determine the ph of a 0.0500 m solution of potassium hydroxide (koh).
determine the ph of a 0.0500 m solution of potassium hydroxide (koh).
Answer
Explanation:
Step1: Determine $[OH^-]$ concentration
KOH is a strong - base and dissociates completely as $KOH\rightarrow K^+ + OH^-$. So, if $[KOH]=0.0500\ M$, then $[OH^-]=0.0500\ M$.
Step2: Calculate pOH
The formula for pOH is $pOH =-\log[OH^-]$. Substituting $[OH^-]=0.0500\ M$ into the formula, we get $pOH=-\log(0.0500)$. $pOH = 1.301$.
Step3: Calculate pH
We know the relationship $pH + pOH=14$. So, $pH = 14 - pOH$. Substituting $pOH = 1.301$ into the formula, we get $pH=14 - 1.301 = 12.699\approx12.70$.
Answer:
$12.70$