What is the #"pOH"# of a solution if the #["OH"^-] = 33.5 xx 10^-2# #"M"#? Chemistry Acids and Bases Stoichiometry with Acid and Base Dissociation 1 Answer Monzur R. Apr 15, 2017 #"pOH"=0.475# Explanation: The chemical definition of #"pOH"# or in fact, the #"p"# of any value/constant is given as the cologarithm of that thing. That is the negative (or reciprocal) logarithm of that thing. #therefore# #"pOH"=-log["OH"^-]=log(1/(["OH"^-]))# #"pOH"=-log(3.35xx10^-1)=0.475# Answer link Related questions Question #5c3cd What are some common mistakes students make with stoichiometry? What is an example of a stoichiometry practice problem? What are some examples of acid and base dissociation? What is an example of an acid and base dissociation practice problem? What are some common mistakes students make with acid and base dissociation? What is stoichiometry with acid and base dissociation? What are some examples of stoichiometry with acid and base dissociation? What is an example of a stoichiometry with acid and base dissociation practice problem? How do we relate stoichiometry to everyday processes? See all questions in Stoichiometry with Acid and Base Dissociation Impact of this question 1717 views around the world You can reuse this answer Creative Commons License