Taking into account the definition of pH, the hydrogen ion concentration of the acid rain is 1.58×10⁻³ greater compared to normal rainfall.
<h3>Definition of pH</h3>
pH is a measure of acidity or alkalinity that indicates the amount of hydrogen ions present in a solution or substance.
The pH is defined as the negative base 10 logarithm of the activity of hydrogen ions, that is, the concentration of hydrogen ions or H₃O⁺:
pH= - log [H⁺]= - log [H₃O⁺]
<h3>Normal rainfall</h3>
Normal rainfall has a pH of 6.2. Replacing in the definition of pH:
6.2= - log [H⁺]
Solving:
[H⁺]= 10⁻⁶ ²
<u><em>[H⁺]= 6.31×10⁻⁷</em></u>
<h3>Acid rain</h3>
Acid rain has a pH of 2.8. Replacing in the definition of pH:
2.8= - log [H⁺]
Solving:
[H⁺]= 10⁻² ⁸
<u><em>[H⁺]= 1.58×10⁻³</em></u>
<h3>Hydrogen ion concentration difference of acid rain compared to normal rain.</h3>
To know how much greater is the hydrogen ion concentration of the acid rain compared to normal rainfall, you must do the subtraction between both concentrations:
1.58×10⁻³ - 6.31×10⁻⁷= 1.58×10⁻³
It is practically equal to the concentration of hydrogen ions in acid rain because its concentration is much higher than the concentration in normal rainfall.
In summary, the hydrogen ion concentration of the acid rain is 1.58×10⁻³ greater compared to normal rainfall.
Learn more about pH:
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