• 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

Does the concentration of hydrochloric acid affect its rate of reaction with calcium carbonate?

Extracts from this document...


Chemistry Investigation: Does the concentration of hydrochloric acid affect its rate of reaction with calcium carbonate? Aim As stated in the title, I will investigate the differences in the rates of reaction between hydrochloric acid and calcium carbonate if the concentration of the acid is varied. This is the equation for this reaction: 2HCl + CaCO3 CaCl2 + H2O + CO2 Hydrochloric acid + Calcium Carbonate Calcium chloride + Water + Carbon Dioxide Possible Variables that could be used The variables that may have an affect on this experiment are: * Size of marble chip - the size of the marble chip will affect our experiment, because this dictates the surface area. The larger the surface area, the more acid that will be in contact with the hydrochloric acid and able to react. * Concentration of hydrochloric acid - this is the proportion of hydrochloric acid in the solution. * Volume of acid - this will be the amount of hydrochloric acid that will be reacted with the marble chips. * Catalysts - weakening bonds increases the rate of reaction by lowering activation energy. A catalyst will not be used in this reaction, however. ...read more.


This should make a graph of the reaction curved as the reaction rate slows down. The increase in the concentration should be directly proportional to the increase of the reaction rate at a given time. This is because by doubling the number of hydrochloric acid molecules present, the chance of a collision should be doubled, as there is now twice the possibility of a collision-taking place. Activation energy should not be changed in this experiment though as the same amount energy will be required to break the bonds. This is because each particle has the same amount of energy, and the only reason the reaction is faster, is because there are more particles. This means activation energy will not have an effect on this experiment. Method Procedure 1. Attach a delivery tube to a conical flask. 2. Fill a tub with water to produce a water bath. 3. Measure out 5g of calcium carbonate on a piece of paper on some electronic scales. 4. Measure out 50cm� of hydrochloric acid solution in a measuring cylinder. 5. Fill a 100cm�-measuring cylinder with water and put it upside down on top of a beehive jar in the water bath so that none of the water inside the cylinder escapes. ...read more.


It could not be fully determined whether the increase in concentration would increase the rate of reaction whether we continued this experiment with much larger figures. This could be found out by extending the range of concentrations that could be reacted with calcium carbonate. This experiment would have to be conducted very carefully as hydrochloric acid at high concentration can be very dangerous, and the fact that a lot more time and preparation would have needed to be taken to maintain the levels of safety. The method showed the relationship between the concentration and the rate of reaction, but there was a slight margin of error because turning the cylinder upside was such a delicate operation, that it was very difficult not to lose some water. To solve this problem we could use a gas syringe, but the difficulty with this is that we could not test the higher volumes of gas, which would mean the range of results would be lower. This would lead to us withdrawing a less formulaic pattern. The experiments were fair tests but there was a margin of error because the scale with which we recorded our results was not precise enough (to 1 cm3), and the values of the controlled variables were not the exact amounts, thus giving us false results and misinterpreted formulae. ...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 Aqueous 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 GCSE Aqueous Chemistry essays

  1. Marked by a teacher

    To see how the concentration of acid, reacting with potassium carbonate, affects the rate ...

    4 star(s)

    To measure the rate of reaction I will collect the carbon dioxide produced and record the time taken every 10 seconds. This will tell me the speed of the reaction because, e.g. if a small amount of gas is produced in a long time then I will know it is slow reaction.

  2. Peer reviewed

    The Effect of Concentration on the Rate of Reaction when you React ...

    3 star(s)

    This gave a lower average time. This does not affect the overall claim because the difference between 2 molar and 2.5 molar concentrations is so small that it is likely that it could have happened anyway. The results gathered supports my prediction that as the concentration of acid increases, the rate of reaction will decrease.

  1. To investigate the rate of reaction between different concentrations of hydrochloric acid with metal ...

    + H2O (l) H+(aq) + Cl-(aq) The solution formed when the HCl acid dissolves in water contains a high concentration of H+(aq) ions. This means that it is a strong acid, as the acid breaks up into ions (ionises) almost completely into H+(aq)

  2. Investigating the effect of temperature on the rate of reaction between hydrochloric acid and ...

    I identified the anomalous results by highlighting them. All of the results in the second experiment of 70� were anomalous. I left these out of the calculations for average and highlighted them to show they are anomalous. The following caused problems with the experiment: - - The acid was a different concentration from one experiment to another.

  1. Investigate how the concentration of 10 ml of hydrochloric acid affects the rate of ...

    The fact that the reactions involving higher concentrations of hydrochloric acid slow down at a higher rate is due to the fact that the reaction rate is so fast that there is not enough marble left towards the end for the reaction to reach its full potential.

  2. How much Iron (II) in 100 grams of Spinach Oleracea?

    If the end point had not been reached, (i.e. the solution did not appear as dark in colour as the others at the end point) the average titre point would be lower; therefore the concentration of Iron (II) would appear lower suggesting that the solution was less concentrated. If either of these had occurred the redox titration would have appear less accurate.

  1. Investigating the effect of concentration on the rateof reaction between marble chips and Hydrochloric ...

    If the acid were less reactive the reaction would take place slower, therefore less carbon dioxide would be produced overall, and at a slower rate. Proving the Prediction On the whole, my prediction was more or less right. As the acid got weaker, the amount of gas produced, decreased, apart from at the 70% concentration, where it instantaneously increased.

  2. Investigate how the concentration of hydrochloric acid affects the rate of reaction between calcium ...

    CaCo3 + 2HCL CaCl2 + H2 O + CO Reactant Product I think that the rate of reaction is affected by the concentration of the hydrochloric acid because the rate of reaction depends on how frequently the reactant particles of the reacting substances collide.

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