What mass of HClO₄ must be present in 0.500 L of solution to obtain a solution with each pH value? a. pH = 2.50 b. pH = 1.50 c. pH = 0.50

Verified step by step guidance

1. insert step 1> Calculate the concentration of hydrogen ions \([H^+]\) using the pH formula: \([H^+] = 10^{-\text{pH}}\). For pH = 1.50, find \([H^+]\).
2. insert step 2> Recognize that perchloric acid \(\text{HClO}_4\) is a strong acid and dissociates completely in water, so \([H^+] = [\text{HClO}_4]\).
3. insert step 3> Use the concentration of \([H^+]\) to find the moles of \(\text{HClO}_4\) in the 0.500 L solution. Use the formula: \(\text{moles} = \text{concentration} \times \text{volume}\).
4. insert step 4> Calculate the molar mass of \(\text{HClO}_4\) by adding the atomic masses of hydrogen, chlorine, and oxygen.
5. insert step 5> Convert the moles of \(\text{HClO}_4\) to mass using the formula: \(\text{mass} = \text{moles} \times \text{molar mass}\).