A solution containing sodium fluoride is mixed with one containing calcium nitra

Question

A solution containing sodium fluoride is mixed with one containing calcium nitrate to form a solution that is 0.015 M in NaF and 0.010 M in Ca(NO3)2. Will a precipitate form in the mixed solution? If so, identify the precipitate. I saw a worked out problem like this in my text. I know the answer is CaF2--but I don't understand how if the Ksp isn't given you can know that Q is greater than or less that Ksp. Could you explain that to me? Also, how do you know to calculate Q for just CaF2, and not also NaNO3?

Explanation / Answer

Yes, you are correct in your first statement that the solubility product must be given for its comparison with the ionic product. It is generally taken from the data.

Now, for calculating the Ionic product we need to calculate the concentration of both the ions and then find the ionic product to compare it with solubility product.

If Ionic Product >Solubility Product Precipitation occurs.

and if reverse happens then precipitaion does not take place.

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