Question

use the references to access important values if needed for this question.
write the net ionic equation for the acid - base hydrolysis equilibrium that is established when calcium fluoride is dissolved in water.
(use the lowest possible coefficients. be sure to specify states such as (aq) or (s). if a box is not needed, leave it blank.)
\\( \square + \mathrm { h } _ { 2 } \mathrm { o } ( l ) \
ightleftharpoons \square + \square \\)
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Explanation:

Step1: Analyze the dissociation of calcium fluoride

Calcium fluoride (\(CaF_2\)) dissociates in water as \(CaF_2(s)
ightleftharpoons Ca^{2 +}(aq)+2F^{-}(aq)\). The \(Ca^{2+}\) is the cation of a strong base (\(Ca(OH)_2\)) and does not hydrolyze. The \(F^{-}\) is the anion of a weak acid (\(HF\)) and will hydrolyze.

Step2: Write the hydrolysis reaction of \(F^{-}\)

The \(F^{-}\) ion reacts with water (\(H_2O\)) in a hydrolysis reaction. The reaction is \(F^{-}(aq)+H_2O(l)
ightleftharpoons HF(aq)+OH^{-}(aq)\)

Answer:

\(F^{-}(aq)+H_2O(l)
ightleftharpoons HF(aq)+OH^{-}(aq)\)