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

To Investigate the Effect that the Concentration of Acid has on a Reaction

Extracts from this document...

Introduction

-Experiment- To Investigate the Effect that the Concentration of Acid has on a Reaction between HCl and MCl Introduction: The reaction that I am investigating in this experiment is the reaction between dilute hydrochloric acid and magnesium ribbon. The equation for this experiment is shown below: 2HCl + Mg MgCl2 + H2 What I actually will be investigating is the effect that the concentration of Hydrochloric acid has on the rate of reaction. To start off with the concentration of HCl which will be used is 4 molar. But to do the experiment I will have to use 8 different concentrations of the hydrochloric acid, and try the experiment 8 different times using a same-size piece of magnesium ribbon but different concentrations of the acid. The concentrations of the acid that I am going to be using are : 4.0m, 3.5m, 3.0m, 2.5m, 2.0m, 1.5m, 1.0m, and 0.5m. In this experiment I will be using magnesium ribbon as a reactant along with hydrochloric acid. Magnesium is a highly reactive metal, which is pretty high in the reactivity table for metals. What I will be investigating in this experiment is to try and find out weather or not there is any correlation between the concentration of the Hydrochloric acid and the rate of reaction. I will be using 8 different concentrations of the acid, which are shown above. A piece of magnesium ribbon will be dropped into the acid solution and the time it takes for the ribbon to completely disappear will be recorded using a stopwatch. Because this reaction is between an acid and a metal then there will be two main products formed which will be a salt and a gas. In this case the salt produced is Magnesium Chloride and the gas produced is hydrogen! Acid + Metal Salt + Gas Hydrochloric + Magnesium Magnesium Chloride + Hydrogen Acid This reaction is an Exothermic Reaction. ...read more.

Middle

Collision theory is the name given for the amounts of ions, which collide in a certain reaction. This explains that if there are more ions in a solution then there will be more collisions between the ions in the solution and more collisions between the reactants in that reaction. This is because the ions are closer together and there is more of a chance that they will collide with other ions in the solution. Apart from increasing the amount of ions in a solution (increasing the concentration), there is another way in which the collisions between ions can be increased! This is by giving the ions already in the solution more energy. We must consider what happens when a reaction takes place. First of all the particles of the reacting substances must collide with each other, and secondly a fixed amount of energy called activation energy (Ea.) must be reached if the reaction is to take place. If the particles can produce the right amount of energy (i.e. if they collide fast enough and in the right direction) a reaction will take place. The reaction is speeded up if the number of collisions is increased. This energy is heat, when heat is added to the experiment it increases the energy in the ions, which makes them move around in the solution a lot faster. This means that the ions will collide more frequently and more vigorously increasing the rate of the reaction and the amount of collisions in the reaction. This also explains why the greatest rate of reaction is usually as soon as the reactants have been mixed; i.e. they are both at their highest concentrations. As the reaction continues, the concentration of the reacting substances decrease and so does the rate of reaction. The higher the concentration of HCL you use, the less time it takes for the magnesium to disappear and so the rate reaction increases. ...read more.

Conclusion

This would mean that the average would be more accurate and that the results would be fairer because any anomalous results would be counted out because the results would be averaged to get the final set of results. This would also have implications on the conclusion, which could be slightly wrong because of the inaccuracy of the results! Maybe the rate of reaction was proportional to the concentration of the acid but because of the inaccuracy of the results it might not have been shown that the results actually are proportional to one another. These are all things that I could do to improve the accuracy of the experiment. Another thing which would increase the accuracy of the results, although not dramatically would still add to the accuracy and fairness of the experiment would be to keep the beaker with the reacting solution in it in a water bath which would be kept at the same temperature throughout the whole experiment, this would ensure that there would be no change in the temperature of the solution. A change in temperature could have happened whilst the experiment was taking place so this water bath idea would account for any temperature changes and get rid of them. These three factors bellow could also effect the fairness and accuracy of the results I obtained but I could do nothing to change them. 1) When the reaction takes place bubbles of H2 are given off, which might stay around the magnesium which therefore reduces the surface area of the magnesium and so the acid cannot react properly so this effects the results. 2) We could have controlled factors in the investigation better (e.g. the stirring of the solution because if this isn't done properly it can lead to incorrect results). 3) Using larger concentrations of acid would give a bigger more accurate conclusion instead of just using 10ml test tubes use 1litre test tubes, this way graphs would be more spaced out and give an accurate form or curve Chemistry Coursework Completed By: - Colin Stuart Form 11-2 Colin Stuart 11.2 ...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 Patterns of Behaviour 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 Patterns of Behaviour essays

  1. Marked by a teacher

    The Effect of Concentration on the Rate of Reaction between Magnesium [Mg] and Hydrochloric ...

    4 star(s)

    As the reactant particles will also move more quickly the frequency of the collisions also increases. If the temperature is low the reactant particles consist of less energy. So when particles are heated they gain more energy. As they gain more energy this enables them to move around faster, this

  2. Marked by a teacher

    In this project I am going to investigate rates of reaction of an indigestion ...

    3 star(s)

    Average (secs) Rate 10 44.0 1.1 15 42.0 1.2 18 30.0 1.7 20 24.5 2.0 24 18.0 2.8 30 15.5 3.2 36 14.0 3.6 40 11.5 4.3 50 10.0 5.0 A graph showing temperature against rate of reaction while collecting 50cm� of carbon dioxide gas when 50cm� of Hydrochloric acid is added

  1. The effect of temperature on the rate of reaction between magnesium ribbon and hydrochloric ...

    When it comes to doing my actual method I will use a constant length of magnesium which will be decided from the preliminary trial. The maximum length of magnesium I can use in all the actual experiments is 40cm. Safety: The reaction between magnesium ribbon and hydrochloric acid can be

  2. How does changing the concentration of the Hydrochloric acid affect it reactions with Magnesium?

    To get a fair reaction we had to keep the amount of magnesium the same and the concentration of the acid. In the experiment we used 0.1g of magnesium and the concentration of the acid was 50cm3 of acid to 50cm3 of water.

  1. To investigate the effect of the concentration of nitric acid on the rate of ...

    (See conversion table) 4. Place the magnesium granules into the conical flask. 5. Immediately afterwards, pour the acid into the conical flask and quickly seal it with the rubber cork. 6. At the same time, start the timer and begin to observe the amount of gas produced using the gas cylinder.

  2. Investigating the Rate of Reaction Between Hydrochloric Acid (Hcl) and Magnesium (Mg).

    to have formed a layer of oxide, a black substance, around it. I will use sand paper to remove the oxide. If the oxide is not removed it will be an unfair test, because the reaction will take longer, as the oxygen layer acts as a shield, and it will

  1. Rates of reaction between Magnesium and HCl.

    The steeper the slope of the line, the faster the reaction. For example the gradient for when the concentration of the hydrochloric acid is 1M is Gradient= Vertical change Horizontal change =0.6 For when the concentration of the hydrochloric acid is 0.9M: Gradient = 0.4 From this example, I can

  2. Rate of reaction between magnesium ribbon and hydrochloric acid.

    My prediction went on to say "I also predict that as the concentration doubles the rate of reaction will double, this is because there are more molecules in a given volume, in 2m hydrochloric acid there are twice as much molecules than in 1m of hydrochloric acid", the rate of reaction did not double according to my results.

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