Description
What is the pH of a 0.0035 M Ba(OH)2 solution?
Explanation & Answer
Thank you for the opportunity to help you with your question!
The formula for finding the pH of 0.0035 M Ba(OH)2 is = 14.000 - (- log [OH^(-1) moles])
I assume Barium Hydroxide is a strong base. Therefore all the hydroxide ions ionize.
0.0035 * 2 = 0.007 moles of OH, because each molecule of Ba(OH)2 has 2 hydroxide ions.
pH of this solution = 14 - (-log [0.007]) = 14 - (2.1549) = 11.845 pH
Answer choice D ) 11.85
Please let me know if you need any clarification. I'm always happy to answer your questions.