Question

Because it dissolves carbon dioxide from the atmosphere to make mild carbonic acid, natural rain has a pH of around 5.5. However, due to pollutants such as sulfates from coal-fired power plants and nitrates from car exhausts, the pH of rain can drop to as low as 2. This decrease in pH represents a change in H+ concentration by approximately what factor?

A. 3000
B. 300
C. 3.5
D. 35

Answer 1

The pH of normal rain is around 5.6 but can drop to as low as 2 due to pollutants. To determine the change in H+ concentration, we compare the difference in pH values using antilogarithm. The change in H+ concentration is approximately a factor of 4000.

Step-by-step explanation:

The pH of normal rain is around 5.6 due to the presence of dissolved carbon dioxide, which forms carbonic acid. However, due to pollutants like sulfates from coal-fired power plants and nitrates from car exhausts, the pH of rain can drop to as low as 2. To determine the change in H+ concentration, we need to compare the difference in pH values.

The change in pH is calculated by taking the antilogarithm of the difference in pH values. In this case, the change in pH is 5.6 - 2 = 3.6. Taking the antilogarithm of 3.6 gives us a factor of approximately 4000.

Therefore, the correct answer is A. 3000.