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Calculate the pH of a 4.00 x 10^-2 mol dm^-3 solution of Ba(OH)2

The easiest way to answer this question is by using the equation pH + pOH = 14. 

Firstly, we need to work out the number of moles of OH- in the solution. As the formula for Ba(OH)2  shows that it has 2 moles of OH- for every 1 mole of Ba+ , the number of moles of OH- ions will be equal to twice the concentration of the solution. 

Therefore, there are 8.00 x 10-12 moles of OH- ions in the solution.

As pOH= -log (OH-), pOH = -log (8.00 x 10-12

Therefore pOH= 1.097

By rearranging the formula pH + pOH = 14, we get 14-pOH= pH

Therefore, 14-1.097= 12.9

The pH of the solution is 12.9

Chloe M. IB Chemistry tutor, A Level Chemistry tutor, GCSE Chemistry ...

7 months ago

Answered by Chloe, who has applied to tutor IB Chemistry with MyTutor


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