* HBr (Hydrobromic Acid) is a Strong Acid: It completely dissociates in water, meaning it releases all of its hydrogen ions (H+). This makes it a very strong acid.
* Units of Measurement: 998 likely refers to the number of molecules of HBr, which isn't a useful unit for calculating pH. We need either:
* Moles: The number of moles of HBr present.
* Molarity: The concentration of HBr in moles per liter (mol/L).
Here's how to calculate the pH of a solution with known quantities:
1. Calculate the number of moles of each acid:
* Moles of HNO₃ = (mass of HNO₃) / (molar mass of HNO₃) = 45 g / 63.01 g/mol ≈ 0.714 mol
* You need to provide the mass of HBr to calculate its moles.
2. Calculate the total concentration of H+ ions:
* Both HNO₃ and HBr are strong acids, so they contribute all their H+ ions to the solution.
* [H+] = (moles of HNO₃ + moles of HBr) / (total volume of solution)
* You'll need the volume of the solution in liters (150000 L in this case).
3. Calculate the pH:
* pH = -log[H+]
Example:
Let's say you have 100 grams of HBr.
1. Moles of HBr:
* Moles of HBr = (mass of HBr) / (molar mass of HBr) = 100 g / 80.91 g/mol ≈ 1.237 mol
2. Total concentration of H+ ions:
* [H+] = (0.714 mol + 1.237 mol) / 150000 L ≈ 1.30 x 10^-5 mol/L
3. pH:
* pH = -log(1.30 x 10^-5) ≈ 4.89
Please provide the mass of HBr in grams to get an accurate pH calculation.
