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

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

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Nov 15th, 2015

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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

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Nov 15th, 2015

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