Sodium hydroxide and hydrochloric acid

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SUMMARY

The discussion focuses on the thermodynamic analysis of the reaction between sodium hydroxide (NaOH) and hydrochloric acid (HCl). Participants explore the calculation of delta H values for three different scenarios: dissolving solid NaOH in water, mixing aqueous NaOH with HCl, and combining solid NaOH with HCl. It is concluded that the delta H values from the first two reactions should approximately equal the delta H of the third reaction, accounting for experimental error.

PREREQUISITES
  • Understanding of thermodynamics and enthalpy changes
  • Familiarity with chemical reactions involving strong acids and bases
  • Knowledge of calorimetry techniques for measuring heat changes
  • Basic skills in handling and preparing solutions of NaOH and HCl
NEXT STEPS
  • Research the principles of calorimetry and its applications in measuring delta H
  • Study the enthalpy of neutralization for strong acid-base reactions
  • Learn about experimental error analysis in thermodynamic measurements
  • Explore the use of Hess's Law in calculating reaction enthalpies
USEFUL FOR

Chemistry students, educators, and laboratory technicians involved in thermodynamics and reaction energetics.

Jan Hill
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Homework Statement


We break down the rxn of NaOH with HCl into putting solid NaOH pellets in water and determine the delta H value. Next, we mix aqueous NaOH with a HCl (aq) and determine the delta H.
Then we mix solid NaOH pellets in HCl(aq) and measure the delta H. Can we say that the delta H values for the first two rxns should add up to roughly the value of the third delta H allowing for some difference due to experimental error?



Homework Equations





The Attempt at a Solution

 
Last edited:
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The answer is '42'.
 

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