Titration Techniques in Laboratory Analysis

Titration is a quantitative analytical method used to determine the concentration of analytes through controlled chemical reaction between a standard solution (titrant) and an unknown sample. It is one of the most fundamental and widely used analytical techniques in ISO 17025 accredited laboratories.

Basic Working Principle

A titrant of known concentration is added gradually to a sample until the reaction reaches its equivalence point. The endpoint is detected using an indicator, pH electrode, or potentiometric sensor.

Types of Titration

• Acid–Base Titration – Neutralization reaction between acid and base.
• Redox Titration – Based on oxidation-reduction reactions.
• Complexometric Titration – Uses chelating agents like EDTA.
• Potentiometric Titration – Endpoint detected using electrode potential measurement.
• Precipitation Titration – Formation of insoluble precipitate.

Important Calculations

For acid-base titration:

M₁V₁ = M₂V₂

Where:
M₁ = Molarity of titrant
V₁ = Volume of titrant
M₂ = Molarity of analyte
V₂ = Volume of sample

Common Sources of Error

• Improper burette calibration
• Air bubbles in burette tip
• Incorrect endpoint detection
• Improper standardization of titrant
• Temperature variations affecting reaction kinetics

ISO 17025 Laboratory Relevance

Accredited laboratories must ensure:

• Traceable standard solutions
• Regular burette calibration
• Documented method validation
• Uncertainty estimation
• Proper reagent storage and expiry tracking

Part of Laboratory Engineering Hub

Titration techniques are essential components of laboratory chemical analysis within our complete analyzer engineering framework.

Explore the full Laboratory Engineering reference: Laboratory Analyzers – Engineering Fundamentals