Experiment 1: Preparation of a 1N HCl Solution

Objective: To prepare 100 milliliter of a 1N (Normal) hydrochloric acid (HCl) solution from a
concentrated stock solution of HCl.

Materials Required:
• Concentrated hydrochloric acid (usually around 36% HCl by weight, with a density of
~1.18 g/mL).
• Distilled water.
• 1000 mL volumetric ask.
• Graduated cylinder or pipette.
• Personal protective equipment (gloves, lab coat, goggles).
• Analytical balance.

Theory: The normality (N) of a solution refers to the number of equivalents of solute per liter
of solution. For HCl, each mole of HCl provides one equivalent because it dissociates to
give one mole of H+ ions. Therefore, for HCl:

Normality (N)=Molarity (M)×n-factor

where the n-factor for HCl is 1.

Calculating the volume of concentrated HCl needed:

Determine the molarity of the concentrated HCl stock:

If the concentrated HCl solution is 36% by weight with a density of 1.18 g/mL, the molarity
(M) of HCl can be calculated as follows:

Mass of HCl per liter = Density × Volume × %concentration =

= 1.18g/mL × 1000mL × 0.36 = 425.4g

Since the molar mass of HCl is approximately 36.46 g/mol:

Molarity (M) = 425.4/36.46 ≈ 11.67M

Calculate the volume of concentrated HCl needed for 1N solution:

Volume of HCl needed =

(Desired Normality × Volume of solution) / Molarity of stock solution =

= (1N × 1000mL) /11.67 M ≈ 85.7mL

So, 85.7 mL of concentrated HCl will need to be diluted to 1 liter with distilled water to
prepare a 1N HCl solution. Hence, for 100 milliliter 8.57 ml of concentrated HCl will be
required.

Procedure:

1. Safety First: Put on gloves, goggles, and a lab coat.

2. Measure the Concentrated Acid: Using a graduated cylinder, carefully measure out 8.57
mL of concentrated HCl. Always handle concentrated acids in a fume hood.
3. Dilute with Distilled Water: Add about 80 mL of distilled water to the 100 mL volumetric
ask.
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 4. Slowly add the measured 8.57 mL of concentrated HCl to the water. Always add acid to
water, never the reverse, to avoid splashing and excessive heat generation.
5. Swirl the ask gently to mix the solution thoroughly.
6. Bring to Final Volume: After the solution cools down, add more distilled water to bring
the total volume up to the 100 mL mark on the ask.
7. Mix the Solution: Cap the ask and invert it several times to ensure thorough mixing.

Observations:

Record any noticeable temperature change or reactions (e.g., heat release or fumes) when
diluting the concentrated acid.

Results:
Now we have a 1N HCl solution.

Precautions:
Always wear appropriate protective equipment.
Always add acid to water to avoid splashing.
Use a fume hood when handling concentrated HCl due to its fumes.
This experiment provides a practical understanding of normality and careful preparation of
solutions, relevant in titrations and other quantitative analyses.
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 Experiment 2: Preparation of 1% Sodium Chloride (NaCl) Solution
Objective: To prepare 100 mL of 1% NaCl solution using analytical grade sodium chloride.

Principle: A 1% (w/v) solution means 1 g of solute (NaCl) dissolved in 100 mL of solution.

Sodium chloride is highly soluble in water, so the solution is prepared by weighing the
required amount of salt and dissolving it in distilled water up to the desired volume.

Requirements
• Sodium chloride (NaCl, analytical grade)
• Distilled water
• Analytical balance
• 100 mL volumetric ask
• Spatula
• Beaker (100 mL)
• Glass rod / magnetic stirrer

Calculation:
1% = 1 g NaCl in 100 mL solution; therefore, weigh 1.00 g NaCl.

Procedure
1. Weighing: Place a clean and dry paper on the balance. Accurately weigh 1.00 g NaCl
using an analytical balance.
2. Dissolving: Add about 80 mL of distilled water. Stir with a glass rod until the salt
dissolves completely.
3. Dilution to Volume: Transfer the solution into a 100 mL volumetric ask. Make up the
volume to the 100 mL calibration mark with distilled water.
4. Mixing: Stopper the ask and invert it gently several times to ensure uniform mixing.

Observation: A clear, colorless NaCl solution is obtained.

Result: 100 mL of 1% NaCl solution has been successfully prepared.

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Experiment 3: Preparation of 1% Acetic Acid Solution (v/v and w/v both)

Objective: To prepare 100 mL of 1% acetic acid solution in the laboratory.

Principle
Acetic acid is commonly available as glacial acetic acid (100% acetic acid, density ≈ 1.049
g/mL, molar mass = 60 g/mol). A 1% solution may be prepared either:

v/v basis → 1 mL glacial acetic acid in 99 mL water.

w/v basis → 1 g acetic acid dissolved and diluted to 100 mL water.

Materials Required
• Glacial acetic acid
• Distilled water
• 100 mL volumetric ask
• Measuring cylinder (1 mL, 10 mL, 100 mL)
• Dropper and funnel
• Beaker, glass rod, pipette

Procedure
v/v method: 1% v/v

1. Take a clean 100 mL volumetric ask.

2. Using a pipette or measuring cylinder, measure 1 mL of glacial acetic acid carefully.
3. Transfer the acetic acid into the volumetric ask.
4. Add about 50 mL of distilled water, mix gently.
5. Make up the volume to the 100 mL mark with distilled water.
6. Stopper and invert the ask several times to ensure uniform mixing.

w/v method: 1% w/v

1. Calculate the required amount: 1% w/v = 1 g acetic acid in 100 mL solution.
2. Since density of glacial acetic acid ≈ 1.049 g/mL:
Volume needed =1g / 1.049g/mL ≈ 0.95 mL

3. Pipette out 0.95 mL glacial acetic acid and transfer into a 100 mL volumetric ask.
4. Add distilled water up to the mark, mix well.

Observation: A clear, colorless solution is obtained.

Result: 1% acetic acid solution is successfully prepared.

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 Experiment 4: Predicting the Solubility of Sodium Chloride (NaCl) in
Water at Room Temperature
Objective: To measure and predict the solubility of NaCl in water at room temperature.

Materials Required:
• Sodium chloride (NaCl).
• Distilled water.
• Beakers (100 mL or larger).
• Graduated cylinder (for measuring water).
• Stirring rod or magnetic stirrer.
• Thermometer.
• Hot plate (for heating).
• Analytical balance.
• Filter paper and funnel (optional, to remove undissolved salt).

Theory: Solubility refers to the maximum amount of solute that can dissolve in a solvent at a
speci c temperature to form a saturated solution. This experiment will help to understand
solubility by determining the amount of NaCl that dissolves at room temperature.

Procedure:
1. Preparation of NaCl Solutions: Measure 100 mL of distilled water using a graduated
cylinder and pour it into a beaker.
2. Weigh out a known amount of NaCl (e.g., 30 to 35 grams) on an analytical balance.
3. Add the NaCl to the water in small increments, stirring constantly with a stirring rod or
magnetic stirrer.
4. Keep adding NaCl until no more dissolves and a small amount remains undissolved at
the bottom. This indicates the solution is saturated.
5. Record the amount of NaCl added up to this saturation point.
6. Optional Filtering: If there is undissolved NaCl left after reaching saturation, we can lter
the solution to remove it.

Observations: Record the amount of NaCl dissolved in grams.

Results: A clear, colorless NaCl solution is obtained.

Precautions: Make sure to add NaCl slowly to avoid oversaturation.

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 Experiment 5: Recovery of Salt from Saltwater Solution
Objective: To recover solid salt (sodium chloride) from a saltwater solution through the
process of evaporation.

Materials Required:
• Salt (sodium chloride, NaCl).
• Distilled water.
• Beaker (100 mL or larger).
• Heat source (hot plate or Bunsen burner).
• Evaporating dish.
• Tripod stand and wire gauze (if using a Bunsen burner).
• Spatula.
• Weighing balance.

Theory:
Salt recovery from a saltwater solution is based on the principle of evaporation. When a salt
solution is heated, the water evaporates, leaving behind the dissolved salt as a solid
residue.

Procedure:
1. Preparation of Saltwater Solution: Use solution from previous experiment 4.
2. Setting Up for Evaporation: Transfer the saltwater solution from the beaker to an
evaporating dish.
3. Place the evaporating dish on a heat source, such as a hot plate or over
4. Evaporation: Heat the solution gently to avoid splattering.
5. Allow the water to evaporate slowly until only the solid salt remains in the evaporating
dish.
6. Observation of Crystals: After all the water has evaporated, observe the salt crystals left
in the evaporating dish.
7. Allow the evaporating dish to cool before handling.
8. Collection and Weighing: Once the salt is dry, we may weigh it to determine the amount
recovered and compare it with the initial amount of salt used.

Observations: Record the appearance of the salt before and after the experiment.

Results: Recovered solid salt in the evaporating dish, which should closely match the initial
amount of salt added to the water.

Conclusion: This experiment demonstrates that salt can be recovered from a saltwater
solution through evaporation, separating the dissolved solid from the liquid.

Precautions:
• Use heat-resistant gloves or tongs when handling hot equipment.
• Heat gently to prevent splattering and avoid overheating once the water evaporates.
• Be cautious not to overheat once the water is gone, as excessive heating may cause
salt to decompose.