Hello, I'm having a few problems with this question.
If 535 mL of gaseous HCL, at 26.5ºC and 747 mmHg, is dissolved in enough water to prepare 625 mL of solution, what is the pH of this solution?
I partially understand what to do for this equation. Use the ideal gas law, PV = nRT, and solve for n. Then somehow use that to find the HCL concentration. Then use Kw = [H30][OH] = 1.0 x 10^-14 and find OH. Finally, use OH concentration to find pH. But each attempt to try to solve this, I am not getting the correct answer. The back of the book answer is, "pH= 1.466".
Thanks for reading, and for any helpful advice or solution.