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Anika [276]
3 years ago
15

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\bold{ \sf{what \: is \:nitrogen \: fixation }}
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Chemistry
2 answers:
Brums [2.3K]3 years ago
8 0

Nitrogen fixation is the incorporation of atmospheric nitrogen into ammonia by various bacteria, catalyzed by nitrogenase.This is an essential stage in the nitrogen cycle and is the ultimate source of all nitrogen in living organisms. Nitrogen cycle: atmospheric nitrogen is inert and cannot be used by living forms

<h3>Hope This Helps You ❤️</h3>
azamat3 years ago
6 0

Answer:

Nitrogen fixation is a chemical process by which molecular nitrogen in the air is converted into ammonia or related nitrogenous compounds in soil or aquatic systems. Atmospheric nitrogen is molecular dinitrogen, a relatively nonreactive molecule that is metabolically useless to all but a few microorganisms.

Explanation:

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A 0. 462 g sample of a monoprotic acid is dissolved in water and titrated with 0. 180 m koh. what is the molar mass of the acid
Len [333]

The molar mass of the acid if 28. 5 ml of the koh solution is required to neutralize the sample is 90.23g/mol.

<h3>For the calculation of molarity of solution</h3>

Molarity = (moles of solute/volume of solution) × 1000

Given,

Molarity of KOH solution = 0.180 M

Volume of solution = 28.5 mL

0.180 = (moles of KOH/ 28.5) × 1000

Moles = (0.18× 28.5)/1000

= 0.00513 mol

<h3>Chemical equation for the reaction</h3>

HA + KOH ------- KA + H2O

1 moles of KOH reacts with 1 moles of HA.

So, 0.00513 moles of KOH react with 0.00513 moles of HA.

<h3>To calculate the molar mass for given number of moles</h3>

Number of moles= given mass/ Molar mass

Given,

Mass of HA = 0.462 g

Moles of HA = 0.00512 mol

0.00512 = 0.462/ Molar mass

Molar mass = 90.23 g/ mol.

Thus the molar mass of HA required to neutralize the 28.5 mL of KOH is 90.23g/mol.

learn more about molar mass or moles:

brainly.com/question/26416088

#SPJ4

3 0
1 year ago
A chemist dissolves 697. mg of pure potassium hydroxide in enough water to make up 160. mL of solution. Calculate the pH of the
umka21 [38]

<u>Answer:</u> The pH of the solution is 12.9

<u>Explanation:</u>

To calculate the molarity of solution, we use the equation:

\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}

Given mass of KOH = 697 mg = 0.697 g    (Conversion factor:  1 g = 1000 mg)

Molar mass of KOH = 56 g/mol

Volume of solution = 160 mL

Putting values in above equation, we get:

\text{Molarity of KOH solution}=\frac{0.697\times 1000}{56\times 160}\\\\\text{Molarity of KOH solution}=0.0778M

1 mole of KOH produces 1 mole of K^+ ions and 1 mole of OH^- ions

To calculate the pOH of the solution, we use the equation:

pOH=-\log[OH^-]

We are given:

[OH^-]=0.0778M

Putting values in above equation, we get:

pOH=-\log (0.0778)=1.11

To calculate pH of the solution, we use the equation:

pH+pOH=14\\pH=14-1.11=12.89

Hence, the pH of the solution is 12.9

5 0
3 years ago
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