What is the effect of changing the concentration of sulfuric acid (0.0625, 0.125, 0.25, 0.5,1) mol dm−3 on the rate of reaction with 0.1g calcium carbonate, calculated by measuring the mass loss per unit time?
The idea behind this investigation began when we were learning about the acidic nature of rainwater which was due to the dissolved carbon dioxide in the atmosphere, pure rainwater is naturally acidic with a pH of 5,6.
Rainwater is associated with acid rain which is one of the most important environmental issues that is caused as a result of air pollution, all rainwater is considered to be slightly acidic because it contains some dissolved carbon dioxide.
The oxides of sulfur and nitrogen are the major sources of atmospheric acidity, these oxides are the products of combustion reactions and are both converted to strong acids in the atmosphere.
When I once traveled to London, I used to hear people refer to London as the city of fog, so I started questioning the reason behind this and it turned out that London was given that nickname because of the huge quantities of air pollutants which were produced by its factories.
- The origin of sulfuric acid.
- Collision theory
- Acid deposition
- Effects of acid deposition
4. . Data collection
1. Five different solutions of sulfuric acid (0.0625, 0.125, 0.25, 0.5,1)mol dm−3 were prepared by the supervisor.
2. A fixed mass of 0.1 grams of calcium carbonate ± 0.0001g was put in a wash glass using a spoon and was measured using an electronic scale.
3. The 0.1 grams of calcium carbonate ± 0.0001g was placed in a 250 cm3 beaker.
4. A 50ml measuring cylinder ±0.5 cm3 was filled with 50ml of 1mol sulfuric acid±0.1 cm3 .
5. The 50 ml of 1 mol dm−3 sulfuric acid was added to the 250 cm3 beaker containing the 0.1 grams of calcium carbonate
6.A stopwatch started to record time as soon as the 50ml of sulfuric acid ±0.1 cm3 was completely poured into the 250 cm3 beaker containing the calcium carbonate.
7. The mass value of the beaker containing calcium carbonate± 0.0001g and sulfuric acid±0.1 cm3 was taken every 30 seconds for 5 minutes.
8. The reaction was filmed from the beginning to the end and the video filmed was used to extract the values that were displayed on the electronic scale.