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126. Lakes that have been acidified by acid rain can be neutralized by liming, the addition of limestone (CaCO3 ). How much limestone in kilograms is required to completely neutralize a 3.8 * 109 L lake with a pH of 5.5?

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26 Oct 2019
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Related questions

10. An 8000 m3 lake has a pH of 4. For this problem, assume no water is added or withdrawn from the lake.

a. What is the molarity of H+ in the lake?

b. How many moles of OH- would be needed to raise the pH of the lake to 6?

c. One method for neutralizing acids in surface water is to add lime (CaCO3). Write a balanced equation for the

neutralization of H+ with limestone. (Hint: see problem 7)

d. If this OH- all comes from limestone, how many kg of limestone will be needed? Assume that all of the

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2. Natural lakes employ the natural bicarbonate/carbonic-acid buffer to help maintain optimal pH levels. (The carbonic acid of the buffer is a result of the Lewis acid-base reaction between dissolved carbon dioxide and the lake water, and the bicarbonate of the buffer is a result of the Brønsted-Lowry acid-base reaction between the carbonic acid and the lake water.) Acid rain (pH < 5.00) falling into such lakes would, therefore, be neutralized by....

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