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xz_007 [3.2K]
3 years ago
10

Increased industrialization has caused a rise in harmful acid rain precipitation that affects plant and marine life. A sample of

acid rain has a proton concentration 10,000 times greater than pure water and more than 100,000 times greater than seawater. What is the approximate pH of this sample?
Chemistry
1 answer:
wolverine [178]3 years ago
3 0

Answer:

pH of the sample of acid rain is 3.

Explanation:

Pure water has a theoretical pH of 7.00. As pH = -log [H⁺], [H⁺] = 1x10⁻⁷M

Now, the sample of acid rain has a proton concentration 10,000 times greater than pure water. That is:

[H⁺] = 10,000 * 1x10⁻⁷M = 1x10⁻³M

The pH of this sample is:

pH = -log 1x10⁻³M

<h3>pH = 3</h3>
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lutik1710 [3]
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A chemist adds of a M zinc nitrate solution to a reaction flask. Calculate the mass in grams of zinc nitrate the chemist has add
weqwewe [10]

corrected question: A chemist adds 135mL of a 0.21M zinc nitrate solution to a reaction flask. Calculate the mass in grams of zinc nitrate the chemist has added to the flask. Round your answer to significant digits.

Answer:

5.37g

Explanation:

0.21M means ; 0.21mol/dm³

1dm³=1L , so we can say 0.21mol/L

if 0.21mol of Zinc nitrate is contained in 1L of water

x   will be contained in 135mL of water

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=0.02835moles

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Read 2 more answers
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