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# Measuring the rate of reaction, when dilute sodium thiosulphate solution and dilute hydrochloric acid are mixed

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Introduction

Measuring the rate of reaction, when dilute sodium thiosulphate solution and dilute hydrochloric acid are mixed. Hypothesis: I predict that the higher the concentration of sodium thiosulphate, the faster the rate of reaction. Aim: In this experiment I intend to test the collision theory. My aim is to see if the concentration of sodium thiosulphate will affect the rate of reaction. Introduction: In this experiment I will vary the concentration of sodium thiosulphate to measure the rates of reaction. I will be mixing different concentrations of sodium thiosulphate with hydrochloric acid, the collision theory says the reaction time will alter; this is what I will be testing. The collision theory tells us that the larger the surface area, the faster the reaction. So the higher the concentration the more atoms there are to react. There are 4 things that affect the rate of reaction, concentration, surface area, catalysts and temperature. Concentration can affect the rate of reaction by increasing atoms to collide with each other. The more atoms there are to collide, the faster the rate of reaction. In reactions where gases are involved, if you increase the pressure the particles will move closer together. ...read more.

Middle

Preliminary Method: * Fill up 5cm� of HCL in a measuring cylinder and 25cm� of sodium thiosulphate in another measuring cylinder. * Empty the sodium thiosulphate in the conical flask and then place the conical flask over the piece of paper with the "X" marked on it. The next few steps we had to do fairly quickly. * Add the hydrochloric acid to the conical flask, as soon as the two solutions come in contact with each other, start the stop watch. * Gently swirl the conical flask so the two solutions can react, while doing this be careful not to breathe in the products produced by this reaction. * When the contents of the conical flask starts to go cloudy, look into the conical flask from above and wait for the "X" to disappear. * When the "X" has disappeared stop the stop watch and record the time on the results table. Repeat this procedure 3 times with the same measurements and then repeat the same experiment using the measurement provided in the results table. The method must be repeated 3 times for each set of measurements, in order to work out the average time when the results need to be recorded onto a graph. ...read more.

Conclusion

Also the anomalies could have occurred because there was too much or too little of a chemical. Again I tried my best to keep the measurements accurate. Some of the bottles that contained the chemicals could have been contaminated, but there was no way of telling if they were or not, so I carried on with my experiment assuming they were not. I noticed the anomalies where the graph was drawn up. I could avoid these anomalies by decontaminating all the equipment I used, make sure the chemicals I use are fresh and also make my measuring of the chemicals used, more accurately. Evaluation: I think the experiment was fair, apart from a few anomalies. I could avoid these anomalies by decontaminating all the equipment I use, make sure the chemicals I use are fresh and also make my measuring of the chemicals used more accurate. I could extend the experiment by testing temperature instead of concentration and then compare the results. My repeats are seconds out apart from the last row on the table. I think that the results are as accurate I will be able to get them. The measuring equipment I used could be at fault, I don't the equipment was that accurate. But in a school laboratory it is difficult to get the results you expected. By Veenesh Halai ...read more.

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