What is the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2?
The question is –
What is the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2?
Answer:
⇒ The pH of a 0.10 M solution of barium hydroxide is approximately 13.3.
Explanation:
Barium hydroxide is a strong base, and it dissociates completely in water:
⇒ Ba(OH)2 → Ba2+ + 2OH–
This means that one mole of barium hydroxide will generate two moles of hydroxide ions. Therefore, a 0.10 M solution of barium hydroxide will generate 0.10 M * 2 = 0.20 M of OH– ions.
The concentration of OH– ions is related to the pH of the solution by the expression:
⇒ pOH = -log[OH–]
We can use this expression to calculate the pOH of the solution:
∴ pOH = -log(0.20) = 0.699
The pH and the pOH of a solution are related by the expression:
⇒ pH + pOH = 14.00
So, we can use this to find the pH:
pH = 14.00 – pOH = 14.00 – 0.699 = 13.301
Therefore, the pH of a 0.10 M solution of barium hydroxide is approximately 13.3, indicating a strong basic solution.
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