write a net ionic equation to explain the measured pH for any two solutions that have a pH less than 6 or greater than 8

HSO4^-(aq) >H^+(aq) + SO4^-(aq). The solution is acidic with a pH less than 6

CO3^2-(aq) + H2O(l) > HCO3^-(aq) + OH^-(aq) the pH of the solution must be greater than 8.

Explanation:

In a net ionic equation, we are only concerned about showing the particular chemical species that participated in a given reaction. There are other species present in the system of course, but we are focused on a particular chemical reaction so we show the ions that participated in the reaction of interest. The other ions that do not participate in the reaction of interest are called spectator ions.

Let us consider two solutions, one is a solution of NaHSO4 and NaCO3. The important ions when these substances are dissolved in water are; HSO4^- and CO3^2-. Let's see how they affect the pH of the solution.

For NaHSO4 solution;

HSO4^-(aq) >H^+(aq) + SO4^-(aq). The solution is acidic with a pH less than 6

For NaCO3 solution

CO3^2-(aq) + H2O(l) > HCO3^-(aq) + OH^-(aq) the pH of the solution must be greater than 8.

the answer is 0.8m.

by: nicholas