Question:
A solution contains 1/10000 moles/l of H⁺ ions. What is the concentration of hydroxyl ions in this solution?
A solution contains 1/10000 moles/l of H⁺ ions. What is the concentration of hydroxyl ions in this solution?
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Ionic product of water:
- [H⁺][OH⁻] = 10^{-14}.
- pH = -log[H⁺].
- pOH = -log[OH⁻].
- [H⁺][OH⁻] = 10^{-14}.
- pH = -log[H⁺].
- pOH = -log[OH⁻].
Updated On: Aug 27, 2026
- 10^{-10} moles/litre
- 10^{-4} moles/litre
- 10^{10} moles/litre
- 10^{4} moles/litre
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The Correct Option is A
Solution and Explanation
Step 1: Understanding the Question:
This question tests knowledge of the ionic product of water and pH calculations.
Step 2: Key Formula or Approach:
The ionic product of water: [H⁺][OH⁻] = 10^{-14} at 25°C.
Step 3: Detailed Explanation:
Given: [H⁺] = 1/10000 = 10^{-4} moles/litre.
Using the ionic product: [OH⁻] = 10^{-14} [H⁺] = 10^{-14} 10^{-4} = 10^{-10} moles/litre.
Thus, the concentration of hydroxyl ions is 10^{-10} moles/litre.
Final Answer:
Thus, the concentration of OH⁻ ions is 10^{-10} moles/litre, which corresponds to option (A).
[0.5cm]
This question tests knowledge of the ionic product of water and pH calculations.
Step 2: Key Formula or Approach:
The ionic product of water: [H⁺][OH⁻] = 10^{-14} at 25°C.
Step 3: Detailed Explanation:
Given: [H⁺] = 1/10000 = 10^{-4} moles/litre.
Using the ionic product: [OH⁻] = 10^{-14} [H⁺] = 10^{-14} 10^{-4} = 10^{-10} moles/litre.
Thus, the concentration of hydroxyl ions is 10^{-10} moles/litre.
Final Answer:
Thus, the concentration of OH⁻ ions is 10^{-10} moles/litre, which corresponds to option (A).
[0.5cm]
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