Buffer Simulator
Demystifying the "Buffer Region". Visualize how weak acids and their conjugate bases work together to resist pH changes.
About this simulation
- What
- An interactive Chemistry simulation of Buffer Simulator.
- Who
- Designed for AP, IB, and A‑Level Chemistry students.
- How
- Runs in any modern browser — drag, adjust, and explore in real time.
Updated 2026-01-05
Key Concepts
Common Ion Effect
Adding the salt (A-) suppresses the dissociation of the acid (HA).
Buffering Capacity
The ability of the buffer to neutralize added acid or base is limited by the amount of HA and A- present.
Henderson-Hasselbalch
Connects pKa and the ratio of concentrations to pH.
Understanding Buffer Solutions
A Buffer Solution is a chemical system designed to maintain a stable pH level when small amounts of strong acids or bases are introduced. These solutions are vital to biological systems, such as human blood, where strictly regulated pH is necessary for life processes.
The pH of a buffer is governed by the Henderson-Hasselbalch equation: \(pH = pK_a + \log(\frac{[A^-]}{[HA]})\). This equation defines the relationship between the weak acid's dissociation constant (\(pK_a\)) and the molar ratio of the conjugate base (\(A^-\)) to the weak acid (\(HA\)).
Our interactive simulator allows you to perform virtual titrations, observing how the Common Ion Effect suppresses pH fluctuations within the 'Buffer Region' until the system's buffering capacity is finally exhausted.
Frequently Asked Questions
📚 Read the Guide
Explore the concepts behind this simulation in our detailed article.
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