10 posts • Page 1 of 1
What is the difference between [OH-] and pOH? Question 5 on sapling asks for us to list both but I thought that they meant the same thing, are we supposed to put the same thing for both of them on Sapling or are they different. Could someone clarify what the difference between the two are?
[OH-] and pOH aren't the same thing but they're related. The difference between the two is that [OH-] represents the concentration of [OH-] or the molarity of OH-. It basically represents the concentration of OH- that is produced when a strong base reacts with water for example. pOH is a value that represents the basicity of a solution. They're related because in order to find pOH, you take the -log[OH-]. I hope that helps!
My understanding is that pH refers to the concentration of H, or more specifically the concentration of H3O+, whereas pOH is the concentration of OH-. To calculate pH, use pH =-log [H3O+] and to calculate pOH, use pOH = -log [OH-]. To if given one and asked to calculate the other, you should be able to subtract from 14 because of the relationship stated above where pH + pOH = 14.
Similar to how pH is not the same as [H3O+] (the concentration of H3O+), pOH is not the same as [OH-]. Like previous users states, pOH = -log[OH-], and [OH-] = 10^-pOH. I believe Dr. Lavelle stated in the lecture that the pH and pOH scale are simply easier methods of describing the concentration of H3O+ and OH-, respectively, in the solution. So instead of saying the solution has an OH- concentration of 1.0 x 10^-8, we would say the pOH is 8 (or the pH is 6). It's just used to make things easier to describe.
[OH-] is the concentration of OH- ions while pOH is a measure of the basicity of a solution. (It is similar to how [H+] is the concentration of H+ ions while pH is a measure of the acidity of a solution.) pOH = -log([OH-] )
Who is online
Users browsing this forum: No registered users and 2 guests