Question

A chemist is using a solution of HNO3 that has a pH of 3.75. What is [OH− ] for the solution?

Answer 1

Step-by-step explanation:

It is known that pH is negative log of
`H^(+)`. Also the relationship between pH and pOH is as follows.

pH + pOH = 14

3.75 + pOH = 14

pOH = 14 - 3.75

= 10.25

Therefore, pOH =
`-log [OH^(-)]`

10.25 =
`-log [OH^(-)]`

antilog 10.25 = -
`[OH^(-)]`

`[OH^(-)] = 5.6 * 10^(-11)`

Thus, we can conclude that
`[OH^(-)]` for the solution is
`5.6 * 10^(-11)`.