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# Solved: Lakes that have been acidified by acid rain (see ISBN: 9780321910295 34

## Solution for problem 118P Chapter 14

Introductory Chemistry | 5th Edition

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Problem 118P

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:
Step 1 of 3

Solution: Here, we are going to calculate the mass of limestone required to completely neutralize the lake.

Step1:

pH is the negative logarithm to base 10 of hydrogen ion concentration.

pH = - log[H+ ]

Step2:

Given, pH of the Lake = 5.5

pH =  - log[H+]

Therefore, [H+] = 10-pH

= 10-5.5

= 3.16 x 10-6 M

Therefore, number of moles of hydrogen ion = Volume of the lake x [H+]

= (3.8 x 109 L) x (3.16 x 10-6 mol/L)

= 12.0 x 103 mol

Step3:

The neutralization reaction taking place in the lake is:

CaCO3(s) +...

Step 2 of 3

Step 3 of 3

##### ISBN: 9780321910295

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. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. Since the solution to 118P from 14 chapter was answered, more than 288 students have viewed the full step-by-step answer. Introductory Chemistry was written by and is associated to the 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: 118P from chapter: 14 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM.

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