Heat of Neutralization
Heat of Neutralization for an acid-base reaction
Contents:
- Abstract
- Introduction
- Results and Discussions
- Conclusion
- References
Abstract:
In the experimental procedure we will measure the heat of neutralization when an acid and base react to form 1 mole of water. This quantity of heat is measured experimentally by allowing the reaction to take place in a thermally insulated Styrofoam cup calorimeter. The heat liberated in the neutralization reaction will cause an increase in the temperature of the solution and of the calorimeter.
Introduction:
What is Heat of Neutralization:
The heat of neutralization is the energy change when one mole of water is formed from the neutralization between one mole of hydrogen ions, H+ from an acid and one mole of hydroxide ions, OH- from a base.
Another definition, Neutralization reaction refers to acid and base reaction producing salt and water.
Acid + Base → Salt + Water
Some definitions used in the study of neutralization reaction are :
Equivalence point : The state of acid base reaction when acid and base react in exact equivalent amounts as determined theoretically.
End point : The state of acid base reaction when acid and base react in exact equivalent amounts as determined practically (during titration). Clearly, end point volume measurement is slightly greater than that corresponding to equivalence point.
Neutral point : The state of acid-base reaction when product solution is neutral (pH=7).
Heat of neutralization between different strength of Acid and Base:
Theory for the heat of neutralization:
where QNeutralization is quantity of heat, m is the mass of the solution ,and S.P. is the specific heat capacity of the solution, and ∆T is the temperature change observed during the reaction.
Results and Discussions:
Objective:
to detemine the heat of nutrilization for this Acid - Base reaction:
NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l) +
Contents:
- Abstract
- Introduction
- Results and Discussions
- Conclusion
- References
Abstract:
In the experimental procedure we will measure the heat of neutralization when an acid and base react to form 1 mole of water. This quantity of heat is measured experimentally by allowing the reaction to take place in a thermally insulated Styrofoam cup calorimeter. The heat liberated in the neutralization reaction will cause an increase in the temperature of the solution and of the calorimeter.
Introduction:
What is Heat of Neutralization:
The heat of neutralization is the energy change when one mole of water is formed from the neutralization between one mole of hydrogen ions, H+ from an acid and one mole of hydroxide ions, OH- from a base.
Another definition, Neutralization reaction refers to acid and base reaction producing salt and water.
Acid + Base → Salt + Water
Some definitions used in the study of neutralization reaction are :
Equivalence point : The state of acid base reaction when acid and base react in exact equivalent amounts as determined theoretically.
End point : The state of acid base reaction when acid and base react in exact equivalent amounts as determined practically (during titration). Clearly, end point volume measurement is slightly greater than that corresponding to equivalence point.
Neutral point : The state of acid-base reaction when product solution is neutral (pH=7).
Heat of neutralization between different strength of Acid and Base:
Theory for the heat of neutralization:
where QNeutralization is quantity of heat, m is the mass of the solution ,and S.P. is the specific heat capacity of the solution, and ∆T is the temperature change observed during the reaction.
Results and Discussions:
Objective:
to detemine the heat of nutrilization for this Acid - Base reaction:
NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l) +
References: 1. http://cnx.org/content/m17138/latest/ 2. http://en.wikipedia.org/wiki/Neutralization_(chemistry) 3. http://en.wikipedia.org/wiki/Enthalpy_of_neutralization 4. http://en.wikipedia.org/wiki/Neutralization_reaction 5. http://ar.scribd.com/doc/60696670/Thermochemistry-Heat-of-Neutralization 6. Practical General Chemistry For Engineering, p 36-39 .