If the ionization constant of water,K_w,at 40°C is 2.92 × 10^-14,then what is the hydronium ion concentration for a neutral solution? A)[H₃O⁺] 1.71 × 10^-7 M C)[H₃O⁺] = 1.71 × 10^-7 M D)[H₃O⁺]

Question

If the ionization constant of water,K_w,at 40°C is 2.92 × 10^-14,then what is the hydronium ion concentration for a neutral solution? A)[H₃O⁺] < 1.00 × 10^-7 M B)[H₃O⁺] > 1.71 × 10^-7 M C)[H₃O⁺] = 1.71 × 10^-7 M D)[H₃O⁺] < 1.71 × 10^-7 M

Quizplus · Accepted Answer

For a neutral solution, the concentration of hydronium ions [H3O+] is equal to the concentration of hydroxide ions [OH-]. The ionization constant of water (Kw) at 40°C is given as 2.92 × 10^-14. Since Kw = [H3O+][OH-], and [H3O+] = [OH-] in a neutral solution, we can solve for [H3O+] by taking the square root of Kw. √(2.92 × 10^-14) = 1.71 × 10^-7 M, which means the concentration of hydronium ions in a neutral solution at 40°C is 1.71 × 10^-7 M.

If the Ionization Constant of Water,Kw,at 40°C Is 2

If the Ionization Constant of Water,K_w,at 40°C Is 2