Calculate the pH and pOH of a 0.159 M solution of KOH.
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calculate the pH and pOH of a 0.157 m solution of KOH?
An aqueous solution contains 0.159 M of methylamine. Kb for methylamine is 4.4 x 10-4. What is the pOH of this solution?
What are the pH and pOH for a 0.025 M KOH solution?
A) pH = +1.60 and pOH =+12.40
B) pH = +12.40 and pOH = +1.60
C) pH = -12.40 and pOH = -1.60
D) pH = +12.40 and pOH = -1.60
E) pH = -1.60 and pOH = +1.60