Answer:
Option A. 2.82 L
Explanation:
Step 1:
Data obtained from the question.
pH = 13.55
Step 2:
Determination of the pOH of the solution.. This is illustrated below:
pH + pOH = 14
pH = 13.55
13.55 + pOH = 14
Collect like terms
pOH = 14 - 13.55
pOH = 0.45
Step 3:
Determination of the concentration of the OH ion.
This is illustrated below:
pOH = - Log [OH-]
pOH = 0.45
0.45 = - Log [OH-]
- 0.45 = Log [OH-]
[OH-] = antilog (- 0.45)
[OH-] = 0.355 M
Step 4:
Determination of the molarity of KOH. This is illustrated below:
First, we'll write the dissociation equation of KOH as follow:
KOH —> K+(aq) + OH-(aq)
From the balanced equation above,
1 mole of KOH produced 1 mole of OH-.
Therefore, 0.355 M of KOH will definitely produce 0.355 M of OH-.
The molarity of KOH is 0.355 M
Step 5:
Determination of the volume of the solution needed to dissolve 1 mole of KOH. This is illustrated below:
Mole of KOH = 1 mole
Molarity of KOH = 0.355 M
Volume =?
Molarity = mole /Volume
Volume = mole /Molarity
Volume = 1/0.355 M
Volume = 2.82L
