What is the pH of a 0.0040 M Sr(OH)₂ solution? A) 2.10 B) 2.40 C) 11.60 D) 11.90 E) 12.00

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Quizplus · Accepted Answer

Sr(OH)2 is a strong base that will dissociate completely in water to produce Sr2+ and OH- ions. The concentration of OH- ions can be calculated by multiplying the molarity of the solution by the number of OH- ions produced per mole of Sr(OH)2. In this case, the concentration of OH- ions is 0.0080 M (2 x 0.0040 M). 
The pH of the solution can be calculated using the equation pH = 14.00 - pOH. Therefore, pH = 14.00 - 1.92 (pOH = -log[OH-] = -log[0.0080]) = 12.08, which rounds to 11.90.

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