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

THERMOMETRIC TITRATION

Extracts from this document...

Introduction

CHEMISTRY COURSEWORK THERMOMETRIC TITRATION Aim The purpose of this experiment is to determine the concentrations of two acids, hydrochloric acid, HCl, and ethanoic acid, CH3CO2H, by thermometric titration; and having done that, to calculate the enthalpy change of neutralisation. Introduction You titrate both hydrochloric acid and ethanoic acid in turn with a standardized solution of sodium hydroxide and record the temperatures of the mixtures during the course of the titration. In each case a plot of temperature against time will enable you to determine the maximum temperature rise, from which you calculate both the concentration of the acid and the enthalpy change of neutralisation. Requirements * Safety spectacles * Pipette, 50.0 cm3 * Pipette filler * Expand polystyrene cup * Sodium hydroxide solution , 1 m NaOH (standardized) * Thermometer, 0-50 C0 (in 0.1 C0) * Burette , 50.0 C0 cm3 * Filter funnel , small * Hydrochloric acid , M HCl * Ethanoic acid, M CH3CO2H Safety/risk assessment: During experiment in laboratory extreme care should be taken to avoid any hazards. ...read more.

Middle

4. Stirred the mixture with the thermometer and recorded its temperature. 5. Added successive 5.0 cm3 portions of HCl solution stirring the mixture and recording its temperature after each addition. 6. Recorded my results in a copy of result table 14a. Stopped after addition of 50.0 cm3 of acid. Titration of ethanoic acid with standard sodium hydroxide solution 7. Followed the same procedure as I did for the titration of HCl, except that I used ethanoic acid in the burette. When filling the burette, I had to remember to use to correct rinsing procedures. 8. Recorded my results in a copy of results table 14b Results Table 14a, Titrations of hydrochloric acid. Volume added/cm3 0.0 5.0 10.0 15.0 20.0 25.0 30.0 35.0 40.0 45.0 50.0 Temperature/C0 24 27 29 31 32.5 33 32.5 31 30.5 30 29.5 Volume added/cm3 0.0 5.0 10.0 15.0 20.0 25.0 30.0 35.0 40.0 45.0 50.0 Temperature/C0 24 27 29 30.5 32 32 31 30.5 30 30 29.5 Results Table 14b Titrations of ethanoic acid. ...read more.

Conclusion

A s long we are considering a strong acid reacting with a strong base , we always dealing with the same reaction; H+ (aq) + OH- (aq) H2O (l) This is because strong acids and bases are assumed to be completely ionised, that is why the value is always constant. 2. Hydrochloric acid is less negative than -57 kj mol-1 because: * Energy was lost to the surrounding because the polystyrene cup was not good insulator. * Secondly, heat escaped through the hole of the polystyrene cup where the thermometer was inserted to take the temperature reading. 3. Weak acids and bases does not fully ionise when they dissolve in water. Ethanoic acid is typical example of a weak acid. It reacts with water to produce hydroxonium and ethonate ions, but the back ward reaction is more successful than the forward one. When ethanoic acid react with water only view percentage of the cid is converted into ions. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Inorganic 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 AS and A Level Inorganic Chemistry essays

  1. Peer reviewed

    Determining the concentration of acid in a given solution

    5 star(s)

    the end point can be reached more accurately with a slow flow of solution * Ensure the burette is vertical and read the reading again to the nearest 0.05cm3 * Record the value on the paper as the final burette reading * Work out how much sodium carbonate solution was

  2. Peer reviewed

    Deducing the quantity of acid in a solution

    5 star(s)

    The most important part is to be very careful because it can cut and cause harmful wounds. First of all, if any glass equipment fall, we need to tell the teacher and ensure everybody is aware of the danger. Then, we need to sweep it thoroughly to ensure no shards remain and put it into the glass bin.

  1. effects Concentration and Temperature on the Rate of Reaction

    x 100] 1000 This would give you the amount of grams of X2Y3 required, with the rest of the solution being made up with distilled water. Pre-test Firstly I have decided to use burettes rather than measuring cylinders for measuring out my solutions.

  2. Lab report Determination of Enthalpy Change of Neutralization

    of acid used / cm3 25 25 25 25 25 25 Volume of base used / cm3 25 25 25 25 25 25 Highest Temperature / 36.8 36.8 34.7 36.8 54.2 37.5 Lowerest Temperature / 24.8 24.0 24.5 23.8 24.2 24.0 Temperature Difference / 12.0 12.8 10.2 13.0 30.0 13.5

  1. Titration Coursework

    Then I will measure 25ml of my standard solution by holding the pipette at eye level and filling it using pipette filler. I will overfill it to some extent and use my thumb to lower it down slowly until the bottom of the meniscus touches the 25ml line. 10.

  2. The periodic table

    Chemists used this because it is in general easier practically to measure the weight of an element that combines with oxygen than the weight that combines with hydrogen. Atomic weights were then found from the equivalent weight using the relationship: Equivalent weight x valency = atomic weight where valency is

  1. Finding Out how much Acid there is in a Solution

    The anomalous titrations were the first and fourth titrations following the rough titration: Titration 1 4 Final burette reading (cm3) 1.55 0.70 Initial burette reading (cm3) 28.10 26.50 Titre (cm3) 26.65 25.80 There are several possible causes for these anomalies.

  2. The Effects of Strong and Weak Acids on the Order of a Reaction.

    This is directly proportional to the surface area of the reactants. The greater the surface area, the higher the chance of correct collisions taking place. The smaller the surface area, the smaller the chance of correct collisions taking place. This is due to the number of particles exposed to the

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