How to Calculate pH of a 0.15 M Solution of Potassium Hydroxide Using Kw Value

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To calculate the pH of a 0.15 M potassium hydroxide (KOH) solution, it is assumed that KOH fully ionizes as a strong base. The hydroxide ion concentration [OH-] is determined to be 0.15 M, leading to a pOH of approximately 0.824. Using the relationship pH + pOH = 14, the pH is calculated to be about 13.18. The discussion emphasizes the importance of recognizing KOH as a strong base for accurate calculations. Overall, the method for determining pH from pOH using the ionization of strong bases is clearly outlined.
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Homework Statement


A strong base cane be assumed to be fully ionised in dilute solution. Use the Kw value to calculate the hydrogen ion concentration and hence the pH of a 0.15 M solution of potassium hydroxide, KOH.

Homework Equations


The Attempt at a Solution



Problem is, I don't know where to begin, so any advice on how to proceed or pointers would be appreciated.
 
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Yeah, I think I managed to do it meself. Forgot it was a strong base.

pOH=-log10[OH-]
pOH=-log10[0.15M]
pOH=0.824

pH+pOH=14 ∴ pH=14-0.824=13.176
 
Too many digits - 13.18 would be more to my liking. Other than that you did OK.
 

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