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A thermometric titration - determine the concentrations of hydrochloric acid and ethanoic acids by thermometric titration and find the enthalpy of neutralization.

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Introduction

Experiment 12 ~ A thermometric titration ~ Lab Report Aim: To determine the conecentrations of hychloric acid and ethanoic acis by thermometric titration and find the enthalpy of neutralization. Procedure: (I) Titration of HCL with standard NaOH: 1. 50cm3 of NaOH solution is pipetted and transfer to the polystyrene cup, It was allow to stand for a few minutes. 2. The initial temperature was recorded. 5.0 cm3 ofHCL was burette to the cup. 3. The mixture was stirred well by using the thermometer, the temperature was recorded. 4. Sucessive 5.0 cm3 portions of HCL was added and the mixture was stirred, the temperature was recorded after each addition. 5. The adding and recording process was continued till the addition of 50 cm3 of acid. (II) Titration of CH3COOH with standard NaOH: 1. ...read more.

Middle

2NaCl + H2O As NaOH is limited reagent, ? no. of mole of H2O = (1)(50/1000) = 0.05 mol ?Honeu = 2926/0.05 ?Honeu = ? 58.52 kJ (Calculations) CH3COOH + NaOH ? CH3COOH-Na+ + H2O As NaOH is limited reagent, ? no. of mole of H2O = (1)(50/1000) = 0.05 mol ?Honeu = 627/0.05 ?Honeu = ? 12.54 kJ ?The standard enthaply change of neutralization of using HCl and CH3COOH are ?58.52kJ mol-1 and ?12.54kJ mol-1 respectively. Questions: 1. [H2O] is a constant when it acts as a solvent. The equilibrium will shifts to the left or shift to the right and [H2O] remanins unchanged. As the [acid] and [base] is very low though it is strong, [H2O] remanins unchanged. 2. (I) Some heat is lost to the surrounding. (II) We assume that the heat capacity of the cup is zero. ...read more.

Conclusion

(discussion) We should try hard to make sure whether the rise in temperature is logical, if the temperature have no willing to increase for a degree after a few times of the addition of the strong acid. We should once report it to the teacher to find if the given reagent has a different concentration from given. As sodium hydroxide is very corrosive, we must use the pipette filler supplied, and we must wear lab coat and safety spectacles in the laboratory. The last drop of the pipette should be dipped into the solution. We should fill the burette with a filter funnel and under eye sight for safety reasons. The filter funnel should be removed after filling. The burette should be placed upright to the vertical. Conclusion: The value from experimential result of neutralizatin using HCl and CH3COOH are ?58.52kJ mol-1 and ?12.54kJ mol-1 respectively. The one using HCl is more negative than ?57.6 kJ mol-1 , as the maximum temperture attained may be higher estimated. ?? ?? ?? ?? 1 ...read more.

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