Hello!
We have the following data:
[acid] = 0.0500 M (mol/L)
[base] = 0.0367 M (mol/L)
pH of a buffer =?
knowing that pKa (acetic acid) = 4.74
Now, using the abovementioned data for the pH formula of a buffer solution or (Henderson-Hasselbalch equation), we have:
[tex] pH = pKa + log\:\dfrac{[base]}{[acid]} [/tex]
[tex] pH = 4.74 + log\:\dfrac{0.0367}{0.0500} [/tex]
[tex] pH = 4.74+ log\:0.734 [/tex]
[tex] pH = 4.74 + (-0.13) [/tex]
[tex] pH = 4.74 - 0.13 [/tex]
[tex] \boxed{\boxed{pH = 4.61}}\end{array}}\qquad\checkmark [/tex]
Note:. The pH <7, then we have an acidic solution.
I Hope this helps, greetings ... DexteR! =)
The pH of the solution ( Buffer ) is approximately 4.60
Given data:
Temperature = 25°C ( room temperature )
pKa = 4.74
Acid concentration = 0.0500 M
Base concentration = 0.0367 M
Calculate the value of the pH of the Buffer solution
pH = pka + log ( base / acid ) --- ( 1 )
∴ pH of the solution = 4.74 + log ( 0.0367 / 0.0500 )
= 4.74 + ( -0.1343 )
= 4.60.
Hence we can conclude that The pH of the solution ( Buffer ) approximately = 4.60
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