Sr(NO3)2 + Na2CO3 ==> SrCO3(s) + 2NaNO3
As long as Na2CO3 is available (not all of it has reacted) adding Sr(NO3)2 forms more and more of the ppt of SrCO3. But even after all of the Na2CO3 is used, then increasing Sr(NO3)2 becomes a common ion and the Ksp dictates that the solubility of the ppt decrease.
How does changing the volume of strontium nitrate solution, added to 8 cm3 of sodium carbonate solution, affect the amount of precipitate formed?
Is it the more the strontium nitrate solution is increased, the more precipate formed?
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