(a) Interpretation: The value of change in enthalpy for the reaction between NaOH and HCl needs to be determined. Concept introduction: For a reaction as follows: A ⇄ B + C The change in enthalpy can be calculated as follows: Δ H r e a c t i o n = Δ H B + Δ H C − Δ H A Or, change in enthalpy of reaction is equal to difference in the sum of enthalpy of formation of product and sum of enthalpy of formation of reactants.
(a) Interpretation: The value of change in enthalpy for the reaction between NaOH and HCl needs to be determined. Concept introduction: For a reaction as follows: A ⇄ B + C The change in enthalpy can be calculated as follows: Δ H r e a c t i o n = Δ H B + Δ H C − Δ H A Or, change in enthalpy of reaction is equal to difference in the sum of enthalpy of formation of product and sum of enthalpy of formation of reactants.
Solution Summary: The author explains the value of change in enthalpy for the reaction between NaOH and HCl.
The value of change in enthalpy for the reaction between NaOH and HCl needs to be determined.
Concept introduction:
For a reaction as follows:
A⇄B+C
The change in enthalpy can be calculated as follows:
ΔHreaction=ΔHB+ΔHC−ΔHA
Or, change in enthalpy of reaction is equal to difference in the sum of enthalpy of formation of product and sum of enthalpy of formation of reactants.
Interpretation Introduction
(b)
Interpretation:
The value of change in enthalpy for the reaction between NaOH and HF needs to be determined.
Concept introduction:
For a reaction as follows:
A⇄B+C
The change in enthalpy can be calculated as follows:
ΔHreaction=ΔHB+ΔHC−ΔHA
Or, change in enthalpy of reaction is equal to difference in the sum of enthalpy of formation of product and sum of enthalpy of formation of reactants.
Hypochlorous acid, HOCl, is a weak acid having a pKa = 7.46. (a) Show the balanced chemical equation for the hydrolysis of water by OCl- (aq). (b) Compute the value of pKb for aqueous hypochlorite ion. (c) If [OCl-] = 0.050 M, then what is the pH of this aqueous solution?
(a)
(b)
(c)
An acetic acid solution was prepared by dissolving 0.02 moles of acetic acid (HOAC)
in water to give a final volume of 1L. The Ka of HOAC s 1.82 x 10°.
(a) Calculate the pKa of acetic acid
(b) Calculate the pH of the acetic acid solution
(c) If 0.012 moles of concentrated NaOH was added to your prepared solution
from above, what is the new pH (There is no appreciable chareo ine
volumes).
Like any equilibrium constant, Kw changes with temperature. (a) Given that autoionization is endothermic, how does Kw change with rising T ? Explain with a reaction that includes heat as reactant or product. (b) In many medical applications, the value of Kw at 37°C (body temperature) may be more appropriate than the value at 25°C, 1.0 x 10-14. The pH of pure water at 37°C is 6.80. Calculate Kw, pOH, and [OH-] at this temperature.
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell