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17. Acid and Base Equilibrium

Auto-Ionization

17. Acid and Base Equilibrium

Auto-Ionization

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Auto-Ionization and Kw

Auto-Ionization and Kw

Kw Temperature Dependence

Kw Temperature Dependence

Auto-Ionization Example

Auto-Ionization Example

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Multiple Choice
Chemistry student prepared an aqueous solution at 30ºC. If the solutions contains 7.42 × 10⁻⁹ M of hydroxide ions, calculate the pH.
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Multiple Choice
Calculate the K_w of pure water given the pH = 6.34.
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Textbook Question
The average pH of normal arterial blood is 7.40. At normal body temperature 137 °C2, Kw = 2.4 * 10-14. Calculate 3H+4, 3OH-4, and pOH for blood at this temperature.
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Textbook Question
Like all equilibrium constants, the value of K_w depends on temperature. At body temperature (37 °C), K_w = 2.4×10^–14. What are the [H₃O⁺] and pH of pure water at body temperature?
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Open Question
What is the pH of pure water at 40.0°C if the K_w at this temperature is 2.92 × 10^-14?
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Open Question
The pOH of a basic solution is 5.63. What is [OH^-]?
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Multiple Choice
At 60 °C, the value of KW is 1.3×10⁻¹³. What is the concentration of H₃O⁺ in a neutral solution at 60 °C?
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Multiple Choice
At 60°C, the ion product constant of water, Kw, is 9.61 x 10^-14. What is the pH of pure water at this temperature?
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