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Question: Conductometric titration of a strong acid with a strong base
Conductometric titration is a type of titration in which the electrolytic conductivity of the reaction mixture is continuously monitored as one reactant is added. The equivalence point is the point at which the conductivity change is the greatest. This process can be used in the titration of a strong acid with a strong base. Here are the steps you need to follow: 1. Preparation of solutions: Prepare the solutions of the strong acid (like HCl or H2SO4) and strong base (like NaOH or KOH). 2. Calibration: Calibrate your conductometer using a known solution. Follow the manufacturer's instructions for this step. 3. Set up the experiment: Fill the burette with the base. Usually, the base is placed in the burette and the acid in the beaker. Place the conductivity sensor immersed in the beaker containing the acid solution. 4. Begin the titration: Add the base to the acid solution slowly, drop by drop. Monitor and record the conductivity after each addition. 5. Plot the data: Plot a graph of conductivity against the volume of base added. 6. Analysis of results: The point of inflection on your graph is the equivalence point, this is where moles of acid are equal to moles of base added. Advice: Carry out the titration at constant temperature because the degree of ionization of water and mobility of ions depend on temperature. Safety precautions: Always follow safety protocols while conducting these experiments including wearing proper lab attire (lab coat, goggles, gloves etc.) and handling all chemicals with care, particularly strong acids and bases.
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