__C + __H2O → __CO + H2
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<u>Answer:</u> The pH change of the buffer is 0.30
<u>Explanation:</u>
To calculate the pH of basic buffer, we use the equation given by Henderson Hasselbalch:
.....(1)
We are given:
= negative logarithm of base dissociation constant of aniline = 9.13
pOH = ?
Putting values in equation 1, we get:
To calculate pH of the solution, we use the equation:
To calculate the molarity, we use the equation:
Moles hydrochloric acid solution = 0.124 mol
Volume of solution = 1 L
Putting values in above equation, we get:
The chemical reaction for aniline and HCl follows the equation:
<u>Initial:</u> 0.418 0.124 0.306
<u>Final:</u> 0.294 - 0.430
Calculating the pOH by using using equation 1:
= negative logarithm of base dissociation constant of aniline = 9.13
pOH = ?
Putting values in equation 1, we get:
To calculate pH of the solution, we use the equation:
Calculating the pH change of the solution:
Hence, the pH change of the buffer is 0.30