Final answer:
To find the pH of a 5.1×10−6 M HBr solution, you take the negative logarithm of its hydrogen ion concentration. Since HBr is a strong acid that fully dissociates, the pH is -log(5.1×10−6) or approximately 5.29.
Step-by-step explanation:
To calculate the pH of a 5.1×10−6 M HBr solution, we use the formula:
pH = -log[H+]
Since HBr is a strong acid, it completely dissociates in water, releasing hydrogen ions (H+) equal to its concentration. Thus, the concentration of hydrogen ions [H+] in the solution is 5.1×10−6 M.
Now, we can use the given information to find the pH:
pH = -log(5.1×10−6)
When calculated, the pH approximately equals:
pH = 5.29
Therefore, the pH of the solution is 5.29, which corresponds to choice (a).