Respuesta :
The question is incomplete, here is the complete question:
Calculate the pH at of a 0.10 M solution of anilinium chloride [tex](C_6H_5NH_3Cl)[/tex] . Note that aniline [tex](C6H5NH2)[/tex] is a weak base with a [tex]pK_b[/tex] of 4.87. Round your answer to 1 decimal place.
Answer: The pH of the solution is 5.1
Explanation:
Anilinium chloride is the salt formed by the combination of a weak base (aniline) and a strong acid (HCl).
To calculate the pH of the solution, we use the equation:
[tex]pH=7-\frac{1}{2}[pK_b+\log C][/tex]
where,
[tex]pK_b[/tex] = negative logarithm of weak base which is aniline = 4.87
C = concentration of the salt = 0.10 M
Putting values in above equation, we get:
[tex]pH=7-\frac{1}{2}[4.87+\log (0.10)]\\\\pH=5.06=5.1[/tex]
Hence, the pH of the solution is 5.1
The pH of the solution is 5.1.
Calculation of the ph of the solution:
Anilinium chloride refers to the salt that should be created by the combination of a weak base (aniline) and a strong acid (HCl).
here the following equation should be used.
ph = 7-1/2(pkb+ logc)
here pkb = negative logarithm of the weak base i.e. aniline = 4.87
And, C = concentration of the salt = 0.10 M
Now the ph should be
= 7-1/2(4.87 + log(0.10))
= 5.1
Hence, The pH of the solution is 5.1.
Learn more about weak base here: https://brainly.com/question/23147566
