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

acid strengths affecting rate of reaction

Extracts from this document...

Introduction

GCSE Chemistry Coursework Aim My aim is to see how the strength of an acid varies how this affects the time is taken to produce 10ml oh hydrogen gas, using magnesium ribbon and 4 different strengths of HCL, 0.2m, 0.4m, 0.7m, 1m. Hypothesis I predict that the higher the strength of the acid, the quicker the time taken to produce the 10ml of gas required. I think this will happen as the stronger the strength of an acid the more h+ Ions to donate, so if the acid has more h(+) Ions then the higher the chance of it not only forming hydrogen gas but producing more of it, in a shorter period of time. Hydrogen gas is produced by, H2= 2H(+) + 2e(-). This then leaves the chloride ions, CL(-) to join with the magnesium and form a salt, magnesium chloride, CL(-) + Mg(+) =MgCL Fair Testing To make sure that the experiments are accurate and fair, I will use a fair and complicated procedure to make sure that the experiment is fair, thus giving more accurate results. These procedures are as follows; 1st I will make sure that the same amount (length) and weight of magnesium is used in each of the experiment, 2nd of all I will make sure that the same amount of HCL is put into the boiling tube in each of the experiments, I will be using 15ml of HCL through-out the experiments. ...read more.

Middle

I carried out several preliminary investigations. This allowed me to choose what strength acids would be best to use, because if the acid is too weak and take too long to fully dissolve then that is not an acid which I would consider appropriate to use in the investigation. Below is the results table from my preliminary investigations. Strength of Acid Time taken to dissolve 0.1m 1.55 minutes 0.4m 9.31 minutes 1m N/A I was unable to complete the experiment due to the time constraints of a 1 hour lesson; therefore I was unable to establish how long it took for all the magnesium ribbon to dissolve. Therefore it wasn't a fair test and they were inaccurate so I decided to change that experiment in favour of seeing how long it took the acids to produce 10ml of hydrogen gas. What I learnt from the Preliminary work The preliminary work showed me that using 0.1m hydrochloric acid was inappropriate, so I decide to not use it. To compensate and still use four strength acids I decided to use 0.7m as this was a realistic strength acid to be able to use in the experiment as it should react quite quickly and be achievable during one lesson. Using the equipment safely When carrying out the experiments I kept my goggles on at all times, I did this so the acid couldn't ...read more.

Conclusion

The accuracy of my observations again I feel was high, this can be backed up by my results as they returned no anomalies and they were very similar in cases when compared to the rest of the classes. Only minor things let the accuracy down, when stopping the stopwatch it is hard to stop it at the precise point when exactly 10ml of gas has been produced, so lowering the accuracy. Improvements which I could do to the method are to take more time when carrying out the experiment. As I had to stay within the time constraints of one lesson I couldn't spend as much time on being as accurate as I would have liked, although they were still accurate to a certain mark and are still very reliable. The reliability of my evidence is again as they are similar to others results from other experiments which were carried out in the same class, so they can be used without fear of them being in accurate or unreliable. The evidence I recorded is more than sufficient to firmly support my conclusion, as the conclusion states that as the strength of the acid increases the time taken to produce 10ml of hydrogen gas de-creases, which when compared to the evidence is exactly the same. So the evidence is more than sufficient so support a firm conclusion. Michael Kemp 1 ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Physical 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 AS and A Level Physical Chemistry essays

  1. Peer reviewed

    Gas Behaviours and the Weather

    3 star(s)

    Temperature and pressure increase in ratio with each other. High temperatures close to the Earth are caused by high pressure systems. High pressure systems drive the higher air to cool and become denser so that as it sinks towards the Earth, it becomes warmer (see Passante, 2006).

  2. Investigating the Rate of the Reaction between Bromide and Bromate Ions in Acid Solution

    where k is the rate constant for the reaction. The overall order of the reaction is the sum of the orders of reaction of the separate reactants, so reaction is (x+y)th order overall. Similarly to the orders of reaction, the value of the rate constant can only be found by experiment.

  1. The Determination of rate equation

    Sodium thiosulphate This aqueous solution may be harmful if swallowed and may also irritate the eyes or lungs. If it comes in contact with Eyes then wash the eye with plenty of water.

  2. Investigating the rate of reaction between peroxydisulphate(VI) ions and iodide ions

    The shape of this graph can therefore be used to calculate the order of reaction of potassium iodide ions in this investigation. The general equation for the rate of a reaction is: Therefore, it can be said that increasing the concentration of one or more reactants will cause an increase in the rate of reaction.

  1. detremining the rate equation

    * test tubes * stirring rod- to stir the reactants ones the are added together * stopwatch- this will be used to time how long it takes for the black cross to despappear. * 1M sodium thiosulphate * HCl- 2.0 moldm-3 * Na2S2O3 0.4 moldm-3 * Distilled Water * 3

  2. Investigating how concentration affects rate of reaction

    This means that the likelihood of collisions occurring is increased, so a reaction will happen sooner (as shown in figure 3). This increased the 'rate of reaction' as a reaction occurs in a shorter space of time. The diagrams below show this effect: (1, pg 221)

  1. Investigating the effect on the rate of reaction when changing the acid that is ...

    Some dissociate far greater percentages than others when in water. This dissociation in water is an equilibrium reaction, the measure of this equilibrium is the Ka value. The greater the dissociation the stronger the acid, this will produce a higher Ka value. [2]Example 100% HCL(g) + H20(l) CL-(aq) + H3O+(aq)

  2. Individual investigation - Reaction to be studied Rate of reaction between propanone and ...

    MAKING STANDARD SOLUTION: > Zero the scale with the watch glass in it. > Transfer the required mass of substance into the beaker. > From the watch glass, put the measured mass into the beaker and dissolve the substance with the distilled water.

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