Answer:
The pH would decrease and the solution would become more acidic
Explanation:
pH of a solution is a measure of its hydronium ion (H3O+) concentration. Mathematically it is given as:
![pH = -log[H3O+] -------(1)\\\\i.e. [H3O+] = 10^{-pH} ------(2)\\](https://tex.z-dn.net/?f=pH%20%3D%20-log%5BH3O%2B%5D%20-------%281%29%5C%5C%5C%5Ci.e.%20%5BH3O%2B%5D%20%3D%2010%5E%7B-pH%7D%20------%282%29%5C%5C)
It is given that pH of the solution = 2.4
Therefore based on equation (2), the [H3O+] would be:
![[H3O+] = 10^{-2.4} = 3.98*10^{-3} M](https://tex.z-dn.net/?f=%5BH3O%2B%5D%20%3D%2010%5E%7B-2.4%7D%20%3D%203.98%2A10%5E%7B-3%7D%20M)
If the [H3O+] concentration were increased then based on equation (1) the pH of the solution would decrease i.e. it would become more acidic.
For example, lets say that the new [H3O+] = 5.0 * 10⁻³ M, then
![pH = -log[5*10^{-3} ] = 2.3](https://tex.z-dn.net/?f=pH%20%3D%20-log%5B5%2A10%5E%7B-3%7D%20%5D%20%3D%202.3)