gen-briefly-explain-acid-base-titration-and-one-common-misconcep-6c58

Briefly explain acid-base titration and one common misconception about it.

# Acid-Base Titration **What it is:** Acid-base titration is a laboratory technique used to determine the unknown concentration of an acid or base by gradually adding a solution of known concentration (the titrant) until the reaction reaches its equivalence point—where moles of acid equal moles of base. **How it works:** A burette slowly dispenses the titrant into a flask containing the unknown solution plus an indicator (or pH meter). The indicator changes color at the endpoint, signaling that neutralization is complete. Using the volume and concentration of titrant added, you can calculate the unknown concentration. ## Common Misconception **"The equivalence point always occurs at pH 7"** Many students assume neutralization means pH 7, but this is only true for strong acid-strong base titrations. The actual equivalence point pH depends on the strength of the acid and base: - **Strong acid + strong base** = pH 7 - **Weak acid + strong base** = pH > 7 (basic) - **Strong acid + weak base** = pH < 7 (acidic) This happens because the salt formed can undergo hydrolysis, affecting the final pH. Choosing the correct indicator requires knowing the expected equivalence point pH for your specific titration.