What is the pOH of a solution that has OH concentration equal to #1.36×10^-10" mol"*"dm"^(-3)# ?

1 Answer
Mar 31, 2018

Answer:

#"pOH"=9.866#

Explanation:

By definition
#"pOH"=-log_(10)["OH"^-]#
where #["OH"^-]# is the hydroxide ion concentration of the solution in #"M"# or #"mol"*"dm"^(-3)#, moles per cubic decimeter, or equivalently moles per liter.

Substituting #["OH"^-]=1.36*10^(-10)" mol"*"dm"^(-3)#,
#"pOH"=9.866#.

Note that by convention the number of decimal places the #"pOH"# value has shall equal to the number of significant figures in the value of #["OH"^-]#. #["OH"^-]# has #3# significant figures, which correspond to three decimal places for the #"pOH"# measurement.