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Magnesium Sulphate (MgSO4) as an Anti-Inflammatory Agent Investigation

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A Medicinal Problem Introduction: This is an investigation to try to produce Magnesium Sulphate (MgSO4) in an efficient way as an anti - inflammatory agent for medicinal purposes. The company producing Magnesium Sulphate has received a very large order due as soon as possible. One way of producing Magnesium Sulphate is to add Magnesium (Mg) to Sulphuric Acid (H2SO4). A chemical reaction takes place because the Magnesium is higher up in the reactivity series than the Hydrogen (reactive part of any acid) and therefore replaces the Hydrogen to form Magnesium Sulphate. Scientific Knowledge: Part of scientific knowledge is the collision theory which firstly states that for particles to react they must first collide. Secondly for reactants to react they require a minimum amount of energy. The rate of reaction is related to the collision theory since that for there even to be any rate of reaction the collision theory has to take place. Strong acids have pH's of 1 - 2 and react a lot more violently than weak acids of pH 5 - 6. The pH of acids change around one main factor the quantity of Hydrogen ions in the solution of any acid. ...read more.


Likewise I didn't choose the Surface area of the Magnesium as this would be even harder that the temperature as the surface area is next to impossible to work out as a human and I don't have a computerized tool of such nature at my disposal. Whether or not a catalyst was present was not what I chose because Catalysts are not as easy to measure as the temperature at which the experiment is being carried out. Now the variables have to be identified and placed into the correct categories. The independent variable (what is going to be investigated by being change during the experiment) is the concentration of the Sulphuric Acid. The dependent variable (what is going to be measured) is the time taken for each reaction to take place. The controlled variables ( what needs to be kept constant for a fair test to be achieved) one is the temperature at which the reactions are carried out at, another is the mass of magnesium ribbon used and finally the apparatus used throughout the experiment. There is a prediction required for this experiment and what I predict is; that as the concentration of the Sulphuric Acid increases the time taken for the reaction to be completed decreases. ...read more.


This is the type of graph that I would expect to obtain: R A T E S O F R E A C T I O N TIME (S) To work out the concentration of the dilute Sulphuric Acid, 25 is divided by the volume of dilute Sulphuric Acid. The number 25 is chosen simply because the total volume of liquid (Sulphuric Acid + water) at the start of each reaction is 25cm3. The mean (average) time can be calculated by taking the two similar times and adding them together and dividing by 2. The rate is then calculated by dividing 1000 by the mean time (seconds) taken for the reactions to be completed. I will ensure that the results achieved from this experiment are precise and reliable by repeating them for as many times as necessary, until similar results are obtained. Obtaining Evidence: The results that I got when I did the experiment are as follows: There were no changes made to my original plan. My results did produce some inconsistancies because I had to repeat four of them a third time to ensure an accurate average is obtained. Even after repeating the results a fourth time there was more time available for me if it had been required. Evaluating: ?? ?? ?? ?? ...read more.

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