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# Lakes that have been acidified by acid rain (see Chemistry ## Problem 116P Chapter 14

Introductory Chemistry | 5th Edition

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Problem 116P

Lakes that have been acidified by acid rain (see Chemistry in the Environment box in Section 5.9) 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?

Step-by-Step Solution:

Solution 116 P:

Here, we are going to calculate the amount of limestone required  to completely neutralize a 3.8 × 109 L lake with a pH of 5.5.

Step 1:

pH = 5.5

Concentration of H+ is

pH =-log[H+]

[H+] = 10-pH = 10 -5.5 = 3.16 x 10-6 mol/L

Step 2:

The moles of  H+ is = 3.8 × 109 L x 3.16 x 10-6 mol/ 1.0 L

= 12.0 x 103 mol

Step 3 of 3

##### ISBN: 9780321910295

This full solution covers the following key subjects: limestone, lake, addition, been, box. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. The full step-by-step solution to problem: 116P from chapter: 14 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. Since the solution to 116P from 14 chapter was answered, more than 248 students have viewed the full step-by-step answer. The answer to “Lakes that have been acidified by acid rain (see Chemistry in the Environment box in Section 5.9) 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?” is broken down into a number of easy to follow steps, and 48 words. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5.

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