Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Chemistry
Acid-base chemistry involves the study of acids, bases, and their reactions. Acids donate protons (H+) in solution, while bases accept protons. The pH scale measures the acidity or basicity of a solution, with lower pH values indicating higher acidity. Understanding these principles is crucial for analyzing the behavior of carbonic acid in rainwater and its impact on the environment.
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Carbonic Acid Equilibrium
Carbonic acid (H2CO3) is a weak acid that exists in equilibrium with bicarbonate (HCO3-) and carbonate ions (CO32-). The equilibrium can be represented by the following reactions: H2CO3 ⇌ HCO3- + H+ and HCO3- ⇌ CO32- + H+. The pH of the solution influences the distribution of these species, making it essential to understand this equilibrium when calculating their concentrations in acidic rainwater.
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Concentration Calculations
Concentration calculations involve determining the amount of a substance in a given volume of solution, typically expressed in molarity (M). In this context, the total concentration of carbonic acid, bicarbonate, and carbonate ions is given as 1.0 * 10-5 M. Using the pH to find the concentration of H+ ions allows for the application of equilibrium expressions to calculate the individual concentrations of the species present in the raindrop.
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