Problem: What mass of Ca(NO3)2 must be added to 1.0 L of a 1.0-M HF solution to begin precipitation of CaF2(s)? For CaF2, Ksp = 4.0 X 10 -11 and Ka for HF = 7.2 X 10 -4. Assume no volume change on addition of Ca(NO3)2(s).

FREE Expert Solution

Determine F- concentration first by constructing an ICE Chart.

Ka=productsreactants=[H+][F-][HF]


7.2×10-4=(x)(x)1.0-x

[HF]initialKa=1.0 M7.2×10-4>>500; ignore x in the denominator

7.2×10-4=x21.0-xx2=7.2×10-4x2=7.2×10-4

x = [F-] = 0.0268 M

Calculate Ca2+:

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What mass of Ca(NO3)2 must be added to 1.0 L of a 1.0-M HF solution to begin precipitation of CaF2(s)? For CaF2, Ksp = 4.0 X 10 -11 and Ka for HF = 7.2 X 10 -4. Assume no volume change on addition of Ca(NO3)2(s).

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