3. 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.
Ksp (CaF2)= 1.46 x 10 -10
Does a precipitate form in the mixed solution? If so, identify the precipitate.
Please show the steps to reaching the solution or why it is so. Thank you.
molarity of [F-] from NaF = 0.015 M
molarity of Ca+2 from Ca(NO3)2 = 0.010 M
CaF2---------------> Ca+2 + 2F-
Q = [Ca+2] [F-]^2
Q = (0.010) (0.015)^2
Q = 2.25 x 10^-6
Ksp value is given
Ksp = 1.46 x 10^-10
Q > Ksp . so there will be precipitate formed
the precipitate = CaF2
note :
1) if Q > Ksp --------------> precipitate will form
2) if Q < Ksp ------------> no precipitate
3) if Q = Ksp -------------> saturated solution and ready to form precipitate
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