pH Determination Lab

Comparing Electrolytic Strength

Principle: $pH = -\log_{10}[H_3O^+]$
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Experimental Theory & Guide
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Aim

"To determine and compare the pH of solutions of strong and weak acids (HCl vs. CH₃COOH) and strong and weak bases (NaOH vs. NH₄OH)."

Chemical Logic

$HCl$ Strong Acid (pH 1)
$CH_3COOH$ Weak Acid (pH 3)
$NaOH$ Strong Base (pH 14)
$NH_4OH$ Weak Base (pH 10)

Procedure

  • 1 Select a reagent bottle from the bench.
  • 2 Click on a pH Paper strip to test the drop on a glazed tile.
  • 3 Click on a Test Tube to add the universal indicator solution.

🔬 The Reagent Bench

$HCl$ 0.1M
$CH_3COOH$ 0.1M
$NaOH$ 0.1M
$NH_4OH$ 0.1M
Click a bottle to select a solution

Method 1: Glazed Tile Test

Method 2: Indicator Test

⚠️ Safety

  • HCl and NaOH are corrosive; concentrated ammonia gives off a pungent, irritating vapour. Handle all four with care and never taste them.
  • Use only a drop or two on the pH paper, and add the universal indicator by dropper — do not pipette by mouth.
  • Wear goggles; rinse any splash on skin or eyes with plenty of water at once.
  • Smell ammonia gently by wafting, and keep it stoppered to avoid strong fumes.
  • Dispose of used solutions in the labelled waste container, not the sink.

pH Reference Chart

1
2
3
4
5
6
7
8
9
10
11
12
13
14

Experiment Log

Sample 1
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Sample 2
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Sample 3
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Sample 4
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Observation Journal

Test a solution to record observations…
Ready