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How does the concentration affect the rate of reaction between sodium thiosulphate and hydrochloric acid

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Introduction

How does the concentration affect the rate of reaction between sodium thiosulphate and hydrochloric acid? Introduction: We are trying to find out how the rate of reaction is affected by the concentration of one of the reactants. We are investigating this with sodium thiosulphate and hydrochloric acid. We will use different strengths of HCI acid and record the results. Method: * Collect the apparatus. * Make up different concentrations of hydrochloric acid using table 1. * Measure 20cm3 of sodium thiosulphate and pour into conical flask * Draw "X" on paper and place under conical flask. * Carefully pour hydrochloric acid into burette using funnel. * Remove funnel. * Turn the tap on the burette and start the stop-clock * Stop the clock when the "X" is no longer visible. * Record the results and repeat x5. ...read more.

Middle

is no longer visible * Using sensors to detect the loss of the starting material or the formation of the product Variables: Temperature: If the temperature is high, the particles have more energy. As a result of them having more energy they move a lot faster. Therefore the particles collide a lot faster increasing the rate of reaction and making a new product. Examples of reactions: An example of a reaction is when water and iron combine together to form iron oxide (H2O) (Fe 3) (Fe2 O3) Another example of a reaction is when zinc and oxygen combine together to form zinc oxide (Zn) (O2) (Zn O2) Concentration: If the concentration is greater so to is the number of particles. ...read more.

Conclusion

1 2 3 4 5 Average time (secs) Rate (sec -1) 0.2 28.94 29.42 30.04 29.54 28.57 29.30 0.034 0.4 22.69 24.47 24.41 23.56 26.59 24.34 0.041 0.6 18.94 19.54 19.42 20.22 20.84 19.79 0.051 0.8 15.72 15.10 15.84 15.91 16.04 15.72 0.064 1 15.28 15.54 15.68 15.17 15.49 15.43 0.065 Conclusion: From my results I can conclude that concentration does affect the rate dramatically. For example if we compare strongest strength of acid (1 molar) to the weakest (0.2 molar), there is a difference of nearly 14 seconds between the averages. This is because in the 0.2 molar acid there is only a small amount of h+ ions where as in the 1 molar acid there is a lot more. Therefore the collisions occur a lot faster and the rate of reaction is increased as illustrated in the diagram above. ?? ?? ?? ?? Science coursework Stephen bannon ...read more.

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