• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month
  1. 1
  2. 2
  3. 3
  4. 4
  5. 5
  6. 6
  7. 7
  8. 8
  9. 9
  10. 10
  11. 11
  12. 12
  13. 13
  14. 14
  15. 15
  16. 16

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

Extracts from this document...


TO: Dr. Al - Khalidi FROM: Nadia Falcon (11-MHA) - Baylis Court School. SUBJECT: DATE: March 9, 2001 TITLE: A report investigating the effect of Concentrated Hydrochloric Acid on Marble Chips (Calcium Carbonate) ( Planning ( Introduction ( Hypothesis/ Prediction ( Apparatus & Safety ? Method ? Fair Test ( Experiment ? Results/Table ? Graph ( Conclusion ? Evaluation Aim & Planning: Aim: In this report on Reaction Rate, I am required to investigate how altering the concentration of Hydrochloric Acid (HCl) affects the rate of reaction with Marble chips (Calcium Carbonate - CaCO3). Plan: My plan will be to add certain amount of acid and 3g of marble chip in a tube. I will leave it for 1 minute and measure the amount of carbon dioxide produced. I will then add some water to make it even. Next, I will add a little more Hydrochloric acid to make it concentrated and again leave it for 1 minute and measure the amount of carbon dioxide produced. I will repeat this process several times. A number of reactions would be carried out in which the temperature and volumes of calcium carbonate will be kept the same, but the concentration of each reaction would be different. I will record these results and repeat this processes five times using different concentrations of hydrochloric acid. Finally, I will be performing the actual experiment to this effect and the details will be noted down in a table supported by a graph to support my experiment. Introduction: I am also going to explain the reaction between Hydrochloric acid and Marble chips (calcium carbonate) by changing the factor (variable) of Concentration in this investigation. I will alter the concentration of the hydrochloric acid each time, and then measure the amount of Carbon dioxide gas given out. The chemical equation for this reaction is: HCl (acid) + CaCO3 (base) ---> CaCl + CO2 + H2O Background Information: Calcium Carbonate - The chemical formula for calcium carbonate is CaCO3. ...read more.


As this happens the rate of reaction slowly decreases and levels at the same point. The key point however, is that, the higher concentration reaction will achieve this in a shorter amount of time, hence my graph will have a steeper initial gradient and will level off to 0 once the reaction stops. Hence, more diluted is the solution, the lesser is the amount of carbon dioxide gas produced. I would expect to obtain the diagram of my experiment something as shown below, (if I dilute the HCL acid with different measurements of water at each stage). Volume of acid (cm3) Apparatus & Safety: Test tube Stopper Rubber-tubing Syringe Timer Top-pan balance or mass balance Marble chips Dilute Hydrochloric Acid Distilled water 2 Clamps Safety: Before starting with performing the experiment, we have to ensure, to follow the outlined safety procedures: Laboratory Safety - Protective clothing * Students must wear protective glasses or safety goggles when diluting concentrated acids, bases, or heat chemicals. There is always the danger of hot or caustic materials being splashed into the eyes. * Students should wear strong shoes and take care of unbuttoned long sleeves and long hair. * Students must wear protective clothing, e.g. gloves, aprons, safety goggles when chemicals are being handled. Teachers should be aware of students who wear contact lenses. Laboratory Safety - Experimental procedures * While performing the experiment, students should ensure to set the things in the middle of the table and not at the side because it may fall off. * Read the label on reagent bottles twice to avoid errors. * Always follow exactly the instructions for chemical experiments. * Do not substitute another chemical for chemicals specified in the experiment. * Clean up the area after use. * Wash your hands. Method: Since I have written my hypothesis (prediction with explanation) and outlined the apparatus and safety measures, my next step is to decide how to do the experiments. ...read more.


If I were to do this experiment again, I would probably make it more accurate by using a Burette instead of a syringe, to measure the amount of gas given off, because a burette is accurate to 0.1 ml. Also, the readings of the volume of gas collected after each minute should have been made until the reaction is complete for each experiment. It means, the reaction should stop in each case when the marble chips, has completely dissolved. So, I feel that given full time for the chips to dissolve in each experiment, would have given me much more accurate measurements and show at which points the rate of reaction was at best and the curve line of reaction on the graph. From this graph it may well be clear that one or two individual results, or a whole set of readings, may not fit very closely to the trend - anomalous results! The measurements may not be that accurate because, this experiment was done on two different days, i.e. one set of results was done on a different day when the temperature in the room may have been different. To ensure that there is place for improvement and if I had to do the experiment all over again, I will have to do the following to improve the accuracy of my results: * Wait for final measurement until the reaction is complete and the marble chip has completely dissolved. * I will ensure that the experiment is done on one day itself, because a change in temperature does effect the rate of reaction. * I will ensure that the test-tube and syringe is completely dry, before I start with the new experiment. In many reactions it is not convenient to measure concentration - instead some other property is monitored which represents the concentration directly, e.g. loss in mass, production of gas, change in color, change in pH, change in conductivity or change in pressure. If I increase both variables, (temperature and concentration) the rate of reaction will definitely increase. 8 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

    Marble Chips and Hydrochloric Acid.

    4 star(s)

    Therefore, we know that 100g of Calcium Carbonate is equal to 1 mole. We also know that 1 mole of gas will always occupy the same volume. This volume is 22, 400cm�. Step 2 We have calculated that: 100g of CaCO 22, 400cm� of CO In our experiment we will

  2. Investigating the reaction between Marble Chips and Hydrochloric Acid.

    for 2 Molar Acid 0 23 47 192 87 n/a 1.8 0 23 42 61 81 97 1.8 0 21 39 59 78 93 1.8 0 22 39 60 81 95 Average Results for 1.8 Molar Acid 0 22 40 60 80 95 1.6

  1. Measuring the Rate of Reaction between Hydrochloric Acid and Calcium Carbonate

    clamp, 25cm� measuring cylinder (6), calcium carbonate (1g of small chips), glass vile, stop clock, small calcium carbonate chips and a balance. - I will wear my safety equipment - goggles and overall - I will measure 1g of calcium carbonate small chips in a glass vile.

  2. An Experiment To Investigate The Rate Of Reaction Between Marble Chips And Hydrochloric Acid.

    This can be done in a few ways. Heating up a reaction gives the particles more energy, making more particles collide with the activation energy. Another way to speed up a reaction is to increase the concentration of reactants, which means that there are more particles to collide with each other making collisions occur more frequently.

  1. Investigate how concentration of hydrochloric acid (HCL) affects its reaction with calcium carbonate (CaCO3).

    This is because at the start of the reaction there are plenty of magnesium atoms and acid particles. But as the time goes by these particles get used up during successful collisions. After more time there are less marble atoms, and the acid is less concentrated.

  2. Free essay

    How does Concentration affect the rate of reaction between Hydrochloric Acid and Calcium Carbonate

    30 40 0.75cm�/s 20% HCl 80%H2O 30 85 0.35cm�/s This shows us that the rate of reaction decreased as the concentration of HCl lowered. Conclusion The rate of reaction graph has a positive correlation between the rate of reaction and the concentration; however the line of best fit is not linear but curved.

  1. How the temperature affects rate of reaction between marble chips and hydrochloric acid?

    However when the temperature is increased to 65�C, the time taken to collect 30ml� of CO2 is only 11 seconds. This clearly shows to prove that my prediction was correct. The graph shows a smooth curve which becomes more horizontal as it reaches higher temperatures.

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

    and put a bung on top of it. We removed the bung when the experiment had been going for 1 minute. We noted down how much carbon dioxide was produced and washed out our flask with distilled water after the experiment to get rid of contaminates.

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