To determine the solubility product constant (Ksp) of a sparingly soluble salt using conductometry, follow these steps:
1. Prepare a saturated solution of the sparingly soluble salt by adding an excess of the salt to a known volume of a solvent (usually water) in a beaker. Stir the solution until no more solute dissolves.
2. Measure the conductivity of the saturated solution using a conductometry apparatus. Record the initial conductivity reading.
3. Gradually add a small amount of a common ion (e.g., chloride ion if the salt is a chloride) to the solution. This will cause a small amount of the sparingly soluble salt to precipitate.
4. Measure the change in conductivity after each addition of the common ion. Record the final conductivity reading when the solution reaches equilibrium again.
5. Use the conductivity values obtained to calculate the solubility of the salt at each point in the experiment.
6. Plot a graph of solubility against concentration of the common ion added. The point of intersection on the x-axis corresponds to the solubility of the sparingly soluble salt. Use this value to calculate the Ksp of the salt using the formula Ksp = [X]^n, where [X] is the molar concentration of the saturated solution and n is the stoichiometry of the salt.
By conducting the above steps, you can determine the solubility product constant (Ksp) of a sparingly soluble salt using conductometry.
How will you find out Ksp of sparingly soluble salt by conductometry
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