• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

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

Extracts from this document...

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.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Aqueous Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Aqueous Chemistry essays

  1. To investigate the rate of reaction between different concentrations of hydrochloric acid with metal ...

    45ml acid- 5ml water- 1.8 molars (90% concentration) 40ml acid-10ml water-1.6 molars (80 % concentration) 35ml acid-15ml water- 1.4 molars (70% concentration) 30ml acid-20ml water- 1.2 molars (60% concentration) 25ml acid-25ml water- 1 molars (50% concentration) 20ml acid-30ml water -0.8 molars (40% concentration)

  2. The effect of Acid Rain on Seed Germination.

    cress started and finished, then simply measure the string on a ruler. The data I received I believe is reliable. I conducted the experiment as accurately as I could with the apparatus I was given. If my method was improved with the suggestions I have already made then my final results of the experiment would be more reliable.

  1. DECOMPOSITON OF HYDROGEN PEROXIDE WITH HEAVY METAL CATALYSTS

    95 93.5 86 91.5 190 100 94 88 94.0 200 100 95 90.5 95.2 The line graph on the next page shows the average amount of oxygen produced by manganese oxide against time in seconds. Adding up all the readings and dividing by all the readings taken i.e.

  2. Rates of Reaction

    the solid have a greater surface area compared to larger pieces of the solid. Therefore, there is more chance that a reactant particle will hit the solid surface and react ultimately causing a successful collision. I will therefore keep the surface area of the reactants the same in my experiment.

  1. Rate of Reaction

    following results obtained -Make sure to keep the angle of which the gas syringe was positioned at the beginning the same throughout all the experiments. So as to keep the force that the syringe has to exert as CO2 enters to get to a certain distance the same.

  2. Investigating rates of reactions. The reaction I am going to be looking at is ...

    Concentration 6 (hydrogen produced cm3) 10 45 47 30 7 5 0 20 64 74 1 15 9 30 84 67 23 15 40 110 70 30 17 50 71 38 21 60 72 44 26 70 49 30 80 54 33 90 58 38 100 64 41 110 67 44 120 73 49 130

  1. Investigating the kinetics involved in the reaction of metals with acids.

    To create accurate results, the all the concentrations should be carried out two more times. Once the times have been recorded for hydrochloric acid, repeat the experiment with ethanoic acid using the same concentrations. Firstly heat the water to 60oC, using the thermometer in the water to measure the temperature.

  2. The Effect of Concentration on the Rate of Reaction.

    Very few molecules of the reactant acquire this activation energy. The energy that the reactants must gain to overcome the energy barrier is called the activation energy. If molecules are moving fast enough part of their kinetic energy is converted into activation energy.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work