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

See how the pH and the temperature levels change during an acid/base titration using the indicator and thermometer method.

Extracts from this document...

Introduction

GCSE Chemistry Coursework on a Titration Aim To see how the pH and the temperature levels change during an acid/base titration using the indicator and thermometer method. Results Tables Analysis of Results From my graphs that I have drawn on the previous four pages, I can conclude that adding any amount of acid to a solution of alkali will result in a change of pH value, colour and temperature. This is very clear, despite the fact that I managed to achieve some anomalous results during my experiment. This error only occurred during the 2 Molar solution experiment where the temperature and colour was recorded and not in the 0.5 Molar solution where the pH value and colour was recorded. For the 0.5 Molar solution, as the amount of acid added to the alkali increases the pH value of the solution decreases at quite a steady rate until it reaches pH 7 (neutralisation) and then the pH value decreases very quickly. Between 24cm3 and 27cm3 of acid added to the alkali the pH value dropped from pH 8 and pH 9 respectively to pH 1. ...read more.

Middle

The graph of the acid added against amount of temperature shows a positive correlation up to 27cm3 of acid added and then also shows the signs of a negative correlation between 28cm3 and 30cm3 of acid added. I have found that for the thermometer method, the temperature was inversely proportional to the amount of acid that was added to the alkali. Also, before the neutral point, the temperature started to increase quickly and then slowed down as it got closer to the neutral point. This may have happened because at the start of the experiment there was less liquid in the beaker for the reaction to heat. As acid was added, this meant that there was more liquid for the reaction to heat, and so the rate of temperature increase would have started to slow down as you got closer to the neutral point, where the temperature started decreasing. Another reason for the slow increase in temperature was that the acid was cooler than the alkali when it was added. ...read more.

Conclusion

be poured into it * An alternative piece of equipment than a burette should be used to make sure that the correct amount of acid is poured into the beaker containing alkali. I suggest using a 2ml syringe to slowly pour the acid in as the results will be more accurate * You could also keep adding more and more acid to the alkali and see how the temperature of the solution is affected and draw a graph to show your findings * The main problem that was affecting the results of the thermometer method was that the room temperature was changing and never remained at a constant temperature. There was no way of controlling the temperature in this experiment unless it was done in a laboratory under controlled conditions If I had had enough time, I would have repeated my experiment for each molar solution two times and take an average of the results so that I can get a more accurate result. I would have also taken more readings closer to the point of neutralisation to make sure that I got a more accurate result. Khushpal Grewal 11K ...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. Marked by a teacher

    Enthalpy of Neutralisation.

    3 star(s)

    and the heat conducted to the calorimeter containing the reactants. A thermometer can be used to follow the heat flow during the reaction. If the temperature is observed to rise, this means that the heat is flowing from the system into the thermometer (and other surroundings).

  2. Find out the percentage of citric acid present in lemon squash by using a ...

    Similar thermometer (0oC- 110oC). This has to be the same because each thermometer could give slightly varying results. 2. Amount of water in each beaker (in the 500ml beaker I will use 500ml, in the 200ml beaker I will use 200ml,and in the 30ml beaker I will use 30ml).

  1. Mix an acid and an alkali and measure the temperature change.

    + H2O (1) - 57.8 HNO3 (aq) + NaOH (aq) --> NaNo3 (aq) + H2O (1) - 57.6 HNO3 (aq) + KOH (aq) --> KNO3 (aq) + H2O (1) - 57.7 HBr (aq) + NaOH (aq) --> NaBr (aq) + H2O (1) - 57.6 If all acid solutions are ionized and contain hydrogen ions, H+ (aq), and

  2. Investigating the effects of varying pH levels on the germination of cress seeds

    they will all weigh the same. * I will add 20cm� of each solution to the corresponding sample petri dish. * I will count and add 40 cress seeds to each sample petri dish. * I will add a further 10cm� of each solution to the corresponding sample petri dish.

  1. Establish what types of soil holds the most water and to see if changing ...

    The experiment proved this wrong as observations noted showed that the water filtered through the sandy soil quicker than expected resulting in only 15.4ml of water being absorbed in total. This may have been to the fact that only a small quantity of the sand was used or that it

  2. Calibrating pH meters

    Method When the experiment was carried out the first thing that needed to be attended to was having all the correct equipment and materials at hand. The following equipment and material were gathered: * Beaker- A beaker made out of glass with measurement markings on the side.

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

    The system was left for one hour for reflux. During the reflux, the degree of heating was adjusted to make sure that the vapours did not rise above the lower half of the condenser. The third titration: 1. After 1 hour, the flask and its contents were cooled in an ice bath.

  2. Energy Change Associated With Neutralisation

    - therefore they have not required as much energy to form as they already had stored in them. = NaCl (sodium chloride) = H2O (water (hydrogen x 2 + oxygen)) This means there is some excess energy that is diffused into the surroundings as heat.

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