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To calculate the pH of a solution given the concentration of hydroxide ions \([OH^-]\), we can follow these steps:

1. **Find the pOH**:
   The formula to calculate the pOH from the hydroxide ion concentration is:
   \[
   \text{pOH} = -\log[OH^-]
   \]
   Here, \([OH^-] = 2.8 \times 10^{-4}\).

   Let's calculate pOH:
   \[
   \text{pOH} = -\log(2.8 \times 10^{-4}) = 3.55
   \]

2. **Use the relationship between pH and pOH**:
   The relationship between pH and pOH is given by:
   \[
   \text{pH} + \text{pOH} = 14
   \]
   Therefore:
   \[
   \text{pH} = 14 - \text{pOH}
   \]
   Substituting the calculated value of pOH:
   \[
   \text{pH} = 14 - 3.55 = 10.45
   \]

Thus, the pH of the solution is **10.45**.

Would you like more details or have any further questions?

Here are some related questions for further exploration:
1. How do you calculate pH from hydrogen ion concentration \([H^+]\)?
2. What is the significance of a solution's pH value?
3. How does pH affect chemical reactions in a solution?
4. What is the relationship between pH and the strength of acids and bases?
5. How do changes in temperature affect pH calculations?

**Tip:** Always remember that a pH above 7 indicates a basic (alkaline) solution, while a pH below 7 indicates an acidic solution.

Calculate the pH of a solution with [OH-] = 2.8 x 10^-4.

Learn how to calculate the pH of a solution when given the hydroxide ion concentration [OH-] = 2.8 x 10^-4. This problem covers key concepts in chemistry and logarithmic functions, suitable for students in Grades 10-12.

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