Calculate the pH of a 0.2 M solution of KOH.

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Question: Calculate the pH of a 0.2 M solution of KOH.

Options:

Correct Answer: 13

Solution:

pOH = -log(0.2) = 0.7, thus pH = 14 - 0.7 = 13.3.

Calculate the pH of a 0.2 M solution of KOH.

Calculate the pH of a 0.2 M solution of KOH.

Step 1: Understand that KOH is a strong base and will completely dissociate in water. This means that a 0.2 M solution of KOH will have a hydroxide ion concentration [OH-] of 0.2 M.
Step 2: Calculate the pOH using the formula pOH = -log[OH-]. Here, [OH-] = 0.2 M, so pOH = -log(0.2).
Step 3: Use a calculator to find -log(0.2). This gives you pOH = 0.7.
Step 4: Use the relationship between pH and pOH, which is pH + pOH = 14. Since you found pOH = 0.7, you can find pH by rearranging the equation: pH = 14 - pOH.
Step 5: Substitute the value of pOH into the equation: pH = 14 - 0.7, which equals 13.3.

pH and pOH Calculations – Understanding the relationship between pH, pOH, and the concentration of hydroxide ions in a solution.
Strong Bases – Recognizing that KOH is a strong base that fully dissociates in solution.