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charle [14.2K]
2 years ago
4

A chemist prepares a solution of ironIII bromide FeBr3 by measuring out 47.6mg of FeBr3 into a 50.mL volumetric flask and fillin

g to the mark with distilled water.
Calculate the molarity of Br− anions in the chemist's solution.

Be sure your answer is rounded to 2 significant digits.
Chemistry
1 answer:
adell [148]2 years ago
7 0

A chemist prepares a solution of iron(III)bromide FeBr₃ by measuring out 47.6 mg of FeBr₃ into a 50.0 mL volumetric flask and filling to the mark with distilled water. the molarity of Br⁻ anions in the chemist solution is 0.0096 M

Molarity is defined as no. of solute present in 1 liter of solution.

M = n / v

no. of moles = mass / molar mass

mass of FeBr₃ = 47.6 mg = 0.0476 g

molar mass FeBr₃ = 295.6 g/mol

moles of FeBr₃ = 0.0476 g / 295.6 g/mol

                         =  0.00016 mol

now,

Molarity = 0.00016 mol / 0.05 L

             = 0.0032 M

1 mol of FeBr₃ gives 3 moles of Br⁻

so, 0.0032 moles of FeBr₃ = 3 × 0.0032 = 0.0096 moles of Br⁻

Molarity of Br⁻ = 0.0096 M

Thus, A chemist prepares a solution of iron(III)bromide FeBr₃ by measuring out 47.6 mg of FeBr₃ into a 50.0 mL volumetric flask and filling to the mark with distilled water. the molarity of Br⁻ anions in the chemist solution is 0.0096 M.

To learn more about Molarity here

brainly.com/question/15411303

#SPJ1

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