• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

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

Extracts from this document...


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.


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.


(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.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Aqueous Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Aqueous Chemistry essays

  1. Determine the enthalpy of neutralization for HCl +NaOH, CH3COOH +NaOH, and 1/2H2SO4 +NaOH.

    3. 25 cm3 of a aqueous NaOH (1.04M) was added to the dilute HCl and the apparatus stirred after the lid was closed 4. Since the reaction is quick the thermometer was kept immersed into reaction mixture as soon as the NaOH (aq)

  2. Back Titration to find the Concentration of Vinegar (Ethanoic Acid)

    + H2SO4(aq) � Na2SO4(aq) + 2H2O(l) Indicator: Bromothymol Blue Colour change: blue to yellow (green at equivalence point) Table 1: Amount of sulphuric acid that was needed to neutralise 1cm3 of sodium hydroxide Run Flush 1 2 3 Volume of NaOH used (cm3)

  1. Analysing the ethanoic acid concentration in different types of vinegars.

    Results: Titration: Malt Vinegar: Titration no. 1 2 3 Start position 23.4 31.5 40.3 End position 31.5 40.3 48.7 NaOH used 8.1 8.8 8.4 Average NaOH used = ( 8.1+8.8+8.4)/3 = 8.43 (3sf) I can now convert use this to calculate the number of moles of NaOH used, using this formula: Number of moles = (Concentration

  2. To investigate the effect of concentration on the temperature rise, heat evolved and heat ...

    It is because the heat of neutralization is nothing but the amount of heat evolved per mole. The concentration change will change the mole and as well as the heat evolved. Concentration is directly proportional to the heat evolved and it is also directly proportional to the mole, thus any

  1. How much Iron (II) in 100 grams of Spinach Oleracea?

    I completed this experiment twice using two different spinach extract solutions, which were produced using the same method. This was done so that I could compare the two results and find an average. Average mg in 100 grams of Spinach Oleracea =1.0020075 + 1.69330044 2 = 1.34765397 mg These results

  2. Determine the concentration or molarity of Ethanoic acid (CH3COOH) in two types of commercial ...

    0.7235 = the no. mole in 1 dm3 (1000 cm3). It is more convenient to use 100 cm3 so 0.7235 will have to be divided by 10: 0.7235 / 10 = 0.07235 The percent by mass data can now be found out: Mass = No.

  1. Determination of the equilibrium constant for esterification of ethanoic acid and propan-1-ol by using ...

    The two reactants were then mixed thoroughly. The first titration: 1. The burette was rinsed, and then it was filled up with sodium hydroxide solution. 2. On the other hand, a 100 cm3 conical flask containing about 25 cm3 deionized water and two drops of phenolphthalein indicator solution was prepared.

  2. Obtain pure samples of Ethanol (CH3CH2OH) and Ethanoic Acid (CH3COOH) from fermented Yeast (Saccharomyces ...

    Energy PRACTICAL 2 Distillation of the ethanol solution In this practical the ethanol solution will be distilled using the distillation apparatus (see method - practical 2- FIGURE 2). Distillation is used to separate a liquid from either a dissolved non-volatile solid or another liquid.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work