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The aim of this investigation is to find out the effect of concentration of acid, in the reaction between dilute hydrochloric acid and magnesium strip.

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Introduction

Chemistry Coursework Hydrochloric Acid and Magnesium Planning Aim The aim of this investigation is to find out the effect of concentration of acid, in the reaction between dilute hydrochloric acid and magnesium strip. Introduction The rate of a chemical reaction is a measure of how fast the reaction takes place. The way that you measure this is by timing how long it takes for the product to appear or the reactants to disappear. It is important to remember that a rapid reaction is completed in a short period of time; therefore we must pay close attention during observation in order to complete the experiment correctly. In this investigation we will test different concentrations of acid reacting with magnesium to see how long it takes the magnesium strip to dissolve in different strengths of diluted hydrochloric acid. Key Variables The key variables in this experiment are; Variables How the variables will affect the experiment. Concentration In order to fulfil this experiment correctly I will vary the concentration of hydrochloric acid. This is because the whole point of this experiment to see how long it takes the magnesium strip to dissolve in different concentrations of hydrochloric acid. ...read more.

Middle

An equation for the reaction: Magnesium + hydrochloric acid >magnesium chloride + hydrogen Mg (s) + 2HCL (aq)>Mgcl2 (aq) + H2 (g) Throughout the experiment, I diluted the acid solution using water, as I did this the concentration of the acid decreased. I measured out 10ml of acid and then poured the solution into the beaker with the magnesium strip init and then measured the time taken for the magnesium strip to dissolve, using the stop clock. Next, I diluted the acid by placing 8ml of acid and 2ml of water into the test tube and then poured it into the beaker with the magnesium strip init and measured the time taken for the magnesium strip to dissolve using the stop clock. I then repeated this experiment three more times, with 6ml of acid and 4ml of water, 4ml of acid and 6ml of water and 2ml of acid and 8ml of water. I then repeated this experiment two more times to get a fair test by proving that all my results were accurate, if they were inaccurate I repeated the experiment again, or ignored the wrong result. ...read more.

Conclusion

The graph gives us a good device to prove that if you double the concentration the rate of reaction doubles. Evaluation If I was to repeat this experiment I believe that the results would be a little different. The reason I think this is because; the reaction it self is exothermic. This mean because I used the same test tube through the experiment the temperature of the test tube was varied for every attempt. Next time I would use a water bath, this would control the temperature and wouldn't affect the experiment. The surface area affected the experiment. As I removed the oxide layer from magnesium, I could only remove certain amounts. Next time to ensure that I have both sides oxide layer free; I might use brand new magnesium. Also as the reaction produced alto of bobbles it lifted the magnesium strip on top of the acid, so it was floating the entire time. This affected the rate of the reaction because the magnesium strip wasn't entirely in contact with the acid. Also if I was to repeat the entire experiment I would use a burette to measure out the reactants. Also to make sure that I collected all the gas possible I would use a gas syringe. ...read more.

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