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Investigate the rate of the reaction between aqueous sodium thiosulphate and dilute hydrochloric acid.

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My aim in this coursework is to investigate the ratee of the reaction between aqueous sodium thiosulphate and dilute hydrochloric acid. The ionic equation for the reaction betweem aqeous sodium thiosulphate and dilute hydrochloric acid is : 2h+ (aq) + S2O3 2- So 2 (aq) + H20 (l) + S (s) When a solution of sodium thiosulphate reacts with any acid a precipitate of sulphur forms. The reaction occurs between the hydrogen ions from the acid and the thiosulphate ions in the sodium thiosulphate. Backround information There are many variables, which affect the rate of the reaction between aqueous sodium thiosulphate and hydrochloric acid. These are ; The temperature at which the reaction is taken place at A Catalysy The concentration of the sodium thiosulpate The concentration of the hydrochloric acid The collision theory states that the rate of a rection simply depends on how often and how hard the reacting particles collide with each other. The basic idea is that particles have to collide with each other to react, and they have to collide hard enough as well. When the temperature is increased the particles all move quicker. If they're moving quicker, they're going to have more of a chance of colliding with each other. ...read more.


I also believe that as I double the concentration the rate would also double. Method Firstly I will draw a cross on a white tile using a marker pen. The using the burette I will measure out of 20 cm3 of hydrochloric acid and pour it in a conical flask. Then I will measure out the concentration of the sodium thiosulphate solution. Then I will pour the solution into the conical flask and as soon as the first drop of sodium thiosulphate drops on the conical flask I shall start the stopwatch. Looking directly above the conical flask I will wait until the cross disappears and then stop the stopwatch. Apparatus Conical flask Hydrochloric acid Sodium Thiosulphate Dilute water 3 Burettes white tile Per,manent marker Stopwatch 2 Beakers Diagram Results concentration of time taken for repeat 1 repeat 2 solution mol/dm3 cross to disappear seconds seconds 1 6.51 6.23 6.43 0.8 8.44 8.97 8.36 0.6 9.76 10.38 9.41 0.5 12.09 12.61 11.98 0.4 14.95 15.54 15.29 0.2 32.23 32.26 33.64 0.1 65.12 62.47 61.32 concentration of average of results solution mol/dm3 in seconds 1 6.39 0.8 8.59 0.6 9.85 0.5 12.23 0.4 15.23 0.2 33.01 0.1 62.97 concentration of Rate of reaction solution mol/dm3 1/time taken (s-1) ...read more.


This ould have made my experiment very reliable and would have made my graph more acurate. It would have made my graph more accurate as there would be more points plotted on it. Another way in which I could have had anomalous results was by stopping the stopwatch early or too late. I could have also meausref the wrong concentration, this would have either increased or decreased the rate of my reaction. I believe a more accurate way in which I could have carried out this experiment was by using the light sensor, which is attackes to the data-logging computer. The way in which it works is that the computer measures the percentage of light, which is picked up by the sensor. The reaction stops when the reading on the computer goes down to 0%. This is a more reliable way in which to carry out the experiment as there is no chance of a human error to be made andd practically no chance of there being a computer error. For my furhter work I could have also done this experiment at a higher temperature. This would have probably increased the rate of the reaction. This is because when the temperature is increased the particles all move quicker. If they're moving quicker, they're going to have more of a chance of a collisions to occur with eachother. ...read more.

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