Aspirin (acetylsalicylic acid, C9H8O4) is a weak monoprotic acid. To determine its acid-dissociation constant, a student dissolved 2.00 g of aspirin in 0.600 L of water and measured the pH.

What was the Ka value calculated by the student if thepH of the solution was 2.62?

A 0.100 M solution of ethylamine (C2H5NH2) has a pH of 11.87.

Calculate the Kb for ethylamine.

1. was the value calculated by the student.

2. was the of ethylamine value calculated by the student.

Explanation:

1.

The value of Aspirin solution = 2.62

Moles of s asprin =

Volume of the solution = 0.600 L

The initial concentration of Aspirin  = c =

initially

c       0    0

At equilibrium

(c-x)      x   x

The expression of dissociation constant :

:

was the value calculated by the student.

2.

The value of ethylamine = 11.87

The initial concentration of ethylamine = c = 0.100 M

initially

c                    0    0

At equilibrium

(c-x)                x   x

The expression of dissociation constant :

:

was the of ethylamine value calculated by the student.

idk

explanation: