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

Investigation to find out how the rate of reaction between sodium thiosulphate and hydrochloric acid.

Extracts from this document...

Introduction

Investigation to find out how the rate of reaction between sodium thiosulphate and hydrochloric acid Aim Investigation to find out how the rate of reaction between sodium thiosulphate and hydrochloric acid is affected by changing the concentration of hydrochloric acid Introduction In this experiment I am going to find out how the rate of reaction between sodium thiosulphate and hydrochloric acid is affected by changing the concentration. The equation to this is as follows: Sodium +Hydrochloric Acid Sodium +Sulphur +Sulphur +water Thiosulphate Acid Chloride Dioxide Na2 S2 O3 (aq) +2HCL (aq) NaCl (aq)+ S(s) +SO2(g) + H2O(l) This reaction usually produces a yellow precipitate. We place the reaction flask on a card with a black cross-drawn on it. When the cross is completely obscured, the reaction will have finished. The time taken for this to happen is the measure of the rate of reaction. We must do this several times, and change the concentration of sodium thiosulphate. The rate of reaction is a measure of the change, which happens during a reaction in a single unit of time. The things that affect the rate of reaction are as follows: 1. Surface area of the reactants-does not apply for this experiment 2. Concentration of the reactants 3. The temperature at which the reaction is carried out- If not kept the same particles will get more energy for being of a higher temperature and therefore causing more collisions. ...read more.

Middle

We then recorded the time for the cross to become completely obscured. We repeated this many times, adding different amounts of sodium thiosulphate and water each time, and recording the time taken each time. Diagram Fair test To make this experiment a fair test, we need to make sure we do a number of things. In this experiment we are trying to find the rate of reaction using concentration as a factor, so there is a number of things we need to make sure we do to keep it a fair test. Firstly, we need to keep a chemical at a constant concentration. So, in this experiment we have chose to keep hydrochloric acid at a constant concentration. We could have, however, used sodium thiosulphate as a constant, but we had chose to use hydrochloric acid. Next we must make sure that the solution is kept at a constant volume throughout the experiment. If the volume is different, then it could give different results to if it was at a constant volume. We must also make sure that we add both the water and the sodium thiosulphate at exactly the same time (into the conical flask with the hydrochloric acid in it), or it could effect the results of the experiment. We must start the stop watch at the exact time as we put the water and the sodium thiosulphate into the conical flask. ...read more.

Conclusion

However, there are still a few anomalous results which I will now point out. Hydrochloric Acid Sodium Thiosulphate Water Time Taken (s) 50 10 0 49 45 10 5 45 40 10 10 51 35 10 15 69 This is the only anomalous result that I have recorded. The result may have turned out anomalous because of basic human error, or maybe because we measured the substances wrong. It may have even been because we did not clean the apparatus properly. Apart from this, the accuracy of my experiment has been more or less accurate. Although there are a number of ways in which we could have made the results more reliable. For instance, we could have used better measuring equipment, because the apparatus we used was mainly basic equipment. Another thing we could have done to bring more evidence is to have tried to use the hydrochloric acid as the variable substance, and used the sodium thiosulphate as the constant substance. This would have brought more evidence to support the idea that the higher concentration of a substance, the faster it will react. I think that the evidence, which I have received, is enough to reach a suitable conclusion, but there are a few flaws to the experiment (which I have mentioned). Apart from them, the experiment is fine. ...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. Aspirin Investigation

    TEST FOR PURITY: Titration Apparatus 250ml conical flasks Beakers Burette Busen burner Distilled water Filter funnel Phenol red indicator Pipette Pi-pump Sodium Hydroxide 1M Standardised Sulphuric acid Tripod, heatproof mat and gauze Wash bottles A known mass of the aspirin was weighed and placed in a conical flask.

  2. Antacid Investigation.

    We shall only be doing this once because it is a preliminary experiment. Results. Burette Start Burette Finish (ml) Difference (ml) Tablet brand Indicator used 0ml 8.5 8.5 Settlers Bromophenol blue 0ml 7.5 7.5 Superdrug Bromophenol blue 11.5 ml 23 11.5 Rennie (pepper mint flavour)

  1. An Investigation Into The Rate Of Reaction Between Sodium Thiosulphate and Hydrochloric Acid.

    And other than that, the only other thing to be done in order to ensure safety is that General Laboratory Practice (GLP) should be used. Variables that should be kept constant to ensure a fair test and accurate results: Volume of Sodium Thiosulphate Temperature Voltage used in circuit Wattage of

  2. To investigate the rate of reaction between different concentrations of hydrochloric acid with metal ...

    Here are the lessons that I have learned from the preliminary experiments for Technique 2: Problems 1. The readings will not be very accurate as you will be looking at the experiment for a qualitative result and therefore there is a margin of error because you will have to make a judgement on whether the reaction has stopped or not.

  1. Reactivity Series Investigation

    without heat by fizzing the most with the acid and creating the most vapour.Calcium was the metal that dissolved completly not like the other metals and also had the highest temperature after the experiement about 45 degrees celsius which is a 6 degrees higher than magnesium and 15 degrees higher

  2. What factors affect the rate pf reaction between sodium thiosulphate and hydrochloric acid?

    I will then put a piece of paper with an "X" marked on it underneath my conical flask. I will use the same marker for all my experiments, the marker will be printed off on the computer because it is more accurate this way as the printing is even

  1. Rates of Reaction

    We must then add the medium sized marble chips measured at 2g to 15ml of hydrochloric acid and then quickly fasten the bong to the flask trying not to let any gas escape. We would then record the amount of gas given off every 10 seconds in a period of 2 minutes.

  2. Rate of Reaction

    - 90 24 - - 100 27 - - Medium pieces of marble chippings, 2 mol HCl 0 0 0 0 10 4 18 25 20 8 28 54 30 12 36 91 40 17 47 - 50 21 68 - 60 26 85 - 70 30 - - 80

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