[Solved] pH of Aqueous Solution 1. The problem statement, all variables and given/known data Calculate the pH of the following aqueous solution prepared by adding 3.0L HBr(g), measured at 27 degrees Celsius, 757 mmHg pressure, to sufficient water to give 0.10L of solution. 2. Relevant equations pH = -log[H+] 3. The attempt at a solution I'm not sure how to handle a question with gas? Is there another equation I'm supposed to use? The answer says -0.08, which doesn't seem to make sense... I tried to do this question by first writing the equation HBr(g) + H20(l) --> Br- + H30+ I found the number of moles of HBr gas to be 37.07...mol, and this is where my understanding fails me and I have no idea what to do. I even tried using n=cv which didn't work... Please help!