The neutralization of a strong acid and strong base has an enthalpy change, ∆H°, = -55.9 kJ/mol. The net ionic equation for this reaction is H⁺(aq) + OH⁻(aq) ⇌ H₂O(l) which is the reverse of the autoionization of water, and therefore ∆H° for the autoionization of water = +55.9 kJ/mol. Kw for the autoionization of water is 1.0 × 10⁻¹⁴ at 25°C. Distilled water has a [H⁺] = 1.0 × 10⁻⁷ M and a neutral pH of 7.0. Calculate the neutral pH of distilled water at 65°C.
The neutralization of a strong acid and strong base has an enthalpy change, ∆H°, = -55.9 kJ/mol. The net ionic equation for this reaction is H⁺(aq) + OH⁻(aq) ⇌ H₂O(l) which is the reverse of the autoionization of water, and therefore ∆H° for the autoionization of water = +55.9 kJ/mol. Kw for the autoionization of water is 1.0 × 10⁻¹⁴ at 25°C. Distilled water has a [H⁺] = 1.0 × 10⁻⁷ M and a neutral pH of 7.0. Calculate the neutral pH of distilled water at 65°C.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The neutralization of a strong acid and strong base has an enthalpy change, ∆H°, = -55.9 kJ/mol. The net ionic equation for this reaction is H⁺(aq) + OH⁻(aq) ⇌ H₂O(l) which is the reverse of the autoionization of water, and therefore ∆H° for the autoionization of water = +55.9 kJ/mol. Kw for the autoionization of water is 1.0 × 10⁻¹⁴ at 25°C. Distilled water has a [H⁺] = 1.0 × 10⁻⁷ M and a neutral pH of 7.0. Calculate the neutral pH of distilled water at 65°C.
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