Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Win,odd Dhamnekar on July 05, 2021, 06:21:24 AM
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1)Calculate the mass of CaF2 produced when 5g of Ca(NO3)2 is mixed with 3g of NaF in water, with a final volume of 500 mL. Ksp is 3.5E-11 for the system.
My attempt to answer: Reaction equation is Ca(NO3)2 + 2NaF :rarrow: CaF2 + 2NaNO3
We have 5/164.088 moles of Ca(NO3)2 and 3/41.9882 moles of NaF
How to answer this question?
2)What is the intention of the questioner to include highlighted portion in the question?
(Note:You can see that the highlighted portion of information is not useful in answering this question.)
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1)Calculate the mass of CaF2 produced when 5g of Ca(NO3)2 is mixed with 3g of NaF in water, with a final volume of 500 mL. Ksp is 3.5E-11 for the system.
My attempt to answer: Reaction equation is Ca(NO3)2 + 2NaF :rarrow: CaF2 + 2NaNO3
We have 5/164.088 moles of Ca(NOF3)2 and 3/41.9882 moles of NaF
How to answer this question?
1. Calculate mass of precipitated CaF2.
2. Using solubility product calculate how much Ca2+ can dissolve in NaF solution.
3. Mass of CaF2 residue is reduced by this soluble part.
2)What is the intention of the questioner to include highlighted portion in the question?
(Note:You can see that the highlighted portion of information is not useful in answering this question.)
It is direct answer that formation of solid OsO4 is more exotermic - nothing more.
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CaF2 ::equil:: Ca2+ +2F-, Ksp=[Ca2+] + [2F-]2 [itex]\implies[/itex] ,Q=[0.061]*[2*0.143]2=4.97e-3
Q> Ksp, , so, CaF2 will precipitate if its mass > 2.38 grams
Are this workings correct answers to your point 2) and 3)?
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Solubility of CaF2 is very low (does not change mass of the residue), so you are right.
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Ksp = [Ca2+][F-]2. Do not multiply the concentration of F- by 2!
If, and only if, CaF2 is the only source of calcium and fluoride ions, then if the concentration of CaF2 is C, [Ca2+] = C and [F-] = 2C (that's where a factor of 2 comes in) and Ksp = 4C3. You can't use this when there are other sources of the ions.
Where do you get the figure of 2.38 g? I calculate the solubility to be 8 mg in 500 mL. (confirmed by looking it up)
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@mjc123 - 2,38 g is the mass of precipitate.
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Oh, I see. Then the statement "CaF2 will precipitate if its mass > 2.38 grams" is wrong.