Question

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

Answer 1

Answer:

[OH-] = 5.62

n = -11

pOH = 10.25

Explanation: Just did it on edge

Answer 2

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 = - $[OH^{-}]$

                         $[OH^{-}] = 5.6 \times 10^{-11}$  

Thus, we can conclude that $[OH^{-}]$ for the solution is $5.6 \times 10^{-11}$.