Answer:
13.301
Explanation:
To calculate the pH of the solution, we must obtain the pOH of the solution as illustrated below:
The dissociation equation is given below
Ba(OH)2 <==> Ba^2+ + 2OH^-
Since Ba(OH)2 dissociate to produce 2moles of OH^-, the concentration of OH^- = 2x0.1 = 0.2M
pOH = - Log[OH^-]
pOH = - Log 0.2
pOH = 0.699
But
pH + pOH = 14
pH = 14 — pOH
pH = 14 — 0.699
pH = 13.301
Answer:
The pH of this barium hydroxide solution is 13.30
Explanation:
Step 1: Data given
Concentration Ba(OH)2 = 0.10 M
Step 2: Calculate [OH-]
Ba(OH)2 ⇒ Ba^2+ + 2OH-
[OH-] = 2*0.10 M
[OH-] = 0.20 M
Step 3: Calculate pOH
pOH = -log[OH-]
pOH = -log(0.20)
pOH = 0.70
Step 4: Calculate pH
pH + pOH = 14
pH = 14 -pOH
pH = 14 - 0.70
pH = 13.30
The pH of this barium hydroxide solution is 13.30
