What is the pH of a 0.025M solution of Hydrobromic Acid?
The pH of a solution of hydrobromic acid can be determined using the formula:
pH = -log[H+]
Hydrobromic acid (HBr) dissociates completely in water to produce hydrogen ions (H+).
Since the concentration of hydrobromic acid in the solution is 0.025 M, the concentration of hydrogen ions is also 0.025 M.
pH = -log(0.025) ≈ 1.60
Therefore, the pH of a 0.025 M solution of hydrobromic acid is approximately 1.60.
To determine the pH of a solution of hydrobromic acid (HBr), we must first calculate the concentration of hydronium ions (H3O+) in the solution. Since HBr is a strong acid, it completely dissociates in water to produce H3O+ and bromide ions (Br-). In this case, the concentration of H3O+ will be equal to the concentration of HBr.
Given that the solution has a concentration of 0.025M HBr, the concentration of H3O+ ions is also 0.025M.
The pH of a solution is calculated by taking the negative logarithm (base 10) of the concentration of H3O+ ions:
pH = -log[H3O+]
Substituting the concentration value, we have:
pH = -log(0.025)
Using a calculator, we find that the pH of the 0.025M hydrobromic acid solution is approximately 1.602.