Скачать или смотреть EXP:1|Determine Molarity & Volume of the given H₂SO₄|CHEMISTRY|PBA| GRADE:12|FBISE|NBF|HSSC-I&II

Experiment: Acid–Base Titration
📘 Description

This experiment is based on the principle of acid–base neutralization reaction. In this practical, the exact molarity of the given Sulfuric acid solution is determined by titrating it against a standard solution of Sodium carbonate.

Sodium carbonate is used as a primary standard because it is pure, stable, and its molarity can be prepared accurately. The reaction between sulphuric acid (strong acid) and sodium carbonate (weak base) occurs in a fixed 1:1 mole ratio:

H₂SO₄ + Na₂CO₃ → Na₂SO₄ + CO₂ + H₂O

By applying the formula:

𝑀
1
𝑉
1
=
𝑀
2
𝑉
2
M
1
​

V
1
​

=M
2
​

V
2
​


the unknown molarity of H₂SO₄ is calculated using the known molarity and volume of Na₂CO₃ solution.

An appropriate indicator, Methyl orange, is used because the equivalence point of a strong acid–weak base titration lies in the acidic range. Methyl orange provides a sharp and clear colour change from yellow to orange-red at the end point.

After determining the exact molarity of the given H₂SO₄ solution, the dilution formula:

𝑀
1
𝑉
1
=
𝑀
2
𝑉
2
M
1
​

V
1
​

=M
2
​

V
2
​


is used again to calculate the volume of concentrated acid required to prepare 500 mL of 0.02 M H₂SO₄ solution using the volumetric method.

This experiment helps students understand:

Acid–base reactions

Standard solutions

Use of indicators

Concept of molarity

Volumetric analysis

Dilution calculations

Accuracy through concordant readings

It also develops laboratory skills such as proper use of burette, pipette handling, and observation of colour change at the correct end point.

📌 Educational Importance (FBISE – PBA)

This experiment strengthens conceptual understanding of:

Neutralization reactions

Primary and secondary standards

End point vs equivalence point

Practical application of molarity formula

Accuracy and precision in titration

It is an essential practical for Grade 12 Chemistry (HSSC I & II) under the FBISE practical-based assessment (PBA) system.

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