatus list:
1) 500 mL volumetric flask
2) Filter paper
3) Spatula
4) Conical flask
5) Funnel
6) Digital weight machine
Chemicals and Reagents:

1) Sodium Hydroxide (NaOH), 2 grams of 0.1 M concentration
2) Distilled water
Procedure:
1) Use the digital weight machine to accurately weigh 2 grams of sodium
hydroxide pellets. Use a spatula to transfer the pellets to the filter paper.
2) Carefully transfer the weighed NaOH pellets from the filter paper to a
clean, dry conical flask.
3) Add approximately 200 mL of distilled water to the NaOH in the conical
flask. Stir gently until the NaOH is completely dissolved. This will generate
heat due to the exothermic reaction, so be careful while handling.
4) After the NaOH is completely dissolved, carefully pour the solution into the
500 mL volumetric flask using a funnel. Make sure not to spill any solution.
5) Rinse the conical flask with small amounts of distilled water several times
and add these washings to the volumetric flask. This ensures that all NaOH
from the flask is transferred.
6) Add more distilled water into the 500 mL volumetric flask until the lower
part of the meniscus touches the 500 mL mark on the neck of the flask.
Make sure to add water slowly when you’re near the mark to prevent
overfilling.
7) Stopper the flask and invert it several times to ensure the NaOH is evenly
distributed throughout the solution.
Calculations:
The molar mass of Sodium Hydroxide (NaOH) is approximately 40 g/mol. The
molarity (M) of a solution is calculated by the number of moles of the solute per
litre of solution.
In order to prepare a 0.1 M solution of NaOH in a 500 mL (or 0.5 L) solution, we

can use the following formula:
Molarity (M) = Moles of solute / Volume of solution in litres
To calculate the number of moles of solute needed for the 0.1 M solution:
Moles of solute = Molarity (M) * Volume of solution in litres

= 0.1 M * 0.5 L = 0.05 moles of NaOH
The mass of solute required can be calculated by:
Mass of solute = Moles of solute * Molar mass of solute
= 0.05 moles * 40 g/mol = 2 grams of NaOH
Therefore, 2 grams of Sodium Hydroxide is required to prepare a 0.1 M NaOH

solution in a 500 mL volumetric flask.
Results and Observations:

At the end of the procedure, a 0.1 M solution of sodium hydroxide was
successfully prepared. The final solution was clear and colorless.
Discussion:
During this experiment, we precisely weighed 2 grams of Sodium Hydroxide
(NaOH) and dissolved it in 200 mL of distilled water, subsequently diluting the
solution in a 500 mL volumetric flask. Through calculations using the molar mass
of NaOH (approximately 40 g/mol) and the molarity formula, it was confirmed
that the final solution was indeed 0.1 M, adhering to the initial objective. Key
precautions taken included careful handling of NaOH, ensuring its complete
dissolution, and accurate measurement of the final volume at room temperature.
The experiment demonstrated crucial laboratory techniques and safety measures
while solidifying fundamental chemical concepts.
Precautions:
1) Sodium Hydroxide is a strong base and can cause burns. Handle with care,
use gloves, and wear safety goggles.
2) Always add NaOH to water, not water to NaOH to prevent a violent
reaction.
3) When filling the volumetric flask, make sure the solution is at room
temperature to ensure accurate volume measurements. Heat can cause the
solution to expand, which can lead to inaccurate measurements.
4) Ensure thorough mixing of the solution in the volumetric flask to ensure
uniform concentration.

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Chem Lab Report 2

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Objective: To prepare a 0.

1 mol sodium hydroxide solution by dissolving 2g of

Theory: Sodium Hydroxide (NaOH) is a strong base, and it is commonly used in

Chemicals and Reagents:

In order to prepare a 0.1 M solution of NaOH in a 500 mL (or 0.5 L) solution, we

Molarity (M) = Moles of solute / Volume of solution in litres

Moles of solute = Molarity (M) * Volume of solution in litres

The mass of solute required can be calculated by:

Mass of solute = Moles of solute * Molar mass of solute

= 0.05 moles * 40 g/mol = 2 grams of NaOH

Therefore, 2 grams of Sodium Hydroxide is required to prepare a 0.1 M NaOH

Results and Observations:

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