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The Effect of Concentration on the Rate of Reaction of Sodium Thiosulphate with Hydrochloric Acid.

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Introduction

The Effect of Concentration on the Rate of Reaction of Sodium Thiosulphate with Hydrochloric Acid AIM: I intend to conduct an experiment on the effect the concentration of the hydrochloric acid has on the rate of reaction between it and Sodium Thiosulphate. It will be conducted in a controlled environment, I will be following the method that has been supplied to me by my teacher with my own additions to try and ensure the best possible results. I will be altering the variable of concentration of sodium thiosulphate solution, the other variables are changing temperature, or changing the surface area of a solid reactant, or adding a catalyst. Factors to consider: To ensure that my investigation provides the best results possible, I must consider, the efficiency of myself and partner. We must be focused and attentive. I think to prevent any cause for problem in the investigation, I will try and lessen the chance of boredom by writing a method that is quick and more than satisfactory so as to obtain the best results possible. Fair Test: I plan to do a safe and fair investigation into the effect of concentration on the rate of reaction of sodium thiosulphate with hydrochloric acid. I will use safety goggles and gloves to protect my skin from the acid and to protect my eyes from any splatter. ...read more.

Middle

Place equipment as required on the work surface, with the conical flask over the crossed white sheet, and the hydrochloric acid placed at one end of the work area with a plastic measuring cylinder and glass beaker and at the other end with a plastic cylinder and glass beaker the Sodium Thiosulphate Solution. (the beakers and cylinders are not to be mixed) 3. Set the Stop Clock 4. Measure out 15cm3 of 2M thiosulphate solution and pour into conical flask 5. Measure out 15cm3 of dilute hydrochloric acid as it is poured into conical flask start timer. 6. Stop the clock once the cross on the paper is no longer visible. 7. Wash out conical flask dry and redo experiment twice more with the same Molar. 8. Redo experiment again with 1 Molar testing it at least twice, then again at least twice for 0.5 Molar and finally at least twice for 0.25 Molar. Predictions: I predict that the higher the molar concentration of the solution the quicker the reaction will take place due to concentration being a factor that can change the rate of reaction. Other factors that affect the rate of reaction apart from the concentration are the surface area, the use of a catalyst, the temperature and the pressure. ...read more.

Conclusion

Reactions can only happen when the reactant particles collide, but most collisions are not successful in forming product molecules. The reactant molecules must collide with enough energy to break the original bonds so those new bonds in the product molecules can be formed. All the rate-controlling factors are to do with the frequency of reactant particle collision. What will happen in this experiment is I will add hydrochloric acid to an equal amount of sodium thiosulphate. During the experiment the sodium in the sodium thiosulphate solution will displace the hydrogen, to form sodium chloride solution. Once the solution has become opaque I will know the reaction is complete this is due to a precipitate caused by sulphur which turns the solution cloudy whilst expelling sulphur dioxide. The same number of atoms will be kept throughout the experiment they will just be distributed differently compared to the start of the experiment. The rule for calculating the rate of reaction is; Rate of reaction = change in amount of substance time taken for the change to occur Below are a word and chemical equation of the experiment; Na2S2O3(aq) + 2HCl(aq) 2NaCl(aq) + SO2(g) + H2O(l) + S(s) I know that any increase in concentration during an experiment the rate of reaction will increase due to the likelihood of more collisions between molecules due to their being more of them in the same volume of the solution. GCSE Chemistry Coursework 1 Planning Samirah Toure ...read more.

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