• 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).

    I recognised the anomaly for the 2 molar set of results by looking at my graph. I looked at the molar 2 line of best fit and I could see that the point of the anomalous results was not stuck closely to the line.

  2. 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.

  1. Reactions between HCL and Marble chips.

    I could not control the room temperature but I assumed that the room temperature would stay around the same for the duration of the experiment. The temperature would affect the concentrations of the acid. I will start timing the collection of the gas when I replace the bung on top of the conical flask.

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

    What is the rate of a chemical reaction? The rate of a chemical reaction is how fast the reactants react. Measuring the reaction rates: In general to find the rate of a reaction, you should measure either the amount of reactant used up per unit of time or the amount of product produced per unit of time.

  2. An experiment to investigate the reaction between marble chips and HCl

    I will keep the 5g of 2-4mm CaCO3 chips constant throughout each experiment. I chose 2-4mm sized CaCO3 chips because I found in my preliminary that the 10-12mm sized chips were making the reaction too slow and so if I used smaller chips it would mean an increase in surface

  1. Effect Of Substrate Concentration On The Activity Of Catalase

    As well as this, hydrogen peroxide can be very harmful if it enters the eyes. Thus, goggles must be worn. Also, if available lab coats will also be worn. The cork borer is also a potential hazard as it is quite sharp.

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

    We noted down the temperature of the hydrochloric acid in the buckler flask before the reaction. 10. We then put the powdered marble into the buckler flask with an attached delivery tube and put a bung on top of it.

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