Calculate [H₃O⁺] and [OH^–] for each solution at 25 °C. b. pH = 11.23 c. pH = 2.87

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Hello. In this problem, we are asked to determine the values of the hydro nea mine and hydroxide ion concentrations for a solution with a ph of 8.92 at 25 degrees Celsius, we call at 25 degrees Celsius. The Ph plus the P O H is equal to 14. So our P O H then is equal to 14 minus the PH Which is equal to 8.92. So our POH is 5.08. We can find the hydrogen ion concentration By taking 10 to the -4. So this is then 10 to the negative 8.92 Which works out to 1.2 times 10 to the -9 moller. And then our hydroxide ion concentration is equal to 10 to the negative P O H. So this is equal to 10 to the negative 5.08, Which is equal to 8.3 times 10 to the -6 smaller. So we could also do a check on our work 25°C. Then iron product constant of water should be equal to one times 10 to the minus 14. So we can plug in what we found and verify then that the hydro mine and hydroxide ion concentration are 1.2 times 10 minus nine moller and 8. times 10 to minus six Mohler. Respectfully. Thanks for watching. Hope this helps.

Calculate [H₃O⁺] and [OH^–] for each solution at 25 °C. b. pH = 11.23 c. pH = 2.87

Verified Solution

Key Concepts

pH Scale

Ion Product of Water (Kw)

Hydronium and Hydroxide Ion Concentrations

Calculate [H3O+] and [OH–] for each solution at 25 °C. b. pH = 11.23 c. pH = 2.87

Verified Solution

Key Concepts

pH Scale

Ion Product of Water (Kw)

Hydronium and Hydroxide Ion Concentrations

Calculate [H₃O⁺] and [OH^–] for each solution at 25 °C. b. pH = 11.23 c. pH = 2.87