Answer:
Recycled Ammonia
Explanation:
Ammonia can be extracted from livestock wastewater and used as a fertilizer. There are systems available that extract the ammonia and mix it with acids to create ammonium citrate or ammonium nitrate, both of which can be used as fertilizers. The extraction system removes ammonia from the waste, which significantly reduces the amount of ammonia that is released into the air. This has the added bonus of improving the air quality where animals are kept.
Algae living on a sloth is considered an example of mutualism because both of them benefit from each other.
Mutualism is one of the symbiotic relationships in which both the two species living together benefit in one way or another. A considerable example of such a relationship is between algae and a sloth.
The algae provide camouflage to the sloth and protect it from predators while the sloth provides shelter to the algae for its growth. The sloth also gets nutrition from algae which perform photosynthesis and synthesize food.
Another mutual relationship is observed between the aphids and ants. Aphids produce honeydew as a waste product of their diet which is consumed by ants. While ants protect the aphids from predators and parasites.
To know more about mutualism, refer to the following link:
brainly.com/question/94753
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Answer:The ratio of the concentrations of 
and 
when the buffer has a pH of 7.02 is 0.69
Explanation:
The dissociation constant for formic acid = 
Concentration of HA= 0.5 mM
Concentration of = 0.1 mM
pH = 6.16
First we have to calculate the value of 
.
Using Henderson Hesselbach equation :
![pH=pK_a+\log \frac{[A^-}{[HA]}](https://tex.z-dn.net/?f=pH%3DpK_a%2B%5Clog%20%5Cfrac%7B%5BA%5E-%7D%7B%5BHA%5D%7D)
Now put all the given values in this expression, we get:
![6.16=pK_a+\log (\frac{[0.1]}{0.5})](https://tex.z-dn.net/?f=6.16%3DpK_a%2B%5Clog%20%28%5Cfrac%7B%5B0.1%5D%7D%7B0.5%7D%29)
To calculate the ratio of the concentrations of and when the buffer has a pH of 7.02.
Using Henderson Hesselbach equation :
![7.02=6.86+\log \frac{[A^-]}{[HA]}](https://tex.z-dn.net/?f=7.02%3D6.86%2B%5Clog%20%5Cfrac%7B%5BA%5E-%5D%7D%7B%5BHA%5D%7D)
![\frac{[A^-]}{[HA]}=1.44](https://tex.z-dn.net/?f=%5Cfrac%7B%5BA%5E-%5D%7D%7B%5BHA%5D%7D%3D1.44)
![\frac{[HA]}{[A^-]}=0.69](https://tex.z-dn.net/?f=%5Cfrac%7B%5BHA%5D%7D%7B%5BA%5E-%5D%7D%3D0.69)
Thus the ratio of the concentrations of and when the buffer has a pH of 7.02 is 0.69
Covalent bonds is the correct answer
