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The effect of change in concentration of Hydrochloric Acid On its reaction with Magnesium metal.

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Introduction

The effect of change in concentration of Hydrochloric Acid On its reaction with Magnesium metal Magnesium is a light, shiny grey metallic element, with the symbol Mg and atomic number 12. Magnesium is found in group two of the periodic table. It is a reactive metal giving vigorous reactions towards acids. Magnesium is used in alloys, flash photography, flares, fireworks and flash bulbs. Hydrochloric Acid, HCL, is a typical monobasic acid and is corrosive. It releases hydrogen ions when it is added to water and certain metals and has a Ph of less than 7. Equation: Magnesium + Hydrochloric Acid Magnesium chloride + Hydrogen (Information from chemistry- Martin Stirrup, exercise book and internet) For a chemical reaction to happen the particles need to collide with each other and they need a certain amount of energy to break the bonds. As I dilute the acid and the concentration becomes less the reaction will become slower as there is less energy to break the bonds. The variables I could use are: * Temperature: increase of temperature produces an increase in the rate of reaction. ...read more.

Middle

* Measuring cylinder- to measure acid and water * 2m acid * water * magnesium Safety: While doing this experiment I will carry out these safety precautions. Always wear safety goggles to protect eyes from the Hydrochloric Acid. Keep all the apparatus away from the edge of the desk to prevent breakages. 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 ribbon. Prediction: I predict that as the concentration of Hydrochloric acid decreases, the time taken for the Magnesium to dissolve increases. Method: Firstly I measured out the amount of 2m Hydrochloric acid using the measuring cylinder. I used the measuring cylinder to pour the acid into the conical flask. Then I cut my magnesium into 1/2 cm pieces then added it to the acid, and started the stop clock at the same time. When the magnesium ribbon had stopped fizzing, I stopped the clock and recorded the time. I used the same method only when I had done three readings of the same concentration, I then replaced 20% of acid with water each time. ...read more.

Conclusion

The higher concentration the faster rate of reaction. It was a fair test and there is only one anomalous result that I could find. My anomalous result was with 60mls acid and 40mls water. The result for this was 69 seconds but from what the line of best fit shows, it should have been around 56 seconds I could improve the investigation by taking more care in measuring out the different amounts of liquid more accurately. I also think that we should have done all the experiments on the same day as the temperature in the room would have been the same. The factors that could have caused my anomalous result are: * condition of magnesium * temperature in the room of the day of the practical * accuracy of measuring I could have improved some of these by checking that all the magnesium was all the same size before putting it into the hydrochloric acid and that I use the same concentrated acid in every repeat i.e. 2 molar. In this investigation I found out that the higher the concentration, the faster rate of reaction. I think my investigation was a fair test and that I got a good accurate set of results. Catrina Kottritsch ...read more.

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