Determine the pH of each solution. a. 0.048 M HI b. 0.0895 M HClO₄ c. a solution that is 0.045 M in HClO₄ and 0.048 M in HCl d. a solution that is 1.09% HCl by mass (assume a density of 1.01 g/mL for the solution)

Verified step by step guidance

1. <strong>Step 1:</strong> Understand the nature of the acids involved. HI and HClO₄ are strong acids, meaning they dissociate completely in water. This means the concentration of H⁺ ions in the solution is equal to the concentration of the acid.
2. <strong>Step 2:</strong> Calculate the pH for each solution using the formula: \( \text{pH} = -\log[\text{H}^+] \). For part (a), use the concentration of HI, which is 0.048 M.
3. <strong>Step 3:</strong> For part (b), use the concentration of HClO₄, which is 0.0895 M, to find the pH using the same formula.
4. <strong>Step 4:</strong> For part (c), since both HClO₄ and HCl are strong acids, add their concentrations to find the total [H⁺] and then calculate the pH.
5. <strong>Step 5:</strong> For part (d), convert the percentage concentration of HCl to molarity. Use the formula: \( \text{Molarity} = \frac{\text{mass percent} \times \text{density} \times 10}{\text{molar mass of HCl}} \). Then, calculate the pH using the molarity obtained.