1
$\begingroup$

Is $\ce{NaCl}$ in water aqueous? For a certain amount of $\ce{NaCl}$, it can dissolve in water but if you add more $\ce{NaCl}$ it can't dissolve any more.

So, if in a certain reaction $\ce{NaCl}$ is formed with water:

$$\ce{HCl(aq) + NaOH(aq) -> H2O(l) + NaCl(aq)}$$

My question is does $\ce{NaCl}$ in the previous reaction totally dissolve in the water formed? Or in other words is this equation correct?

$$\ce{HCl(aq) + NaOH(aq) -> H2O(l) + NaCl(aq) + NaCl(s)}$$

Another question is why do we write (l) beside water rather than (aq) since it's part of the aqueous solution?

Improve this question
$\endgroup$
1
  • $\begingroup$ I have improved the formatting of your post using $\LaTeX$. For more information on how to do this yourself please see here and here. $\endgroup$
    – bon
    Commented Jun 28, 2015 at 16:09

1 Answer 1

Reset to default
1
$\begingroup$

When we are considering $\ce{HCl(aq)}$ and $\ce{NaOH(aq)}$. the system contain sufficient amount amount of solvent water molecules in situ already present and this is more than sufficient to hydrate the produced $\ce{NaCl}$ in the reaction. Hence the first equation
$$\ce{HCl(aq) + NaOH(aq) -> NaCl(aq) + H2O(l)}$$

will be the correct expression.

Improve this answer
$\endgroup$
1
  • $\begingroup$ I have improved the formatting of your post using $\LaTeX$. For more information on how to do this yourself please see here and here. $\endgroup$
    – bon
    Commented Jun 28, 2015 at 16:11

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service and acknowledge you have read our privacy policy.

Not the answer you're looking for? Browse other questions tagged or ask your own question.