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.
This intrigued my interest and I started to wonder about the effects of acidic deposition on the environment and health, but what intrigued me the most was the influence of acid rain on buildings and the sculptures that we see in our daily lives.
- The origin of sulfuric acid.
- Collision theory
- Acid deposition
- Effects of acid deposition
3.6 Risk assessment
- Sulfuric acid:
- Calcium carbonate
- Safety consideration:
- Ethical and environmental concerns:
4. Data collection
4.1 qualitative observations
- Before the reaction:
- During the reaction:
- At the end of the reaction:
4.2 Quantitative data
4.3 processed data
- Percentage uncertainty for trial one :
- Percentage uncertainty for trial two
- Percentage uncertainty for trial three
In these experiments, different concentrations of sulfuric acid solutions were mixed with a fixed mass of calcium carbonate
and each reaction was filmed for five minutes in order to see how the mass decreases over time and to later be able to calculate the rate of reaction. The concentration values that were chosen for the sulfuric acid solutions were in increasing
order (0.0625, 0.125, 0.25, 0.5,1)mol dm−3
concentration affects the rate of mass loss. The reaction formed. for the purpose of observing how increasing the
H2SO4 (aq)+ CaCO3 (s)→ CaSO4 + CO2 (g)+ H2O(l). The experiment used 5 different concentrations of sulfuric acid (0.0625, 0.125, 0.25, 0.5,1) mol dm−3