Rainwater near a coal-fired power station has a pH of 3.7. Normal rainwater has a pH of 5.5.How many times greater is the concentration of H⁺ ions in the polluted rainwater compared to normal rainwater?

Question

BlackTom AI · Accepted Answer

First, note the given pH values: polluted rainwater pH = 3.7 and normal rainwater pH = 5.5. The concentration of H+ ions is related to pH by [H+] = 10^(-pH). The ratio of hydrogen ion concentrations is 10^(-3.7) / 10^(-5.5) = 10^(5.5 - 3.7) = 10^1.8.

Now evaluate each option:

- Option a: 63. This is correct because 10^1.8 ≈ 63.1, so the polluted rainwater has about 63 times more H+ ions than normal rainwater.
- Option b: 1.8. This is the difference in pH between the two samples, not the concentration ratio. It does not represent how many times greater the H+ concentration is.
- Option c: 100. This would correspond to a pH difference of 2.0 (since 10^2 = 100), which is larger than the actual difference of 1.8.
- Option d: 180. This would imply a pH difference of roughly log10(180) ≈ 2.26, again larger than the observed 1.8 difference.
- Option e: 16. This would correspond to a pH difference of log10(16) ≈ 1.204, which is smaller than the actual 1.8 difference.

In summary, the correct interpretation is that the H+ concentration increases by a factor of 10^(5.5 − 3.7) = 10^1.8 ≈ 63, making option a the appropriate choice. The other options misinterpret either the magnitude of the pH difference or miscalculate the exponential relationship between pH and [H+].

Rainwater near a coal-fired power station has a pH of 3.7. Normal rainwater has a pH of 5.5.How many times greater is the concentration of H⁺ ions in the polluted rainwater compared to normal rainwater?

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Rainwater near a coal-fired power station has a pH of 3.7. Normal rainwater has a pH of 5.5.How many times greater is the concentration of H⁺ ions in the polluted rainwater compared to normal rainwater?

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