# What is the pH of a 0.0035 M Ba(OH)2 solution?

Anonymous
timer Asked: Nov 15th, 2015
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### Question Description

What is the pH of a 0.0035 M Ba(OH)2 solution?

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alancheng
School: University of Virginia

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.

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Anonymous
Tutor went the extra mile to help me with this essay. Citations were a bit shaky but I appreciated how well he handled APA styles and how ok he was to change them even though I didnt specify. Got a B+ which is believable and acceptable.

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