A chemist dissolves 413.mg of pure hydrobromic acid in enough water to make up 250.mL of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits.

Sure, here are the steps to calculate the pH of the solution:

1. First, we need to convert the mass of hydrobromic acid (HBr) to moles. Hydrobromic acid has a molar mass of approximately 80.91 g/mol. So, 413 mg is equal to 0.413 g. Therefore, the number of moles of HBr is 0.413 g / 80.91 g/mol = 0.0051 mol.

2. Next, we calculate the molarity of the solution. Molarity is defined as the number of moles of solute per liter of solution. Since we have 0.0051 mol of HBr in 0.250 L of solution, the molarity is 0.0051 mol / 0.250 L = 0.0204 M.

3. Hydrobromic acid is a strong acid, which means it completely dissociates in water. Therefore, the concentration of H+ ions is equal to the molarity of the HBr solution, which is 0.0204 M.

4. The pH of a solution is calculated using the formula pH = -log[H+], where [H+] is the concentration of H+ ions in moles per liter. So, the pH of the solution is -log(0.0204) = 1.69.

Therefore, the pH of the solution is 1.69.