Chapter 22, Problem 19STP

To determine

To explain: The chemical equation for dissociation of ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}$ .

Explanation of Solution

Introduction:

Any soluble salt in water gets completely dissociate into respective ions. The overall solution will be neutral as number of hydrogen and hydroxide ions is same and balance each other.

The given salt is ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}$ . It is a soluble salt, so it reacts with water to form respective acid and base. Here, sodium sulphate is formed after the reaction of strong acid-sulfuric acid and strong base-sodium hydroxide.

The reaction is represented as follows:

  ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}\left(s\right)+2{\text{H}}_{\text{2}}\text{O}\left(l\right)\to 2\text{NaOH}\left(aq\right)+{\text{H}}_{\text{2}}{\text{SO}}_4\left(aq\right)$

Since, it is a soluble salt, it gets completely dissociate into sodium and sulfate ions.

Now, dissociation of sodium sulphate in aqueous solution is represented as follows:

  ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}\left(aq\right)\to 2{\text{Na}}^{+}\left(aq\right)+{\text{SO}}_4^{2-}\left(aq\right)$ .

Conclusion:

Thus, the dissociation reaction of sodium sulphate in aqueous solution is:

  ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}\left(aq\right)\to 2{\text{Na}}^{+}\left(aq\right)+{\text{SO}}_4^{2-}\left(aq\right)$