Use a scientific calculator to calculate [H+] for the following pH values: 7 (a neutral solution)

5.6 (unpolluted rainwater)

3.7 (first acid rain sample in North America)

How many times higher is the concentration of H+ in the Hubbard Brook sample than in unpolluted rainwater?

pH = 7 ⇒ [H⁺] = 1.0x10⁻⁷ M

pH = 5.6 ⇒ [H⁺] = 2.5x10⁻⁶ M

pH = 3.7 ⇒ [H⁺] = 2.0x10⁻⁴ M

H⁺ concentration in the Hubbard Brook sample is 80 times higher than in unpolluted rainwater.

Explanation:

To answer this problem we need to keep in mind the definition of pH:

pH = -log[H⁺]

Meaning that after isolating [H⁺] we're left with:

[H⁺] =

Now we proceed to calculate [H⁺] for the given pHs:

pH = 7 ⇒ [H⁺] = = 1.0x10⁻⁷ MpH = 5.6 ⇒ [H⁺] = = 2.5x10⁻⁶ MpH = 3.7 ⇒ [H⁺] = = 2.0x10⁻⁴ M

Finally we calculate how many times higher is [H⁺] when pH = 3.7 than when pH = 5.6.

2.0x10⁻⁴ / 2.5x10⁻⁶ = 80

Because electrons have negligible mass, to account for the mass of the isotope, there must be 16 neutrons, 16 neutrally charged, massive, fundamental particles present in the sulfur nucleus. and thus finally, if we have the 32s2− ion, there are 18 electrons, 16 protons, and 16 neutrons.

Rethink and reinvent