Reaction between calcium carbonate and hydrochloric acid
the reaction between calcium carbonate and hydrochloric acid
AIM- My task is to investigate the reaction between calcium carbonate and hydrochloric acid, which produces calcium chloride, carbon dioxide, and water. To do this I will conduct an experiment.
Word Equation:
Calcium + Hydrochloric Calcium + Carbon Dioxide + Water
Carbonate Acid Chloride
Chemical Equation:
CaCo3 (s) + 2Hcl (aq) CaCl2 + Co2 (g) + H20 (l)
The key variables in this experiment that affect the rate of reaction is, surface area, temperature, mass of CaCo3 and concentration of acid.
The surface area can be investigated by increasing or decreasing the surface area of the calcium carbonate (marble) chips (i.e. have them as chips or powdered). The temperature can be investigated by increasing the temperature of water in the water trough. Increasing or decreasing the mass of the calcium carbonate chips used in the experiment can investigate the mass. The concentration can be investigated by increasing or decreasing the concentration of acid put on the marble chips.
The variable I will be changing in order to conduct my experiment is the concentration of acid as this will have an effect on how much Carbon Dioxide is produced.
There are a number of ways in which this experiment can be conducted. Firstly, the volume of Carbon Dioxide produced can be measured at regular intervals- using a gas syringe or a measuring cylinder. The second way is to measure the loss in mass of the container, calcium carbonate, and hydrochloric acid at intervals.
I will be conducting this experiment, by using a measuring cylinder, to measure the volume of Carbon Dioxide produced at regular intervals of one minute until ten minutes have passed. I will be doing it this way, as this is the way I did it in my preliminary experiment and it produced accurate results.
This is how I will conduct the experiment. I will set up the apparatus as shown below. I will pour in the Hydrochloric acid and get someone else to start the stopwatch for me, next I will measure the volume of Co2 produced ...
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I will be conducting this experiment, by using a measuring cylinder, to measure the volume of Carbon Dioxide produced at regular intervals of one minute until ten minutes have passed. I will be doing it this way, as this is the way I did it in my preliminary experiment and it produced accurate results.
This is how I will conduct the experiment. I will set up the apparatus as shown below. I will pour in the Hydrochloric acid and get someone else to start the stopwatch for me, next I will measure the volume of Co2 produced at intervals of one minute until ten minutes have passed. I will do it for ten minutes as when I did my preliminary experiment, all the reaction had stopped completely within ten minutes.
Therefore, I think the initial rate will be ten minutes. I will do four different experiments, using four different concentrations of acid. I will be starting with 0.5 molar acid. This is because, I thought 0.5 molar would produce a sufficient enough reaction and the difference can be seen quite clearly. In the next experiment I will use 1 molar acid. As you can tell that is a difference of 0.5 molar. I will work up in a difference of 0.5 molar until 2 molar. I decided to stop at 2 molar, as I think I will be able to see quite clearly up to then whether the concentration of acid has an effect on the volume of Carbon Dioxide produced I will be using 30ml of Hydrochloric acid as when I did my preliminary experiment, it was enough to cover the marble chips. I will be doing each of the four experiments, three times. I will do them three times each as that will mean I can have an average, which will mean more accurate results and any minor problems won't be noticed as well.
DIAGRAM-
The apparatus I will be using to conduct this experiment are:
00ml measuring cylinder,
Water trough,
Hydrochloric acid, (0.5M, 1M, 1.5M, 2M)
Calcium Carbonate Chips,
Side-arm flask,
Thermometer,
Top-pan-balance,
Stop-watch &
Water.
I will make sure this experiment is fair, by always using the same amount/mass of marble chips, making sure the same volume of water is used every time in the water trough, and making sure the water in the water trough is at a constant temperature. I will also make sure the same volume of acid is used. The only factor, I will be changing is the concentration of hydrochloric acid.
I will make sure this experiment is safe, by always wearing goggles as acid is being used and there will be a chemical reaction. Also I will make sure, that if any acid is spilled, it should be cleared away quickly. If it gets on my hands or clothes, I will wash them thoroughly to avoid burning myself. If it spills on the desk, I will inform the teacher and clean it without getting it on my hands or clothes.
The measuring cylinder I will use to measure the volume of Co2 produced will be 100ml because I will be able to measure quite accurately.
The mass of the calcium carbonate chips I will be using is 10g.
The volume of acid I will use is 30ml.
This is the table I propose to record my results in:
Volume of
Acid
Concentration
Of Acid
Time/
Minutes
Mass of
Marble chips
Volume of Co2 produced
Temp of H20
HYPOTHESIS- I think that as the concentration of acid increases the volume of Co2 produced will also increase. I think this is because as the acid becomes more concentrated it will be easier for the calcium carbonate (marble) chips to react (come into contact) with the acid particles and therefore will produce more Carbon Dioxide. For example, what it says in this book I used as a secondary source, ' If the acid is at low concentrations, the acid particles, will be widely spread in the water, and the number of collisions between them and the marble chips will be limited. At higher concentrations, however, the chances of a collisions between the acid particles and the marble chips are greatly increased.' (Heinemann, Higher Chemistry) That is why I feel, that as the concentration of acid increases, the volume of Carbon Dioxide produced will also increase.
RESULTS-
Concentration
Of acid
Time/
Minutes
First
Results
Second
Results
Third
Results
Average
(3sf)
0.5 Molar
65.0 ml
50.0 ml
60.0 ml
58.3 ml
0.5 Molar
2
20 ml
80.0 ml
90.0 ml
96.7 ml
0.5 Molar
3
30 ml
00 ml
10 ml
13.3 ml
0.5 Molar
4
35 ml
20 ml
20 ml
25 ml
0.5 Molar
5
40 ml
30 ml
30 ml
33 ml
0.5 Molar
6
42 ml
35 ml
35 ml
37 ml
0.5 Molar
7
43 ml
40 ml
38 ml
40 ml
0.5 Molar
8
45 ml
42 ml
40 ml
42 ml
0.5 Molar
9
45 ml
45 ml
41 ml
44 ml
0.5 Molar
0
45 ml
45 ml
41 ml
44 ml
Concentration
Of acid
Time/
Minutes
First
Results
Second
Results
Third
Results
Average
(3sf)
Molar
65 ml
65 ml
60 ml
63 ml
Molar
2
200 ml
220 ml
220 ml
213 ml
Molar
3
220 ml
248 ml
245 ml
238 ml
Molar
4
228 ml
255 ml
255 ml
246 ml
Molar
5
229 ml
258 ml
259 ml
249 ml
Molar
6
230 ml
258 ml
260 ml
249 ml
Molar
7
230 ml
258 ml
260 ml
249 ml
Molar
8
230 ml
258 ml
260 ml
249 ml
Molar
9
230 ml
258 ml
260 ml
249 ml
Molar
0
230 ml
258 ml
260 ml
249 ml
Concentration
Of acid
Time/
Minutes
First
Results
Second
Results
Third
Results
Average
(3sf)
.5 Molar
210 ml
50 ml
200 ml
87 ml
.5 Molar
2
295 ml
200ml
280 ml
258 ml
.5 Molar
3
330 ml
210 ml
305 ml
282 ml
.5 Molar
4
342 ml
215 ml
312 ml
290 ml
.5 Molar
5
350 ml
216 ml
315 ml
294 ml
.5 Molar
6
351 ml
217 ml
317 ml
295 ml
.5 Molar
7
352 ml
217 ml
317 ml
295 ml
.5 Molar
8
352 ml
217 ml
317 ml
295 ml
.5 Molar
9
352 ml
217 ml
317 ml
295 ml
.5 Molar
0
352 ml
217 ml
317 ml
295 ml
Concentration
Of acid
Time/
Minutes
First
Results
Second
Results
Third
Results
Average
(3sf)
2 Molar
300 ml
335 ml
300 ml
312 ml
2 Molar
2
335 ml
365 ml
325 ml
342 ml
2 Molar
3
395 ml
400 ml
375 ml
390 ml
2 Molar
4
415 ml
419 ml
395 ml
410 ml
2 Molar
5
426 ml
429 ml
400 ml
418 ml
2 Molar
6
432 ml
435 ml
405 ml
424 ml
2 Molar
7
434 ml
439 ml
406 ml
426 ml
2 Molar
8
435 ml
439 ml
406 ml
427 ml
2 Molar
9
436 ml
439 ml
406 ml
427 ml
2 Molar
0
436 ml
439 ml
406 ml
427 ml
