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

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Introduction

An Investigation Into The Rate Of Reaction Between Sodium Thiosulphate and Hydrochloric Acid The purpose of this investigation / experiment is to observe the rate of reaction between sodium thiosulphate and hydrochloric acid. When these react the colour of the solution changes eventually to an opaque creamy solution. The reaction that will take place is: Na2S2O3 + 2HCl ? 2NaCl (aq) + SO2 (aq) + S (s) + H20 Sodium Hydrochloric Sodium Sulphur Sulphur Water Thiosulphate Acid Chloride Dioxide The reason the solution becomes opaque is that one of the products of the reaction is sulphur and this solid forms in the solution and therefore makes it go cloudy, and opaque. So, to compare reaction times I shall use a light sensor under the solution so that I know when each solution has reached the same stage, as the same amount of light will be let through the solution. The variable that I am to change in this investigation is the amount of hydrochloric acid put into the solution. Equipment List Clamp stand Clamp Bulb Light Sensor Beaker Power Pack Wires Measuring cylinders Sodium thiosulphate Hydrochloric acid Water The equipment should be set up in the following way: Before starting this experiment, how to take the measurements needs to be planned properly. ...read more.

Middle

At low temperatures, particles of reacting solutions, or elements, don't have much energy. But, when these are heated, the particles gain energy. This means they move faster and collide more often. Thus the rate of reaction will speed up. If the collisions have more energy then more of them will be successful. Results Volume of Acid (ml) Time taken to reach 400 lux (seconds) Average Time (seconds) 1st time 2nd time 3rd time 5 67 76 119 87.33 10 50 62 69 60.33 15 49 58 68 58.33 20 46 57 67 56.67 25 41 51 59 50.33 30 40 47 57 48.00 Analysis Volume of Acid (ml) Time taken to reach 400 lux (seconds) 1st time 2nd time 3rd time 5 67 76 119 10 50 62 69 15 49 58 68 20 46 57 67 25 41 51 59 30 40 47 57 It can be clearly seen from my table of results, that not all the results agree. For example, when the solution with 5ml of Acid was done for the third time, it took 119 seconds, this is a huge difference to the first two times. It can also be seen that the times taken in the first attempts column (1st time) ...read more.

Conclusion

are exactly the same concentration. * Wrap the sides of the beaker with opaque paper to ensure that the only light being let into the beaker is that from the bulb. * Use the same light censor on each day. I believe that the evidence shown by my results can support a conclusion that, the rate of reaction between sodium thiosulphate and hydrochloric acid is quicker, the more acid that is used in the reaction and is slower, the less acid that is used in the reaction But, as in this experiment there is a great room for error, my results will not be entirely accurate and therefore cannot support a firm conclusion. Overall I believe I carried out this experiment to the best of my abilities, considering all the different factors that could have affected my results. To extend the investigation I could investigate how temperature would affect the reaction rate between Hydrochloric acid and Sodium thiosulphate. Measuring the reaction times whilst the solutions are at different temperatures could do this. I would predict for this that the warmer the temperature, the quicker the reaction, as in corroboration with my prediction for this experiment, reaction rates are based around collisions and as the reaction is given heat, the particles are given energy and thus there are more successful collisions, therefore speeding up the reaction rate. ...read more.

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