A chemist dissolves 613 mg of pure perchloric acid in enough water to make up 360 mL of solution. Calculate the pH of the solution. Round your answer to 3 significant decimal places.

The first step is to calculate the concentration of the perchloric acid solution in units of moles per liter (M). First, convert the mass of perchloric acid to moles: 613 mg = 0.613 g 0.613 g / 100.996 g/mol (molar mass of HClO4) = 0.00608 mol Next, calculate the molarity of the solution: Molarity (M) = moles of solute / liters of solution M = 0.00608 mol / 0.360 L = 0.0169 M To calculate the pH of the solution, we need to know the concentration of H+ ions. Since perchloric acid is a strong acid, it completely dissociates in water to form H+ and ClO4- ions. Therefore, the concentration of H+ ions in the solution is equal to the molarity of the perchloric acid: [H+] = 0.0169 M Using the equation for pH: pH = -log[H+] pH = -log(0.0169) pH = 1.77 Therefore, the pH of the perchloric acid solution is 1.77.