A solution is made by dissolving 0.0890 moles of Ba(OH)2 in enough water to make 545 mL of solution. What is the pH of the resulting solution

The pH of this solution is 13.515

Explanation:

Step 1: Data given

Number of moles Ba(OH)2 = 0.0890 moles

Volume = 545 mL

Step 2: Calculate moles OH

Ba(OH)2 → Ba^2+ + 2OH-

In 1 moles Ba(OH)2 we have 2 moles OH-

In 0.0890 moles Ba(OH)2 we have 2*0.0890 = 0.178 moles OH-

Step 3: Calculate concentration of OH-

[OH-] = moles / volume

[OH-] = 0.178 moles / 0.545 L

[OH-] = 0.327 M

Step 4: Calculate pOH

pOH = -log[OH-]

pOH = -log(0.327)

pOH = 0.485

Step 5: Calculate pH

pH + pOH = 14

pH = 14 - pOH

pH = 14 - 0.485

pH = 13.515

The pH of this solution is 13.515

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