5. (3 pts) What pH is necessary to start precipitation of Ba(OH), from a 0.250 M...

Question

Question

science chemistry

Answer 1

Answer #1

You have the expression of Ksp:

Ksp = [Ba + 2] * [OH -] ^ 2 = 4 * X ^ 3 = 5x10 ^ -3

It clears X = 0.108 M

[OH-] = 2 * X = 2 * 0.108 = 0.216 M

POH and pH are calculated:

pOH = - log 0.216 = 0.67

pH = 14 - 0.67 = 13.33

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Answer 2

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