Did a solubility product constant for a sparingly soluble salt. Directions were:

Question

Did a solubility product constant for a sparingly soluble salt. Directions were: Accurately prepare three solutions in separate 150mm test tubes by adding 5ml of 0.0040 M AgNO3 to 5mL of 0.0024 M K2CrO4. Transfer approximately 3mL of each solution along with most of the insoluble Ag2CrO4 to 75mm test tubes and centrifuge. Discard the supernatant liquid and retain the precipitate as directed. To each test tube add 2mL of .25 M NaNO3. Mix, centrifuge, and discard supernatant liquid. Add 2mL of .25 M NaNo3 o each of the test tubes, mis, and establish equilibirum. I have to fill out this chart: Absorbance CrO42- Ag+ Ksp of Ag2CrO4 1.398 1 1 1 1.413 2. 2 2 1.622 3 3 3 375mm

Explanation / Answer

As per defination. Solubility product is constant for a particular salt(or sparingly soluble salt) at a fixed temperature. l.e it depends only on temperature.. However the value of solubility product of sparingly soluble salt also depends upon the concentration of respective ions.So if you add a salt having same ion in common with sparingly soluble salt,it shifted the the position of equilibrium ( exist between sparingly soluble salt and it's ion in solution) towards left ,I.E ,towards salt.hence the concentration of ion decrease and it lowers the value of solubility product.This phenomena also known as COMMON ION EFFECT...similarly if you add a soluble salt having no common ion with the sparing soluble salt, then it will increase the value of the solubility product,due to increase of ionic strength..this is called SALT EFFECT.

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