Question

Calculate the pH at of a 0.10 Msolution of anilinium chloride . Note that aniline is a weak base with a of . Round your answer to decimal place. Clears your work. Undoes your last action. Provides information about entering answers.

Answer 1

The question is incomplete, here is the complete question:

Calculate the pH at of a 0.10 M solution of anilinium chloride $(C_6H_5NH_3Cl)$ . Note that aniline $(C6H5NH2)$ is a weak base with a $pK_b$ 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:

$pH=7-\frac{1}{2}[pK_b+\log C]$

where,

$pK_b$ = 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:

$pH=7-\frac{1}{2}[4.87+\log (0.10)]\\\\pH=5.06=5.1$

Hence, the pH of the solution is 5.1

Answer 2

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