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: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter14: Acids And Bases
Section: Chapter Questions
Problem 67QRT: Complete each of these reactions by filling in the blanks. Predict whether each reaction is...
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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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