Final answer:
The pH of a 0.005 M solution of hydrogen tetraoxosulphate VI acid, which is sulfuric acid, is approximately 2.3, indicating the solution is acidic.
Step-by-step explanation:
The pH of a 0.005 M hydrogen tetraoxosulphate VI acid, which is also known as sulfuric acid (H2SO4), can be determined by understanding that sulfuric acid is a strong acid and will dissociate completely in water. This means that the concentration of H+ ions in the solution will be equal to the concentration of the sulfuric acid provided. Given that the concentration of H+ ions is 0.005 M, we can calculate the pH using the formula pH = -log[H+].
However, because sulfuric acid is diprotic (can donate two protons), the actual concentration of H+ ions would be higher if both protons were considered. Nevertheless, for this dilute solution, we can assume that only the first proton fully dissociates, and hence the pH would be calculated using the initial 0.005 M concentration for the purposes of a high school level understanding.
pH = -log(0.005)
pH ≈ 2.3
Therefore, the solution would be acidic, as its pH is significantly less than 7.