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Investigation to find out whether the concentration of sodium thiosulphate affects rate of reaction between itself and hydrochloric acid.

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Introduction

Investigation to find out whether the concentration of sodium thiosulphate affects rate of reaction between itself and hydrochloric acid Aim Plan To see how changing the concentration of sodium thiosulphate affects the rate of reaction between sodium thiosulphate and hydrochloric acid. Method For my first experiment I will mix 20cm^3 of sodium thiosulphate with 10cm^3 of dilute hydrochloric acid then time until the mixture turns opaque or becomes a 'precipitate' and I can't see the picture underneath. I will repeat the experiment changing only the concentration of sodium thiosulphate but keep everything else the same. To make the experiment fair I will make sure I only change the concentration of sodium thiosulphate and not anything else. I will keep the hydrochloric acid, the picture and the beaker the same. I will do a second experiment where instead of changing the sodium thiosulphate I will change the concentration of hydrochloric acid. ...read more.

Middle

I can also see that the rate is proportional to Molarity. My Molarity/time graph goes down in a gradually increasing curve. This is slightly strange because it should be a steady curve and the difference between times increases too much towards the end. This tells me that my results could be slightly inaccurate. These results tell me that as the sodium thiosulphate concentration decreases the time increases. This is because as the sodium thiosulphate is diluted, there are fewer particles to collide with hydrochloric acid particles. Fewer collisions mean a slower reaction because the particles are taking longer to collide with each other. This is because there are also water particles in the way. Therefore as the sodium thiosulphate is diluted more water is added (the number of water particles increase) causing the reaction to be slower and take longer. My results do agree with my prediction because I said that the rate of reaction will decrease and the time will increase. ...read more.

Conclusion

Also, I timed it using the wall clock and this isn't as accurate as using a stop clock. Also, some of the chemicals each time may have been left in the measuring cylinder. All my results do agree, and none of them look wrong. They all follow a sort of pattern so I think they are all sensible results. My results are quite reliable and accurate because all the faults in my method occurred with each experiment so they all were fair to each other. However, the problems above might mean that my results aren't as reliable and accurate as they could be. I think my results that aren't exactly fitting into the pattern may have occurred because of the slight inaccuracy in my equipment. I think my results are good enough though to make a valid conclusion because you can see a difference and patterns in my results as the molarity increases. Also, I kept everything except the sodium thiosulphate the same each time so it was as fair as I could make it. ...read more.

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