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I will be studying the rate of reaction between sodium thiosulphate and dilute hydrochloric acid.

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Introduction

Daniel Hatton Investigating Rate of Reaction I will be studying the rate of reaction between sodium thiosulphate and dilute hydrochloric acid. I believe that if I increase the concentration of the sodium thiosulphate, the rate of reaction will increase, because the molecules are closer together, so there are more collisions per second. I believe if I double the concentration of the sodium thiosulphate then the rate of reaction will double, because there will be twice as many sodium thiosulphate molecules in the same area, and so there will be twice as many collisions. Using the method on the briefing sheet I carried out preliminary experiments using measuring cylinders. The times taken for the cross to disappear are shown bellow: Vol. of Thiosulphate/cm Vol. of H O/cm Time/Sec. 50 0 39 10 40 208 This seemed to be a reasonable range of reaction times so I will study this range of concentrations. Method: Apparatus: -Safety Goggles -Burette -Conical Flask -Measuring Cylinder -Thiosulphate -Dilute Hydrochloric Acid -Water -Stop Watch 1. Wear safety goggles at all times during the experiment. The chemicals being used are at low enough concentrations that they are only dangerous if they get in your eyes and so safety goggles prevent any risk. ...read more.

Middle

This gives the volume of thiosulphate required for the correct concentration. E.g., for 40%: 0.5 40=20cm . 9. Using the burette measure out the amount of thiosulphate needed for the appropriate concentration and put this in the measuring cylinder. Then using the scale on the side of the measuring cylinder add water until the solution is up to 50cm . Then repeat 1-6 with each concentration. Results: This is a table of my results: Thiosulphate -cm H O -cm Thiosulpate -% Acid -cm Time -sec. Average Time -sec. 1 Time 50 50 50 0 0 0 100 100 100 10 10 10 54.29 32.81 33.52 38.95 0.026 40 40 40 10 10 10 80 80 80 10 10 10 42.59 40.37 42.07 48.68 0.021 30 30 30 20 20 20 60 60 60 10 10 10 57.39 61.22 53.32 68.06 0.015 20 20 20 30 30 30 40 40 40 10 10 10 84.15 91.67 61.49 108.68 0.009 10 10 10 40 40 40 20 20 20 10 10 10 177.02 205.52 240.04 207.53 0.005 Analysis: From my results I can see the greater the concentration of thiosulphate the faster its rate of reaction. ...read more.

Conclusion

The experiment could have been improved by giving more attention to the temperature during the experiment. This is a variable that affects rate of reaction, but it was assumed as the experiment was carried out inside, it would be kept constant and so wouldn't be a factor. Drawing the cross, for the experiment, on a piece of paper meant it was easily smudged if anything was spilt on it and it would have been better to use a white tile and a marker pen. I did not always look down the conical flask at the same angle for each experiment and so this could have affected the time recorded. Using a calorimeter could have solved this problem as it passes a beam of light through the solution and so would accurately tell me when the solution had become clouded and be consistent for each repetition. The evidence does seem strong enough to support the conclusion made in my analysis as the graph had no anomalous results and had very strong correlation. The investigation could be extended further by studying a different variable, say temperature, by repeating the experiment in a water bath heated to different temperatures or by studying concentration again, but using a different acid other than hydrochloric. ...read more.

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