Acid–base Equilibria
Calculate [H+] (in mol L⁻¹) after mixing 25 mL of 0.040 M HCl with 75 mL of water (assume volumes additive).
Select the correct option:
Solution
1.0×10⁻² mol L⁻¹
- Initial Moles: n=M1V1=(0.040 mol/L)×(0.025 L)=0.001 moles.
- Final Volume: Vfinal=25 mL+75 mL=100 mL=0.10 L.
- Application of Dilution Formula: M1V1=M2V2.
- Substitution: 0.040×25=M2×100⟹M2=1001=0.010 M.
- Scientific Notation: 0.010=∗∗1.0×10−2 mol/L**.
- Final Result: The concentration is 10−2 M.
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About This Question
- Subject
- chemistry
- Chapter
- equilibrium
- Topic
- acid–base equilibria
- Difficulty
- Easy
- Year
- 2025
Solution
Correct Answer:
1.0×10⁻² mol L⁻¹
- Initial Moles: n=M1V1=(0.040 mol/L)×(0.025 L)=0.001 moles.
- Final Volume: Vfinal=25 mL+75 mL=100 mL=0.10 L.
- Application of Dilution Formula: M1V1=M2V2.
- Substitution: 0.040×25=M2×100⟹M2=1001=0.010 M.
- Scientific Notation: 0.010=∗∗1.0×10−2 mol/L**.
- Final Result: The concentration is 10−2 M.
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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