<u>Answer:</u> The pH of the buffer is 5.25
<u>Explanation:</u>
Let the volume of buffer solution be V
We know that:
To calculate the pH of acidic buffer, we use the equation given by Henderson Hasselbalch:
![pH=pK_a+\log(\frac{[\text{conjugate base}]}{[acid]})](https://tex.z-dn.net/?f=pH%3DpK_a%2B%5Clog%28%5Cfrac%7B%5B%5Ctext%7Bconjugate%20base%7D%5D%7D%7B%5Bacid%5D%7D%29)
We are given:
= negative logarithm of acid dissociation constant of weak acid = 4.90
![[\text{conjugate base}]=\frac{2.25}{V}](https://tex.z-dn.net/?f=%5B%5Ctext%7Bconjugate%20base%7D%5D%3D%5Cfrac%7B2.25%7D%7BV%7D)
![[acid]=\frac{1.00}{V}](https://tex.z-dn.net/?f=%5Bacid%5D%3D%5Cfrac%7B1.00%7D%7BV%7D)
pH = ?
Putting values in above equation, we get:
Hence, the pH of the buffer is 5.25
Answer:
Nitrogen fixation is the conversion of gaseous nitrogen into an organism friendly form (ammonia) .
Explanation:
Nitrogen fixation -
It is very important and necessary process by which the nitrogen gas present in the atmosphere gets converted to nitrogen derivatives like ammonia in the soil , is referred to as the process of nitrogen fixation.
This occurs due to the reason , that the derivatives of nitrogen are of much more importance than the molecular nitrogen.
Biologically the process is done by the rhizobium bacteria .
Hence ,
From the question,
The correct option is a.
Answer:
1.39 atm
Explanation:
First find combined gas law equation. Then rearrange variable to match problem. You should get...
P2 = P1T2/T1
Next, change celcius temperatures to kelvin. Do this by adding 273 K (standard STP). Then fill in the numbers to go along with equation. You should get...
P2 = 1.22 atm x 455 K / 398 K = 1.39 atm
- If you need further explanation or more help please let me know. I would be glad to offer more of an explanation or help on other problems.
