What do you expect if an acid falls on the aluminium piece . write a balanced chemical equation for it
Answers
Answer:
Hydrogen gas is being produced.
Explanation:
Natural Acidity of Rainwater
Pure water has a pH of 7.0 (neutral); however, natural, unpolluted rainwater actually has a pH of about 5.6 (acidic).[Recall from Experiment 1 that pH is a measure of the hydrogen ion (H+) concentration.] The acidity of rainwater comes from the natural presence of three substances (CO2, NO, and SO2) found in the troposphere (the lowest layer of the atmosphere). As is seen in Table I, carbon dioxide (CO2) is present in the greatest concentration and therefore contributes the most to the natural acidity of rainwater.
Gas
Natural Sources
Concentration
Carbon dioxide
CO2 Decomposition 355 ppm
Nitric oxide
NO Electric discharge 0.01 ppm
Sulfur dioxide
SO2 Volcanic gases 0-0.01 ppm
Table 1
Carbon dioxide, produced in the decomposition of organic material, is the primary source of acidity in unpolluted rainwater.
NOTE: Parts per million (ppm) is a common concentration measure used in environmental chemistry. The formula for ppm is given by:
Carbon dioxide reacts with water to form carbonic acid (Equation 1). Carbonic acid then dissociates to give the hydrogen ion (H+) and the hydrogen carbonate ion (HCO3-) (Equation 2). The ability of H2CO3 to deliver H+ is what classifies this molecule as an acid, thus lowering the pH of a solution.
(1)
(2)
Nitric oxide (NO), which also contributes to the natural acidity of rainwater, is formed during lightning storms by the reaction of nitrogen and oxygen, two common atmospheric gases (Equation 3). In air, NO is oxidized to nitrogen dioxide (NO2) (Equation 4), which in turn reacts with water to give nitric acid (HNO3) (Equation 5). This acid dissociates in water to yield hydrogen ions and nitrate ions (NO3-) in a reaction analagous to the dissociation of carbonic acid shown in Equation 2, again lowering the pH of the solution.
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