# Question 7f6cb

Feb 21, 2017

I'd go for no reaction, but I suspect that the answer is 4. dissociation.

#### Explanation:

Potassium chloride, $\text{KCl}$, and sodium hydroxide, $\text{NaOH}$, are both soluble ionic compounds, so you can expect them to exist as ions in aqueous solution.

${\text{KCl"_ ((aq)) -> "K"_ ((aq))^(+) + "Cl}}_{\left(a q\right)}^{-}$

${\text{NaOH"_ ((aq)) -> "Na"_ ((aq))^(+) + "OH}}_{\left(a q\right)}^{-}$

Now, the problem with mixing these two solutions is that the products are soluble ionic compounds as well, which means that the ions will continue to exist as ions in the resulting solution.

That is the case because all ionic compounds that contain group 1 elements (sodium, $\text{Na}$, and potassium, $\text{K}$, in your case) are soluble in water.

Sodium chloride, $\text{NaCl}$, and potassium hydroxide, $\text{KOH}$, are soluble in aqueous solution, so they will not be formed by this reaction.

In other words, no reaction will take place when you mix these two solutions.

${\text{K"_ ((aq))^(+) + "Cl"_ ((aq))^(-) + "Na"_ ((aq))^(+) + "OH"_ ((aq))^(-) -> "Na"_ ((aq))^(+) + "Cl"_ ((aq))^(-) + "K"_ ((aq))^(+) + "OH}}_{\left(a q\right)}^{-}$

Notice that all the ions are present on both sides of the chemical equation, which tells you that no reaction is taking place, i.e. they are all spectator ions.

"KCl"_ ((aq)) + "NaOH"_ ((aq)) -> color(red)("N. R.")#

Here $\textcolor{red}{\text{N. R.}}$ stands for no reaction.

That said, you can say that the two compounds dissociate completely when dissolved in water, so maybe the answer could be 4. dissociation.

If that's the case, then the question could have been worded better. Each compound dissociates in its own aqueous solution, so you can't really say that the two dissociate because the react with each other.