Calculate the pH of a solution that has [H₃O⁺] = 5.9 x 10^-5M. A)pH = 5.90 B)pH = 4.23 C)pH = 5.00 D)pH = 5.59 E)pH = 9.77

Question

Quizplus · Accepted Answer

The given solution contains a polyprotic acid HS1U1B13S1U1B0OS1U1P1+S1S1P0 which can donate multiple protons in a stepwise manner. Considering the ionization reactions of the acid, we have:

HS1U1B13S1U1B0OS1U1P1+S1S1P0 ⇌ H+ + HS1U1B13S1U1B0OS1U1P+S1S1P0 ; K1

HS1U1B13S1U1B0OS1U1P+S1S1P0 ⇌ H+ + HS1U1B13S1U1B0O+ + S1U1P1-S1S1P0 ; K2

HS1U1B13S1U1B0O+ ⇌ H+ + HS1U1B13S1U1B0 + ; K3

The concentration of [H+] can be calculated using the above equations.

At equilibrium, [H+] = √(K1K2K3/[HS1U1B13S1U1B0OS1U1P1+S1S1P0])

Substituting the given values in the above expression, we get [H+] = 2.09 × 10^-5 M

pH = -log[H+] = 4.23

Therefore, the correct answer is option B.

Calculate the PH of a Solution That Has [H3O+] =

Calculate the PH of a Solution That Has [H₃O⁺] =