Acid rain has a pH value of 3.0, whereas
normal rain has a pH value of 5.6. Calculate
the ratio of the hydronium ion in acid rain to
that in normal rain.
Convert pH 3.0 to (H^+) using pH = -log(H^+).
Convert pH 5.6 to (H^+).
Divide 1st by the 2nd to find the ratio acid/normal
do I just use the moles of H+?
No, the pH needs to be converted to H^+ using the inverse log
Example:
ph = -log[H^+] = 3.0
log [H^+] = -3.0
[H^+] = inv log (3.0)
10^(-3.0)
To calculate the ratio of the hydronium ion in acid rain to that in normal rain, we first need to understand the pH scale and how it relates to the concentration of hydronium ions.
The pH scale ranges from 0 to 14, with values below 7 being acidic, values above 7 being basic, and 7 being neutral. Each unit on the pH scale represents a tenfold difference in the concentration of hydronium ions. For example, a substance with a pH of 3 has ten times the concentration of hydronium ions compared to a substance with a pH of 4.
In this case, acid rain has a pH of 3.0, whereas normal rain has a pH of 5.6.
To calculate the ratio of the hydronium ion concentration in acid rain to that in normal rain, we need to compare the difference in pH values.
First, we need to convert the given pH values into hydronium ion concentrations using the equation:
[H₃O⁺] = 10^(-pH)
For acid rain with a pH of 3.0:
[H₃O⁺] in acid rain = 10^(-3.0)
For normal rain with a pH of 5.6:
[H₃O⁺] in normal rain = 10^(-5.6)
To find the ratio, we divide the concentration in acid rain by the concentration in normal rain:
Ratio = [H₃O⁺] in acid rain / [H₃O⁺] in normal rain
Ratio = (10^(-3.0)) / (10^(-5.6))
Using the properties of exponents, we can simplify this ratio:
Ratio = (10^(5.6-3.0))
Ratio = 10^2.6
Using a calculator or mathematical software, we find that:
Ratio ≈ 398.107
Therefore, the ratio of the hydronium ion in acid rain to that in normal rain is approximately 398.107.