A chemist dissolves 840.mg of pure hydrobromic acid in enough water to make up 390.mL of solution. Calculate the pH of the solution. Round your answer to 3 significant decimal places.

To calculate the pH of the solution, we first need to find the molarity (M) of the solution. Molarity is defined as the number of moles of solute per liter of solution.

Step 1: Convert milligrams of hydrobromic acid to grams. 840 mg = 0.840 g

Step 2: Convert grams of hydrobromic acid to moles. The molar mass of HBr is approximately 80.91 g/mol. 0.840 g / 80.91 g/mol = 0.0104 mol

Step 3: Convert milliliters of solution to liters. 390 mL = 0.390 L

Step 4: Calculate the molarity of the solution. 0.0104 mol / 0.390 L = 0.0267 M

Hydrobromic acid is a strong acid, so it will completely dissociate in water. Therefore, the concentration of H+ ions is equal to the molarity of the acid.

Step 5: Calculate the pH of the solution using the formula pH = -log[H+]. pH = -log(0.0267) = 1.574

So, the pH of the solution is approximately 1.574 when rounded to three decimal places.