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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?

Sagot :

maacastrobr

Answer:

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⁺] = [tex]10^{-pH}[/tex]

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

  • pH = 7 ⇒ [H⁺] = [tex]10^{-7}[/tex] = 1.0x10⁻⁷ M
  • pH = 5.6 ⇒ [H⁺] = [tex]10^{-5.6}[/tex] = 2.5x10⁻⁶ M
  • pH = 3.7 ⇒ [H⁺] = [tex]10^{-3.7}[/tex] = 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

Rookulight

Answer:

1. 7 (a neutral solution)

Answer: 10-7= 0.0000001 moles per liter

2. 5.6 (unpolluted rainwater)

Answer: 10-5.6 = 0.0000025 moles per liter

3. 3.7 (first acid rain sample in North America)

Answer: 10-3.7 = 0.00020 moles per liter

The concentration of H+ in the Hubbard Brook sample is 0.00020/0.0000025, which is 80 times higher than the H+ concentration in unpolluted rainwater.

Explanation: -

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