1. Understanding Strong Bases
Strong bases completely dissociate in water, meaning they break apart into their ions. For Sr(OH)₂, this looks like:
Sr(OH)₂ (aq) → Sr²⁺ (aq) + 2OH⁻ (aq)
2. Calculating pOH
Since Sr(OH)₂ produces two hydroxide ions (OH⁻) for every molecule, a 1 M solution of Sr(OH)₂ will have a 2 M concentration of OH⁻ ions.
We can use the pOH formula:
pOH = -log[OH⁻]
For a 1 M solution of Sr(OH)₂:
pOH = -log(2) ≈ -0.301
3. Calculating pH
The relationship between pH and pOH is:
pH + pOH = 14
Therefore:
pH = 14 - pOH ≈ 14 + 0.301 ≈ 14.301
Important Note:
* The actual pH of a Sr(OH)₂ solution will depend on its concentration.
* It's important to note that very concentrated solutions of Sr(OH)₂ can have pH values above 14, but the pH scale is typically limited to 0-14.
Let me know if you'd like to calculate the pH of a specific concentration of Sr(OH)₂!
