Question

A chemist makes a solution of NaOH for use in an experiment. She dissolves 0.00500 mol NaOH in 1.00 L H2O. The NaOH completely dissociates to form a solution with [OH− ] = 0.00500 M. What is the pH of the solution?

Answer 1

The pOH is 2.30 :D

Step-by-step explanation:

taking the test/assignment on Edg. ;-P Hope this helps! UwU

Answer 2

pH = 11.7

Step-by-step explanation:

Given:

[OH-] = 0.00500 M

To determine:

pH of the solution

Step-by-step explanation:

pH refers to the H+ ion concentration in a given solution whereas pOH indicates the OH- ion concentration.

pH and pOH are related by the following equation:

`pH + pOH = 14 ------(1)`

Here:

`pH = -log[H+]\\\\pOH = -log[OH-]`

When OH- = 0.00500 M

`pOH = -log(0.00500) = 2.30\\`

Based on equation(1):

`pH = 14 - pOH = 14 -2.30=11.7`