To investigate the reaction between Sodium Thiosulphate and Hydrochloric Acid.
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Reaction Rates Aim: To investigate the reaction between Sodium Thiosulphate and Hydrochloric Acid. Prediction: I think that as the amount of Sodium Thiosulphate is decreased and the volume of water increased, the reaction time between it and Hydrochloric acid will increase. This is because when the concentration of a substance is increased, it reacts a lot quicker due to there being more particles that want to react with each other. Reactions can only happen when the reactant particles collide, but most collisions are not successful in forming product molecules. Water has been introduced in this experiment to vary the concentration. If there is more water in the experiment, the less concentrated the Sodium Thiosulphate will be, therefore slowing the reaction.
I will take 2 sets of results to ensure that they are accurate. If 1 time taken seems out of place, the value will not be recorded and the experiment will be retaken and the value will not be recorded. In addition I will not stir the solution and it will take place at room temperature. Apparatus: * Measuring cylinder (50cm3) * Conical Flask (100cm3) * Sodium Thiosulphate * Water * Hydrochloric Acid * Stopwatch * Paper with "X" on it Method: 1. Collect equipment 2. Measure out 50cm3 of Sodium Thiosulphate and put into beaker 3. Measure out 10cm3 of Hydrochloric Acid and put into beaker 4. (After first experiment do the same with 5cm3 of water)
There were also a few anomalous results in my experiment. An inaccurate time recording probably caused these or it could've been that the wrong substance was put into the conical flask. Evaluation: Overall my experiment worked very well. The results I produced supported my prediction exactly. The experiment could've been improved by conducting more experiments at more regular intervals. This would make the results much more accurate. Also the temperature of the solution could've been varied to see if the temperature had any relevance to the reaction time. The only problems I encountered during this experiment were that some of the results I produced didn't agree with the others. As a result of this I excluded them when calculating the average and repeated that set of results. Oliver Carter Reaction Rates
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