How do you prepare a 1 molar ferric chloride solution?
Answer (2)
To prepare a 1 molar solution of ferric chloride, weigh 162.2 grams of FeCl₃ and dissolve it in distilled water until the total volume reaches 1 liter. Ensure the solution is well mixed for accurate concentration. This procedure allows for the creation of a solution suitable for various chemical applications.
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To prepare a 1 molar (1 M) ferric chloride (FeCl₃) solution, follow these steps:
Understand Molarity: Molarity is the number of moles of solute per liter of solution. A 1 M solution has 1 mole of solute in 1 liter of solution.
Calculate the Molar Mass of Ferric Chloride: Ferric chloride (FeCl₃) has a molar mass of approximately 162.2 g/mol. This is calculated by adding the atomic masses of iron (Fe) which is about 55.8 g/mol and chlorine (Cl), with each Cl contributing roughly 35.5 g/mol. So, 55.8 + 3(35.5) = 162.2 g/mol.
Measure the Correct Amount of Ferric Chloride: To make 1 L of a 1 M solution, you need 1 mole of FeCl₃. Therefore, you need to weigh out 162.2 grams of FeCl₃ powder.
Dissolve in Water: Pour the 162.2 grams of FeCl₃ into a container. Add distilled water slowly while stirring to dissolve the powder.
Transfer and Dilute to the Final Volume: After the FeCl₃ has dissolved completely, transfer the solution to a 1 L volumetric flask. Add distilled water until the bottom of the meniscus reaches the 1 L mark on the flask.
Mix the Solution Thoroughly: Secure the cap and invert the volumetric flask several times to ensure the solution is well mixed.
By following these steps, you will have successfully prepared a 1 M ferric chloride solution, which is useful for various chemical experiments and instructional purposes.
