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## Homework Statement

Hello!

I am trying to solve the following problem:

A 4.00-L base solution contains 0.100 mol total of

NaOH and Sr(OH)2 . The pOH of the solution is 1.51.

Determine the amounts (in moles) of NaOH and

Sr(OH)2 in the solution.

## Homework Equations

3. The Attempt at a Solution [/B]

I am stuck because I am not sure I correctly constructing the solution path:

We have pOH = 1.51, which means that there are 10^(-1.51) moles of OH in solution, i.e. 0.0309 moles per one liter of solution. If I have 4 liters, then shouldn't there be 0.1236 moles of OH in this solution?

But according to the problem there are only 0.100 moles of NaOH and Sr(OH)2; both are strong bases, therefore there 0.100 moles of OH in the 4 liters of solution. How can that be?

Where is my mistake?

Thank you very much!