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

Nov 9, 2016

$H I \left(a q\right) + K O H \left(a q\right) \rightarrow K I \left(a q\right) + {H}_{2} O \left(l\right)$

#### Explanation:

And the net ionic equation is rather simpler:

${H}_{3} {O}^{+} + H {O}^{-} \rightarrow 2 {H}_{2} O \left(l\right)$

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

This water cluster not only holds for the hydronium ion, but potassium ion, ${K}^{+} \left(a q\right)$, is probably ${\left[K {\left(O {H}_{2}\right)}_{6}\right]}^{+}$, or $C l {\left(a q\right)}^{-}$ ${\left[C l {\left({H}_{2} O\right)}_{4 - 6}\right]}^{-}$.