6.6×10−3 M Ba(OH)2 and 1.00×10−2 M BaCl2 what is [OH-] of solution?

Question

6.6×10−3 M Ba(OH)2 and 1.00×10−2 M BaCl2  what is [OH-] of solution?

DrBob222 · Answer

Ba(OH)2 ==> Ba^2+ + 2OH^- Ksp = (Ba^2+)(OH^-)^2 (Ba^2+) = 6.6E-3 from Ba(OH)2 and 1E-2 from BaCl2. Solve for (OH^-)

Lilly · Answer

So do you add the 6.6E-3 and 1E-2 together as the value for Ba^2+?