Answer:
The concentration of
is 1.48 ×
M
The absolute uncertainty of
is ±0.12 ×
M
The concentration of
is written as 1.48(±0.12) ×
M
Explanation:
The pH of a solution is given by the formula below
pH = ![-log_{10}[{H^{+}]](https://tex.z-dn.net/?f=-log_%7B10%7D%5B%7BH%5E%7B%2B%7D%5D)
∴ ![[H^{+}] = 10^{-pH}](https://tex.z-dn.net/?f=%5BH%5E%7B%2B%7D%5D%20%3D%2010%5E%7B-pH%7D)
where
is the
concentration
From the question,
pH = 8.83±0.04
That is,
pH =8.83 and the uncertainty is ±0.04
First, we will determine
from
![[H^{+}] = 10^{-pH}](https://tex.z-dn.net/?f=%5BH%5E%7B%2B%7D%5D%20%3D%2010%5E%7B-pH%7D)
![[{H^{+}] = 10^{-8.83}](https://tex.z-dn.net/?f=%5B%7BH%5E%7B%2B%7D%5D%20%3D%2010%5E%7B-8.83%7D)
×
M
×
M
The concentration of
is 1.48 ×
M
The uncertainty of
(
) from the equation
is
×
× 
Where
is the uncertainty of
is the uncertainty of the pH
Hence,
= 2.303 × 1.4791 ×
× 0.04
= 1.36 ×
M
= 0.12 ×
M
Hence, the absolute uncertainty of
is ±0.12 ×
M