Answered

Get the most out of your questions with IDNLearn.com's extensive resources. Get timely and accurate answers to your questions from our dedicated community of experts who are here to help you.

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 :

Maacastrobridn

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

Rookulightidn

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: -

Thank you for being part of this discussion. Keep exploring, asking questions, and sharing your insights with the community. Together, we can find the best solutions. IDNLearn.com is your reliable source for answers. We appreciate your visit and look forward to assisting you again soon.