A standard solution in a buret is added to an unknown solution in a flask until the reaction reaches its endpoint, signaled by an indicator color change (or pH jump). Initial and final buret readings are used to calculate the unknown molarity.

- See instructions in the links below

Setting up and Performing a Titration - Carolina Science:

📄 How to Perform a Titration - AACT: https://teachchemistry.org/classroom-resources/how-to-perform-a-titration

• Compare indicators (phenolphthalein vs. bromothymol blue) for strong acid–strong base titrations.
• Use a pH probe to create a titration curve and identify equivalence point without an indicator.
• Explore weak acid–strong base (or weak base–strong acid) titrations and note the shifted equivalence pH.
• Perform a back titration when the analyte reacts slowly or is insoluble.

• Wear splash goggles, lab coat/apron, and gloves at all times.
• When diluting, always add acid to water (never water to acid).
• Clamp the burette securely; keep the area dry and uncluttered to prevent slips and spills.
• If acid/base contacts skin, rinse immediately with water and notify the instructor.
• Neutralize and dispose of acidic/basic waste per local regulations; never return chemicals to stock bottles.
• Read burette volumes at eye level to avoid parallax; handle glassware carefully to prevent breakage.

• Why do we choose different indicators for different titrations? (Each indicator changes color over a specific pH range; you select one whose transition range spans the expected equivalence pH.)
• How is equivalence point different from endpoint? (Equivalence point is the stoichiometric point; endpoint is the observed signal - ideally they coincide but may differ slightly.)
• Why add titrant dropwise near the endpoint? (Small additions prevent overshooting, improving accuracy.)
• How does the balanced equation affect the calculation? (Polyprotic acids/bases require multiplying by the number of acidic hydrogens or hydroxides in the stoichiometry.)