What is the pH of a solution that has a [OH–] of 3.07×10-3 M ?

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Answer 1 · 2018-04-07T01:46:47

#11.49#

We first find the #"pOH"# of the solution by the equation,

#"pOH"=-log[OH^-]#

#[OH^-]# is the hydroxide ion concentration in terms of molarity

Here, we have,

#"pOH"=-log[3.07*10^-3 \ "M"]#

#~~2.51#

The #"pH"# and #"pOH"# of a solution are related by the equation,

#"pH + pOH"=14#

Therefore, this solution's #"pH"# will be,

#"pH"=14-2.51#

#=11.49#