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

Free essay example:

How does concentration affect the rate of reaction between calcium carbonate and hydrochloric acid?

For our coursework investigation we tested how concentration affected the rate of reaction between calcium carbonate and hydrochloric acid. We experimented with the reaction:

Calcium Carbonate + Hydrochloric Acid               Calcium Chloride + Water + Carbon Dioxide

CaCO3 + 2HCl              CaCl2 + H2O + CO2

The rate of reaction is a measure of how quickly a reaction happens. In this instance, we are timing how long it takes for our reaction to produce 50cm3 of carbon dioxide. For chemists synthesizing chemicals, working out the rate of reaction is important as the procedure must be as efficient as possible. A reaction that occurs too quickly could be hazardous, and it is not practical for a reaction to take several days to complete. In our experiment the independent variable would be the concentration of hydrochloric acid, the dependent variable would be the amount of carbon dioxide, and the main variable which we had to control was the reading of carbon dioxide in the cylinder. We also had to make sure the room temperature was similar each day, as this could have affected our results.

We had the option of the surface area, the concentration or the temperature as our independent variable to affect the rate of reaction. We did not choose temperature as our independent variable as sustaining the temperature required was hard to do, and getting chemicals to a certain temperature was very difficult. We did not choose surface area as cutting the calcium carbonate tablets was difficult as the tablets often crumbled once cut. This left concentration as the best possible remaining independent variable.

I predict that the higher concentration of acid, the higher the rate of reaction. I predict this as collision theory states that “Anything that increases the number of successful collisions per second will increase the rate of reaction”. The higher concentration of hydrochloric acid will increase the amount of successful collisions per second as there will be more hydrochloric acid particles to collide with the calcium carbonate particles.

We had three different methods to choose from for measuring the carbon dioxide. The methods were:

Method 1: Collecting gas produced

  • Reaction takes place in a flask. Carbon Dioxide goes up a gas burette and into a measuring cylinder full of water.

Method 2: Timing how long it takes for a solid to dissolve

  • Reaction takes place in a flask.  Time it takes for Calcium Carbonate tablet to fully dissolve measured.

Method 3: Measuring loss of Mass

  • Reaction takes place in a flask. Flask placed on scales with cotton wool blocking up top. The mass is measured every 10 seconds.

Each method has its drawbacks, however. Method 2 had a large scope for human error as it is extremely hard to tell when the calcium carbonate table has dissolved. Method 3 did not work as the scales were not accurate enough, and the changes in mass were not drastic enough to come up with a conclusion. This left us with method 1 as our chosen method. For this method we needed the following equipment:

  • Empty plastic tub
  • Gas burette
  • Flask
  • Clamp stand
  • Measuring cylinder
  • Stop watch

And the equipment was laid out like this:

This is a step by step guide to our method:

  • We half filled the plastic tub with water
  • We filled the measuring cylinder full of water and put our thumbs over the top so that no air bubbles could get in. We then flipped the cylinder upside down and put it into the plastic tube, and attached one end to the clamp stand
  • We poured our hydrochloric acid solution into the flask, and attached the gas burette to the flask
  • We the put the other end of the gas burette into the measuring cylinder
  • When ready, we put the calcium carbonate tablet into the flask and began the timer
  • Every 5 seconds, the amount of water lost from the measuring cylinder was measured and the results were recorded
  • Once over 50cm3 Carbon Dioxide has entered the cylinder, the timer is stopped and a new experiment is set up

For our experiment we had to take several safety precautions. When we were handling the hydrochloric acid we made sure that we were extremely careful, and if we did spill and of the solution onto our hands, we made sure to wash it off very quickly, as hydrochloric acid is extremely corrosive. We also wore goggles whilst the experiment was taking place in case any of the solution may have managed to shoot into our eyes.

Preliminary Experiment 1 – Collecting Gas Produced

Time (Sec)

Concentration Hydrogen Peroxide Solution

100%

80%

60%

40%

20%

5

0

0

0

0

0

10

16

13

7.5

7

4

15

33

26

14

9

6

20

46

39

21

13

8

25

50+

46

28

17

9

30

50+

50+

33

20

10

35

50+

50+

40

23

12

40

50+

50+

44

26

14

45

50+

50+

49

30

16

50

50+

50+

50+

32

17

55

50+

50+

50+

36

18

60

50+

50+

50+

40

20

65

50+

50+

50+

42

24

70

50+

50+

50+

45

25

75

50+

50+

50+

50+

27

80

50+

50+

50+

50+

29

85

50+

50+

50+

50+

30

90

50+

50+

50+

50+

32

95

50+

50+

50+

50+

33

100

50+

50+

50+

50+

34

105

50+

50+

50+

50+

35

110

50+

50+

50+

50+

37

115

50+

50+

50+

50+

39

120

50+

50+

50+

50+

40

125

50+

50+

50+

50+

41

130

50+

50+

50+

50+

42

135

50+

50+

50+

50+

43

140

50+

50+

50+

50+

44

145

50+

50+

50+

50+

46

150

50+

50+

50+

50+

48

155

50+

50+

50+

50+

50+

Preliminary Experiment 2 – Timing how long it takes for a solid to dissolve

Concentration Hydrogen Peroxide Solution

Time taken for tablet to dissolve

100%

1:25

80%

2:00

60%

2:19

40%

3:04

20%

5:20

Preliminary Experiment 3 – Measuring loss of mass

Time (Sec)

Concentration Hydrogen Peroxide Solution

100%

80%

60%

40%

20%

0

54.07

54.12

53.66

54.59

52.33

20

54.03

54.07

53.64

54.56

52.32

40

54.00

54.05

53.61

54.52

52.30

60

53.98

54.02

53.59

54.52

52.28

80

53.98

54.01

53.55

54.50

52.27

100

53.96

54.00

53.54

54.49

52.26

120

54.00

53.54

54.47

52.26

140

54.46

52.26

160

52.25

180

52.23

200

52.21

220

52.21

240

52.20

Our preliminary experiments helped us decide several things about our method. For instance, we started off by saying that we would take a measurement every 10 seconds, but after our first experiment (100% HCl, 0% H2O) only took 15 seconds to complete. We then decided on taking a result every 2 seconds, however, by the time we got to our last experiment (20%HCl, 80% H2O) we tookfar too many meaningless measurements, where there was no change in the amount of CO2.

There were certain control variables which we had to make sure did not affect our results. The main control variable which we could not control was the room temperature. Temperature affects the rate of reaction as explained in Collision theory. Increasing the temperature would increase both the number of collisions per second AND the percentage of successful collisions. However, to make sure that the room temperature had as little affect as possible. We took all of our measurements in the summer, and every day we measured the room temperature to make sure that there was no major difference between days. The other main control variable was human error, which we could control by taking our time, not hurrying and staying focused during our experiment. We also repeated every experiment 5 times to identify outliers and eventually give a mean and ranges. Whilst repeating the experiment does not make it a fair test, it does make the results more reliable.

This is our results table:

Time (Sec)

100% HCl, 0%HO

80% HCl, 20%HO

60% HCl, 40%HO

50% HCl, 50%HO

40% HCl, 60%HO

20% HCl, 80%HO

Key:

5

0.0-0.0-0.0

0.0-0.0-0.0

0.0-0.0-0.0

0.0-0.0-0.0

0.0-0.0-0.0

0.0-0.0-0.0

Lower Range - Mean - Upper Range

10

10.0-12.75-15.0

8.0-8.8-11.0

6.0-7.8-9.0

3.0-4.0-5.0

5.0-5.6-6.0

0.0-1.8-4.0

15

28.0-29.75-34.0

19.0-20.8-24.0

13.0-15.4-17.0

8.0-10.0-12.0

9.0-9.6-10.0

2.0-3.2-5.0

20

41.0-43.75-50.0

28.0-29.8-34.0

21.0-23.2-26.0

12.0-16.2-19.0

13.0-13.4-14.0

4.0-5.6-7.0

25

50.0-50.0-50.0

37.0-39.6-44.0

28.0-29.8-33.0

17.0-22.0-26.0

17.0-18.2-20.0

6.0-7.6-9.0

30

44.0-47.4-50.0

34.0-36.4-40.0

21.0-27.4-32.0

21.0-22.0-24.0

8.0-9.2-10.0

35

50.0-50.0-50.0

41.0-42.8-47.0

26.0-32.8-38.0

24.0-26.0-28.0

10.0-11.2-12.0

40

46.0-47.8-50.0

31.0-37.8-43.0

28.0-30.0-32.0

11.0-13.0-15.0

45

50.0-50.0-50.0

35.0-41.0-50.0

31.0-33.4-36.0

13.0-15.2-17.0

50

38.0-44.0-50.0

35.0-38.0-44.0

14.0-16.6-19.0

55

43.0-43.0-50.0

38.0-41.6-48.0

16.0-18.8-22.0

60

47.0-47.0-50.0

41.0-43.25-50.0

17.0-20.2-24.0

65

44.0-46.25-50.0

19.0-22.2-26.0

70

47.0-47.0-50.0

20.0-23.8-28.0

75

50.0-50.0-50.0

22.0-25.6-30.0

80

24.0-27.4-32.0

85

26.0-29.2-33.0

90

28.0-29.8-35.0

95

29.0-32.6-37.0

100

31.0-34.0-38.0

105

32.0-35.6-40.0

110

34.0-37.8-42.0

115

35.0-39.0-43.0

120

36.0-40.6-45.0

125

38.0-42.2-46.0

130

40.0-43.8-48.0

135

41.0-45.4-49.0

140

44.0-46.0-50.0

145

45.0-46.3-50.0

150

46.0-46.0-50.0

155

47.0-47.0-50.0

160

47.0-47.5-50.0

165

48.0-48.0-50.0

170

50.0-50.0-50.0

Key: Lower Range – Mean – Upper Range

The results were drawn up after outliers had been removed. These outliers were probably caused by human error, as few other variables could have affected the experiment.

From these results we managed to work out the rate of reaction. This is our table:

Volume of CO2 (cm3)

Time (Sec)

Rate

100% HCl 0%HO

30

15

2.00cm³/s

80% HCl 20%HO

30

20

1.50cm³/s

60% HCl 40%HO

30

25

1.20cm³/s

50% HCl 50%HO

30

33

0.91cm³/s

40% HCl 60%HO

30

40

0.75cm³/s

20% HCl 80%HO

30

85

0.35cm³/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. This shows that the rate of reaction gradually increases with the surge becoming more pronounced with a greater concentration of Hydrochloric Acid. Therefore, this means that the greater concentration of Hydrochloric Acid, the higher the rate of reaction. I reach the conclusion as the 100% Hydrochloric Acid solution produced 50cm3 Carbon Dioxide almost 7 times faster than the 20% solution. This is also backed up by the rate of reaction graph, which shows that the 100% Hydrochloric Acid solution’s rate of reaction was almost 6 times greater than the 20% solution.

The conclusion I have reached is what I predicted before the experiments had taken place. I predicted that “the higher concentration of acid, the higher the rate of reaction”. This has turned out to be correct, as previously explained. I believe that concentration affected the rate of reaction in this way as explained in collision theory. Collision theory states that “Anything that increases the number of successful collisions per second will increase the rate of reaction”. Concentration increases the number of successful collisions as there are simply more particles to collide and therefore react. Concentration does not increase the number of successful reactions per second; however both temperature and the use of catalysts, two other independent variables, do increase the number of successful reactions per second. As for why the higher the concentration the quicker 50cm3 Carbon Dioxide is produced, I believe this is because Carbon Dioxide is produced in the reaction, and a higher concentration a faster rate of reaction.

Evaluation

I believe that the data we obtained from our experiments was as reliable as possible.  We made sure that our experiment was a fair test, and we repeated the experiment five times too add reliability. Of course, our results did obtain several outliers, all of which were removed from our final table, and were omitted in working out the means and ranges. The results we obtained we fairly consistent, with all of the results having a range of no more than 10cm3 Carbon Dioxide except the results for the 50% Carbon Dioxide, 50% Water solution. This result had much larger ranges than other experiments. This is probably down to human error, as there was no large difference in temperature that day. However, there could have just been some strange results, and there was no human error which affected the results.

I believe that my conclusion is somewhat limited due to the amount of results. Due to time pressures, we could only do 5 experiments per solution, meaning that the data is not as reliable as possible. I believe that 10 repetitions would be a good amount, as it would be easier to identify outliers and you would get a more accurate average. We could tell from our results that after 5 seconds, there was a real difference in the results (Excluding the 50% Carbon Dioxide, 50% Water solution) as none of the rages overlapped. Checking if the ranges overlap is commonly regarded as the best method to see if there is a real difference in the results.

Out of the three possible methods, I believe that we chose the most precise one which gave the most accurate results. Our preliminary experiments showed us that method 1 was the best possible method as we found many problems with the other methods. Method 2 had too large a scope for human error, due to the majority of the experiment relying on human judgement. Method 3 was not feasible as the scales we had available were not accurate enough for our experiment. Also, there was too little a change in mass to be able to draw a conclusion.

Whilst the equipment we used did what was required, there was one key change in equipment which could have improved the accuracy of our results. We could have used a gas syringe instead of the measuring cylinder and plastic tub. This would mean that the carbon dioxide would have gone straight into the gas syringe instead of having to travel all the way up the measuring cylinder. This would improve our results, as there is a time delay for the carbon dioxide to reach the end of the measuring cylinder. Also, a key difference is that carbon dioxide dissolves in water, meaning that not all of the carbon dioxide was measured, as some would have been lost in the water. I believe that using a measuring cylinder would have improved our results and improved the overall accuracy. That is the main difference I would have made to our method, as the majority of the method was acceptable.

I believe that my conclusion is not hindered by the accuracy of the equipment, but more by the equipment used. The measuring cylinder measured in cm3, which I found accurate enough. If it measured in mm3 than it would have added accuracy, but would probably not have changed much about the conclusion. However, using a gas syringe would have greatly improved the reliability of the results more than mm3.

Another aspect which may have limited my conclusion is the range of data I obtained. Whilst the ranges did not overlap, showing a real difference in the assorted solutions, I would have preferred to have had smaller ranges, meaning more accurate results. I believe that the easiest way to have done this would have been to have done more repetitions of the experiments, so that it would have been easier to identify outliers and make the results more accurate and reliable.

Overall, I believe that I have enough evidence to support my conclusion, however different equipment and more data would give me a more confident and precise conclusion.

This student written piece of work is one of many that can be found in our GCSE Patterns of Behaviour section.

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