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Answer :
The calculated molarity of the new solution is 0.025 M.
If 25.0 mL of a 2.00 M HCl solution is diluted to 2.00 L, what is the molarity of the new solution?
To solve the given problem, we will use the dilution formula: M₁V₁ = M₂V₂, where:
M₁ is the initial molarity
V₁ is the initial volume
M₂ is the final molarity
V₂ is the final volume
Given:
Initial Molarity (M₁) = 2.00 M
Initial Volume (V₁) = 25.0 mL
Final Volume (V₂) = 2.00 L (which is 2000 mL)
We need to find the final molarity (M₂). Rearranging the dilution formula to solve for M₂ gives:
M₂ = (M₁V₁) / V₂
Substitute the values into the formula:
M₂ = (2.00 M × 25.0 mL) / 2000 mL
M₂ = 0.025 M
Therefore, the molarity of the new HCl solution after dilution is 0.025 M.
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Final answer:
The molarity of a solution decreases when it is diluted because the number of solute particles (in this case, HCl) is spread out over a greater volume. In this case, a solution of HCl was diluted from a molarity of 2.00 M to 0.025 M.
Explanation:
The subject matter here is dilutions in the field of chemistry, more specifically, the calculation of molarity after dilution of a solution. In this case, you start with a solution of a known molarity, 2.00 M HCl, and a known volume, 25.0 mL. When you dilute this solution to a larger volume, here 2.00 L, the number of moles of HCl does not change, but they are now spread out in a larger volume of solution, thus reducing the molarity.
First, you would calculate the number of moles of HCl in the original solution using the formula: Moles = Molarity x Volume. This gives you 2.00 M x 0.025 L = 0.05 mol of HCl.
After the dilution, the number of moles remains the same but the volume changes to 2.00 L. To find the new molarity, divide the number of moles by the new volume: 0.05 mol / 2.00 L = 0.025 M.
So, the molarity of the new solution after dilution is 0.025 M.
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