Acid–base Equilibria
A 0.005 M solution of HNO3 (strong acid) is prepared at 25°C. Assuming complete dissociation, the pH of the solution is:
Select the correct option:
Solution
2.30
- Acid Nature: HNO3 (Nitric acid) is a strong monoprotic acid.
- Dissociation: It dissociates completely in water: HNO3→H++NO3−.
- Concentration: [H+]=[HNO3]=0.005 M.
- pH Formula: pH=−log[H+].
- Calculation:
- pH=−log(0.005)=−log(5×10−3)
- pH=−[log5+log10−3]
- pH=−[0.699−3]=−[−2.301]=2.301.
- Result: The pH is approximately 2.30.
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About This Question
- Subject
- chemistry
- Chapter
- equilibrium
- Topic
- acid–base equilibria
- Difficulty
- Easy
- Year
- 2025
Solution
Correct Answer:
2.30
- Acid Nature: HNO3 (Nitric acid) is a strong monoprotic acid.
- Dissociation: It dissociates completely in water: HNO3→H++NO3−.
- Concentration: [H+]=[HNO3]=0.005 M.
- pH Formula: pH=−log[H+].
- Calculation:
- pH=−log(0.005)=−log(5×10−3)
- pH=−[log5+log10−3]
- pH=−[0.699−3]=−[−2.301]=2.301.
- Result: The pH is approximately 2.30.
This easy difficulty chemistry question is from the chapter equilibrium, covering the topic of acid–base equilibria. It appeared in the 2025 exam.
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