What is the pH of an aqueous solution that contains 2.7 *10²⁰ H₃O⁺ ions per liter of solution? A)2.70 B)3.35 C)6.02 D)10.65 E)11.30

Question

Quizplus · Accepted Answer

To determine the pH of the solution, we need to calculate the concentration of H+ ions. We can do this by using the equation for the ionization of water:
H2O ⇌ H+ + OH-

The equilibrium constant for this reaction is Kw = [H+][OH-] = 1.0 × 10^-14 at 25°C.

We are given the concentration of HSO4- ions in the solution, which can react with water to produce H+ ions:
HSO4- + H2O ⇌ H3O+ + SO42-

The equilibrium constant for this reaction is Ka = [H3O+][SO42-]/[HSO4-] = 1.0 × 10^-2.

We can use the given concentration of HSO4- ions to calculate the concentration of H+ ions:
[HSO4-] = 2.7 × 10^-10 M
[H3O+] = sqrt(Ka × [HSO4-]) = 5.20 × 10^-6 M

Finally, we can use the equation for pH:
pH = -log[H3O+] = 3.35

Therefore, the best choice is B.

What Is the PH of an Aqueous Solution That Contains