How do we represent the complete, and net ionic equations for the reaction between hydrogen iodide, and potassium hydroxide?

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How do we represent the complete, and net ionic equations for the reaction between hydrogen iodide, and potassium hydroxide?

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Answer 1 · 2016-11-09T07:02:49

$H I (a q) + K O H (a q) \to K I (a q) + H_{2} O (l)$ $HI(aq) + KOH(aq) rarr KI(aq) + H_2O(l)$

Explanation:

And the net ionic equation is rather simpler:

$H_{3} O^{+} + H O^{-} \to 2 H_{2} O (l)$ $H_3O^+ + HO^(-) rarr 2H_2O(l)$

But what do we mean by $H I (a q)$ $HI(aq)$ ? The $(a q)$ $(aq)$ designation means the socalled $aquated ion$ $"aquated ion"$ . In water, hydrogen iodide speciates to $H_{3} O^{+}$ $H_3O^+$ and $I^{-}$ $I^-$ . So-called hydronium ion, $H_{3} O^{+}$ $H_3O^+$ , as far as anyone knows, is a cluster of water molecules, with an EXTRA proton, $H_{9} O_{4}^{+}$ $H_9O_4^+$ or $H_{11} O_{5}^{+}$ $H_11O_5^+$ or something similar.

This water cluster not only holds for the hydronium ion, but potassium ion, $K^{+} (a q)$ $K^(+)(aq)$ , is probably ${[K {(O H_{2})}_{6}]}_{6}^{+}$ $[K(OH_2)_6]^+$ , or $C l {(a q)}^{-}$ $Cl(aq)^-$ ${[C l {(H_{2} O)}_{4 - 6}]}_{4 - 6}^{-}$ $[Cl(H_2O)_(4-6)]^-$ .

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How do we represent the complete, and net ionic equations for the reaction between hydrogen iodide, and potassium hydroxide?

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