Why do solutions of barium chloride, and barium fluoride give rise to solutions with different $p H$ $pH$ values?

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Why do solutions of barium chloride, and barium fluoride give rise to solutions with different $p H$ $pH$ values?

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Answer 1 · 2017-05-18T03:47:58

Because $fluoride ion$ $"fluoride ion"$ undergoes hydrolysis in aqueous solution.

Explanation:

Consider the solubility equilibrium for $B a F_{2}$ $BaF_2$ :

$B a F_{2} (s) ⇌ B a^{2 +} + 2 F^{-}$ $BaF_2(s) rightleftharpoonsBa^(2+) + 2F^-$

Fluoride is moderately basic.............

$F^{-} + H_{2} O ⇌ H F (a q) + H O^{-}$ $F^(-) + H_2O rightleftharpoons HF(aq) + HO^-$

Addition of $H_{3} O^{+}$ $H_3O^+$ will drive these equilibria to the right as written, and MORE barium salt will go into solution.

On the other hand, $chloride ion$ $"chloride ion"$ , A WEAK BASE, does not speciate in solution, and is inert to added acid.

Note that had we $K_{sp}$ $K_"sp"$ data for $B a F_{2} (s)$ $BaF_2(s)$ , and $K_{a}$ $K_a$ data for $H F$ $HF$ we could solve the solubility equilibrium precisely, and develop an expression for solubility that depends on $p H$ $pH$ .

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Why do solutions of barium chloride, and barium fluoride give rise to solutions with different $p H$ $pH$ values?

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Science

Math

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Why do solutions of barium chloride, and barium fluoride give rise to solutions with different pHpH values?

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Explanation:

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Why do solutions of barium chloride, and barium fluoride give rise to solutions with different $p H$ $pH$ values?