A standard solution of Mn2+ was prepared by dissolving 0.250 g of Mn in 10 mL of concentrated HNO3 (measured with a graduated cylinder). The resulting solution was quantitatively transferred to a 100 mL volumetric flask and diluted to volume with distilled water. A 10 mL aliquot of the solution was pipetted into a 500 mL volumetric flask and diluted to volume.
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Step 1: Calculate the molarity of the standard Mn2+ solution
To calculate the molarity, we need to know the number of moles of Mn2+ and the volume of the final solution.
Given:
Mass of Mn = 0.250 g
Volume of HNO3 = 10 mL
Final volume of standard solution = 100 mL
First, let's convert the mass of Mn to moles using the molar mass of Mn.
Molar mass of Mn = 54.938 g/mol
Moles of Mn = (0.250 g) / (54.938 g/mol)
Next, we need to calculate the molarity of the concentrated HNO3 solution. Since the volume of HNO3 is given, we can assume it is the same as its concentration.
Molarity of HNO3 = 10 M (assumed)
Now, let's calculate the moles of Mn2+ in the 10 mL HNO3 solution.
Moles of Mn2+ = Moles of Mn
Finally, we can calculate the concentration (Molarity) of the standard Mn2+ solution in the 100 mL volumetric flask.
Molarity of standard Mn2+ solution = (Moles of Mn2+) / (Final volume of solution in liters)
Step 2: Calculate the molarity of the diluted Mn2+ solution
Given:
Volume of the aliquot = 10 mL
Final volume of the diluted solution = 500 mL
Since we are diluting a known volume of the standard solution, the moles of Mn2+ will remain constant.
Moles of Mn2+ in the diluted solution = Moles of Mn2+ in the standard solution
Finally, we can calculate the molarity of the diluted Mn2+ solution.
Molarity of diluted Mn2+ solution = (Moles of Mn2+) / (Final volume of solution in liters)
To understand the problem, let's break it down step by step:
Step 1: Preparation of Standard Mn2+ Solution
- Starting with 0.250 g of Mn (manganese)
- Dissolve the manganese in 10 mL of concentrated HNO3 (nitric acid), which was measured using a graduated cylinder.
- The resulting solution is then quantitatively transferred to a 100 mL volumetric flask.
- The volumetric flask is then filled to the mark (volume) with distilled water.
Step 2: Preparation of a 10 mL Aliquot
- Take a 10 mL portion (aliquot) of the standard Mn2+ solution prepared in Step 1.
- This 10 mL aliquot is then pipetted (measured using a pipette) into a 500 mL volumetric flask.
- The volumetric flask is filled to the mark (volume) with distilled water.
Now, let's address any specific questions or calculations you have related to this problem.