A buffer solution contains 0.405 M NAHSO3 and 0.332 M Na,SO3. If 0.0248 moles of potassium hydroxide are added to 150. mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding potassium hydroxide) pH =
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![### Buffer Solution Calculation
A buffer solution contains:
- 0.405 M NaHSO₃
- 0.332 M Na₂SO₃
**Problem Statement:**
If 0.0248 moles of potassium hydroxide (KOH) are added to 150 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding potassium hydroxide.)
**Question:**
Calculate the pH:
pH = [ ]
**Explanation:**
To solve this problem, you need to consider the reaction of the buffer components with the potassium hydroxide. Remember that the volume is 150 mL, and you need to keep in mind that the concentrations of the buffering agents (NaHSO₃ and Na₂SO₃) and the added moles of KOH will affect the pH. You may use the Henderson-Hasselbalch equation for the final calculation, assuming the reaction goes to completion.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F03ba95c9-584b-483d-8f8a-8f0f9c4c55b7%2Fb8b1ac5f-e3b8-4671-af38-08892da1dba8%2F8q5zx3_processed.png&w=3840&q=75)
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