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Introduction I am going to investigate the effect of varying the concentration of Sodium Thiosulphate solution in a reaction with Hydrochloric Acid. The theory behind this experiment is that 'Increasing the concentration can increase the rate of the reaction by increasing the rate of molecular collisions.' I chose this reaction because it has a definite end point (when the cross disappears on the paper). The equation for the reaction is: Sodium Thiosulphate + Hydrochloric Acid Sodium Chloride + Water + Sulphur + Sulphur dioxide Or Na S O (aq) + 2HCL (aq) È 2 Na Cl (aq) + H O (l) + S (s) + SO (g) Plan Equipment · 2 Measuring cylinders · Conical flask · Beaker · Stopwatch · Paper with cross-marked on it · Sodium Thiosulphate solution · Hydrochloric Acid · Water · Pipette Prediction I predict that the greater the concentration of Sodium Thiosulphate solution the faster the chemical reaction will take place. Therefore, the cross will fade away more quickly due to the cloudiness of the solution. I think that the concentration of a solution effects the rate of reaction because 'the rate of reaction depends on how frequently the molecules of the reacting substances collide.
Approximate Word count = 793
Approximate Pages = 3.2
(250 words per page double spaced)
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