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

Answer 1

#HI(aq) + KOH(aq) rarr KI(aq) + H_2O(l)#

Furthermore, the net ionic equation is less complicated:

#H_3O^+ + HO^(-) rarr 2H_2O(l)#

But what do we mean by #HI(aq)#? The #(aq)# designation means the socalled #"aquated ion"#. In water, hydrogen iodide speciates to #H_3O^+# and #I^-#. So-called hydronium ion, #H_3O^+#, as far as anyone knows, is a cluster of water molecules, with an EXTRA proton, #H_9O_4^+# or #H_11O_5^+# or something similar.

This water cluster not only holds for the hydronium ion, but potassium ion, #K^(+)(aq)#, is probably #[K(OH_2)_6]^+#, or #Cl(aq)^-# #[Cl(H_2O)_(4-6)]^-#.

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Answer 2

Ellie Andrews

Net Ionic Equation: (2H^+(aq) + 2OH^-(aq) \rightarrow 2H_2O(l)) Complete Ionic Equation: (2HI(aq) + 2KOH(aq) \rightarrow 2KI(aq) + 2H_2O(l))

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.