Question

The ph of a solution containing 0.818 M acetic acid

(ka1.76*10-5) ans 0.172 M sodium acetate is?

Answer 1

Step-by-step explanation:

It is known that the relation between pH and
`pK_(a)` is as follows.

pH =
`pK_(a) + log ([salt])/([acid])`

and,
`pK_(a) = -log K_(a)`

Hence, first we will calculate the value of
`pK_(a)` as follows.

`pK_(a) = -log K_(a)`

=
`-log (1.76 * 10^(-5)`

= 4.75

Now, we will calculate the value of pH as follows.

pH =
`pK_(a) + log \frac{[\text{sodium acetate}]}{\text{acetic acid}}`

=
`4.75 + log (0.172)/(0.818)`

= 4.75 + (-0.677)

= 4.07

Therefore, we can conclude that the pH of given solution is 4.07.