What is the pH of a solution that has a concentration of hydronium ions that is 1.8 × 10-4 M OH-? Show, or explain, the work used to solve this problem.

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What is the pH of a solution that has a concentration of hydronium ions that is 1.8 × 10-4 M OH-? Show, or explain, the work used to solve this problem.

Chemistry
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makes no sense I have no idea how to do this
pOH = -log[OH-] pH + pOH =14
you meant hydroxide ions, right?

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I don't so that was the exact question.
Is there a formula? I could do it if I had one.
in your question, you said hydronium but then you wrote OH-, which one is it?
I think the (-) is supposed to be up higher if that makes a difference. 1.8 × 10^-4 M OH^-
I guess that makes no sense at all
lol no i understand that part.. but hydronium = H3O+ and hydroxide OH- so it's hydroxide? lol i'm just confused b/c you said two different things and one or the other completely changes the answer
Well the question it asked me was that so i dont know if its right or not :(
there must be a type somewhere if it's 1.8 × 10^-4 M OH^- .. use the equations i gave you first if it's 1.8 × 10^-4 M H3O+ then just use pH= -log[H3O+]
typo**
what do I put into the equation. Whats a -log Ahhh sorry I sound so stupid I suck so bad at chemistry :(
you input the number.. 1.8 × 10^-4 or 0.00018 then press log on your calculator .. which turns into a logarithm base 10 then press the negative sign
lol it's cool, everyone's gotta learn someday, no one is born with this knowledge
okay I did that I got - 3.74472749..... Does that sound right?
you didn't press the negative sign, it's supposed to be 3.74 if it was a negative number it would be very very acidic
Ohhhh, okay. Does that mean the ph is 3.74..?
if the concentration they gave you was in H3O+ ions, if it was OH- you have to subtract from 14
okay so 14-3.74? so 10.26
yep
Thank you!
no problem !

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