how much water should be added to 1l of 0.01M CH3COOH solution to make it 0.0025M?
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Answered by
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Given:
Initial Volume of CH3COOH, V1 = 1 L
Initial Molarity, M1 = 0.01 M
Final Molarity, M2 = 0.0025 M
To Find:
Final Volume of CH3COOH, i.e., V2.
Calculation:
- Using the molarity equation, we get:
M1 × V1 = M2 × V2
⇒ V2 = (M1 × V1) / M2
⇒ V2 = (0.01 × 1) / 0.0025
⇒ V2 = 4 L
- So, 4 L of water should be added to CH3COOH solution to get the required concentration.
Answered by
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Thus we need 4 L of water to make 0.0025 m solution.
Explanation:
We are given that:
- Initial Molarity, M1 = 0.01 M
- Final Molarity "M2" = 0.0025 M
- Initial Volume of CH3COOH, V1 = 1 L
- To Find: Final Volume of CH3COOH "V2" = ?
Solution:
By using the molarity equation, we get:
M1 × V1 = M2 × V2
V2 = (M1 × V1) / M2
V2 = (0.01 × 1) / 0.0025
V2 = 4 L
Thus we need 4 L of water to make 0.0025 m solution.
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