A chemist must dilute 52.9mL of 2.84M aqueous iron(III) bromide FeBr3 solution until the concentration falls to 2.00M . She'll do this by adding distilled water to the solution until it reaches a certain final volume.Calculate this final volume, in milliliters. Round your answer to 3 significant digits.
Question
A chemist must dilute 52.9mL of 2.84M aqueous iron(III) bromide FeBr3 solution until the concentration falls to 2.00M . She'll do this by adding distilled water to the solution until it reaches a certain final volume.Calculate this final volume, in milliliters. Round your answer to 3 significant digits.
Solution
To solve this problem, we can use the formula M1V1 = M2V2, where M1 is the initial molarity, V1 is the initial volume, M2 is the final molarity, and V2 is the final volume.
Given: M1 = 2.84 M V1 = 52.9 mL M2 = 2.00 M
We need to find V2.
Substituting the given values into the formula, we get:
2.84 M * 52.9 mL = 2.00 M * V2
Solving for V2, we get:
V2 = (2.84 M * 52.9 mL) / 2.00 M
V2 = 75.246 mL
Rounding to three significant digits, the final volume V2 is 75.2 mL.
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