📖 Theory & Concepts ▼

Acid-Base Titration

H₂C₂O₄ + 2NaOH → Na₂C₂O₄ + 2H₂O
Primary Standard: Oxalic acid (exact concentration known)
Secondary Standard: NaOH (standardized against primary)
Indicator: Phenolphthalein (colorless → pink at endpoint)

Key Formulas

N₁V₁ = N₂V₂ (at equivalence point)
Normality = Molarity × n-factor
Oxalic acid n-factor = 2 (dibasic)

Tips for Accuracy

  • • Remove air bubbles from burette before starting
  • • Rinse burette with NaOH before filling
  • • Swirl flask continuously while adding titrant
Did you know? The word "titration" comes from the French word "titre" meaning "title" or "rank" - originally used to describe determining the purity of gold!

🎯 Objective

Determine the strength of NaOH solution by titrating against standard oxalic acid using phenolphthalein indicator.

Procedure

1. Prepare 0.1N oxalic acid
2. Fill burette with NaOH
3. Add indicator to flask
4. Titrate until pink color
5. Note burette reading

Theory

H₂C₂O₄ + 2NaOH → Na₂C₂O₄ + 2H₂O
Endpoint
Colorless → Pale Pink
Formula
N₁V₁ = N₂V₂
Initial Reading
0.0 mL
Current Reading
0.0 mL
Volume Used
0.0 mL
Current trial
Rough trial
Meniscus check
0.0 mL at eye level
Endpoint cue
Add indicator first
Burette (NaOH)
01020304050
20 mL Oxalic Acid (0.1N)
No indicator added

📊 Titration Readings

# Type Initial Final Vol Use
No readings yet
Lab Notebook
Observations will appear here...

Concordance Check

Do one rough trial, then collect two close accurate titres within 0.1 mL.