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# Investigating the Effect of Concentration on the Rate of Reaction between Hydrochloric Acid and Sodium Thiosulphate

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Introduction

Planning Section Investigating the Effect of Concentration on the Rate of Reaction between Hydrochloric Acid and Sodium Thiosulphate I think that the higher the concentration of the Sodium Thiosulphate, the faster the reaction will take place. The more water there is in the solution, the slower the rate of reaction will be. This is because the greater the concentration, the more reactant particles there are in that certain solution. There will be more successful collisions and therefore the rate of reaction is increased. Apparatus To successfully carry out this experiment, I will need the following apparatus: * Hydrochloric acid * Sodium Thiosulphate * Distilled water * A beaker * 2 measuring cylinders (one 50cm� and the other 25cm�) * A piece of paper with an "X" on it * Safety goggles * 2 pipettes * Stopwatch * Calculator * Results table * Pencil Preliminary Experiment In order to see in what way to carry out the main experiment, I have carried out a preliminary experiment. I have only recorded two results. For the preliminary, I used 0.1M sodium Thiosulphate. Volume of Sodium Thiosulphate Volume of Distilled Water Volume of Hydrochloric Acid Time taken (seconds) 25cm� 0cm� 5cm� 41 5cm� 20cm� 5cm� 398 After doing the preliminary experiment, I decided to alter the main experiment for practicality reasons ...read more.

Middle

- I will be taking five measurements because it is a wide enough scale and will be practical to plot on a graph. - I measured the solutions accurately by using two different sized measuring cylinders - one small one to measure anything below 10cm�, and one big one to measure anything above 10cm�. This gave me much more accurate solutions. Variables The factors to control are: * Temperature: if the temperature is increased, the rate of reaction increases too. This is because the particles move faster as they have more energy. This means that they will collide more and are more likely to break the bonds, so the reaction is faster. I will control this by doing the experiment at room temperature, and I will do all of the solutions on the same day so the change of weather doesn't affect my experiment and make it less accurate. If I don't control the temperature, it could potentially alter my results (not significantly, but nonetheless it could still alter them) so I have to keep the temperature constant for the best results I can get. * Surface area: if the surface area is increased, more particles are exposed to the reactant, so they will collide more often, therefore increasing the rate of reaction. ...read more.

Conclusion

Volume of Sodium Thiosulphate Volume of distilled water Volume of hydrochloric acid Time Taken (seconds) Concentration of Sodium Thiosulphate* Rate of reaction** (in sec-1) 1 25 cm� 0 cm� 5 cm� 37 0.15M 0.027 2 20 cm� 5 cm� 5 cm� 48 0.12M 0.021 3 15 cm� 10 cm� 5 cm� 67 0.09M 0.014 4 10 cm� 15 cm� 5 cm� 122 0.06M 0.0082 5 5 cm� 20 cm� 5 cm� 366 0.03M 0.0027 * Concentration of sodium thiosulphate solution calculated in this way: Concentration of sodium thiosulphate = 0.15 x volume of sodium thiosulphate Vol. of sodium thiosulphate + vol. water ** Rate of reaction calculated in this way: Rate of reaction = 1 � time taken (seconds) (Note: this will not give me the actual rate of reaction itself, but 1 � time taken is a measure of the rate of reaction. Analysis Section The evidence shows that the more Sodium Thiosulphate used in the solution, the faster the reaction took place, and therefore the rate of reaction is smaller. For example solution number one: volume of sodium thiosulphate: 25 cm�, rate of reaction 0.027 (took 37 seconds). The less Sodium Thiosulphate used, the slower the reaction took place, and therefore the rate of reaction was higher - e.g. solution number 5: volume of sodium thiosulphate: 5 cm�, rate of reaction: 0.0027 (took 366 seconds). Examples: ?? ?? ?? ?? October 2006 ...read more.

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The first part of this write up is good and includes ideas on how the method could be improved and made fair. Unfortunately the latter part of the write up is not as good and lacks any valid, or detailed conclusion 3 stars.

Marked by teacher Louise Star 21/06/2013

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