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Chapter 15: Q39 E (page 873)

What [F-] is required to reduce [Ca2+] to 1.0×10-4M by precipitation of CaF2?

Short Answer

Expert verified

The required [F-] = 6.2 ×10-4M

Step by step solution

01

Define  Ksp

The solubility product constant is the equilibrium constant for the dissolution of a solid substance into an aqueous solution. It is denoted by the symbol

02

Determining F- for deduction

Substituting in solubility product

\[{K_{sp}}=3.9\times1{0^{-11}}\]

= [Ca2+] [F-]2

=1×10-4[F-]2

03

Determining the precipitation [F-]

\[\left[{{F^-}}\right]=\sqrt{\frac{{3.9\times1{0^{-11}}}}{{1\times1{0^{-4}}}}}=6.2\times1{0^{-4}}M\]

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