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

Investigating the effect of acid concentration on marble chips.

Extracts from this document...

Introduction

Investigating the effect of acid concentration on marble chips Planning: The aim of this practical is to investigate the effect of varying acid concentrations on marble chips (CaCO3) 2HCL + CaCO3 --> CaCl2 + CO2 + H20 Hydrochloric Acid + Calcium Carbonate --> Calcium Chloride + Carbon Dioxide + Water Increasing the concentration of an acid increases the number of collisions between particles, therefore, the rate of reaction increases. The reaction will start faster in comparison to the speed at the end of the reaction. This is because when the two reactants are first mixed, their concentrations are both at their highest. As the experiment goes on, the concentration of the reactants will slow down, so the reaction will slow down until it finally comes to a stop. Constants: o The size of the marble chips - all the marble chips used will be 6mm in length. This is because the surface area of the substance affects the rate at which the reaction takes place. A larger surface area means the reaction goes more quickly, so I need to keep the size of the chips equal so as to make it a fair test. ...read more.

Middle

By using these concentrations, I will be able to get a good range of readings and my results will be relevant. I also found out that there is a possibility of anomalies, for this reason I am going to take three readings for each concentration so that I can identify anomalies.. Apparatus: ==> Conical flask ==> Gas syringe ==> Rubber piping to link the above two ==> Safety goggles ==> Retort stand to hold up the gas syringe - Paper towel to be wrapped around the parts that hold the syringe so as not to break it. ==> Volumetric flask ==> Pipette ==> Mass balance ==> Beakers of different size. ==> Stop Clock ==> Rubber Delivery Tube ==> Bunk Safety note: Concentrated acid is very dangerous, when doing the experiment, I must be careful to ensure no acid is spilt as this could lead to corrosion work surface and skin. Also, I must be sure to wear safety goggles at all times when doing the experiment. Obtaining Evidence: Table of results: Concentration of acid mol/dm3 1 2 3 4 5 6 Time taken to reach 40cm3 s 1st reading 84.00 21.00 14.40 11.40 9.60 7.20 2nd reading 90.00 22.20 14.40 12.00 10.20 7.20 3rd reading 81.60 25.20 13.20 12.00 9.00 6.60 average 85.20 22.80 ...read more.

Conclusion

The repeat readings were, more or less, scattered in exactly the same time zone as the 1st reading. By this I mean that apart from the readings at concentration 1Mol/dm3, the repeats were all to within 5seconds of each other. I feel that, perhaps I could have used a two more repeat for each acid concentration as this would have made the results more reliable. At concentration 1Mol/dm3, the readings were scattered over a time range of 15seconds. This was expected as at the lower concentrations, it is harder to reproduce the experiment in exactly the same way so that the results are the same. As an extension to this experiment, I would go on to measure the change in mass over the course of the experiment. This means that I would put the conical flask on a mass balance and measure the mass after certain periods of time. There would not a bung in the top of conical flask, instead some cotton wool as this would allow the gas to escape but no air to get in. This would give another way to find out the rate of the reaction taking place between HCL and CaCO3. I can therefore conclude that the experiment was successful and I found out the aim of the experiment. Peter Hardie 1 08/05/2007 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 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. Investigate how concentration of hydrochloric acid (HCL) affects its reaction with calcium carbonate (CaCO3).

    This should have then doubled the chance of the calcium carbonate atoms and the hydrochloric acid molecules successfully colliding and reacting. However, by taking readings off the graph I can see that this is not the case. At 40 seconds on the 1 molar line 8.5cm3 gas has been produced.

  2. A report investigating the effect of Concentrated Hydrochloric Acid on Marble Chips (Calcium Carbonate).

    A common rate to measure is the rate of reaction between an acid and a carbonate. The equation is: Acid + Carbonate Salt + Water + Carbon dioxide HCl (acid) + CaCO3 (base) CaCl + H2O + CO2 Successful collision: The collision theory is used to explain these effects.

  1. Reactions between HCL and Marble chips.

    To obtain these results I then measured and recorded how. I predict that the solution with the high concentration of acid will have a much faster rate of reaction than the weaker solution. I have predicted this from my knowledge of a previous experiment and scientific knowledge.

  2. Investigation Into the Effect of Concentration On Rate of Reaction Between Marble Chips and ...

    However, we are intending to keep the surface area the same. Another factor is TEMPERATURE. Again, we are not going to alter the temperature. If we were to, the hotter the temperature, the faster the rate of reaction as the molecules would have more energy.

  1. The effect of concentration of acid on the chips

    If I were to conduct my experiment below this temperature then the reaction would not take place. I.e. consider it a game, and the object of the game is to injure yourself and other people so that you can leave the room.

  2. Investigate how concentration affects the rate of a reaction using marble chips (CaCO3 ) ...

    40 mls 10 mls 50 mls 0 mls We have chosen to use 50mls of solution as that is a reasonable amount to use to react with the marble chips. We decided to have a difference of 10mls each time to compare the concentrations against one another; it gives us

  1. Investigation to discover the affect of varying concentrations on the rate of reaction of ...

    The acid does not dissolve the limestone chips it reacts with them as two separate reactants; the shape of the chips stays the same but after the experiment they cannot be used again because the acid would have used all the potential reactant energy to make the gas substance.

  2. How does the concentration of HCl affect the rate of reaction with CaCO3?

    We noted down the temperature for the reactants because we couldn’t keep the temperature constant. Results Concentration (molar) Volume of carbon dioxide produced (cm³) average amout of carbon dioxide produced Time (seconds) Rate of reaction (cm³/s) Temperature (°C) 1 2 3 4 5 start of experiment end of experiment 0.50

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