Calculate the amount (volume) of 5.25% (wt./vol.) NaOCl solution (commercial bleach) required to oxidize 100 mg of 9-fluorenol to 9-fluorenone. Whenever appropriate, use balanced chemical equations as a part of your calculation.
Start with the balanced equation? Have you figured that out yet?
NaOCl+ CH3COOH-> HOCl+ CH3COO+ Na
To calculate the volume of the NaOCl solution required for the oxidation reaction, we need to follow these steps:
Step 1: Write the balanced chemical equation for the oxidation reaction.
The balanced chemical equation for the oxidation of 9-fluorenol to 9-fluorenone using NaOCl can be written as follows:
C13H10O (9-fluorenol) + NaOCl (sodium hypochlorite) -> C13H8O (9-fluorenone) + NaCl (sodium chloride) + H2O
Step 2: Determine the molar mass of 9-fluorenol.
The molar mass of 9-fluorenol (C13H10O) can be calculated by summing the atomic masses of each element:
C (13 atoms x 12.01 g/mol) + H (10 atoms x 1.01 g/mol) + O (1 atom x 16.00 g/mol) = 180.22 g/mol
Step 3: Convert the mass of 9-fluorenol to moles.
Given that you have 100 mg of 9-fluorenol, you can convert this mass to moles using the molar mass calculated in step 2:
100 mg x (1 g / 1000 mg) x (1 mol / 180.22 g) = 0.000556 mol
Step 4: Determine the stoichiometry of the reaction.
By comparing the balanced chemical equation from step 1, we can determine that the molar ratio between 9-fluorenol and NaOCl is 1:1. This means that 1 mol of 9-fluorenol requires 1 mol of NaOCl.
Step 5: Calculate the required moles of NaOCl.
Since the moles of 9-fluorenol and NaOCl are equal, the amount of NaOCl required is also 0.000556 mol.
Step 6: Convert moles of NaOCl to volume.
To convert moles to volume, we need to know the molarity of the NaOCl solution (commercial bleach). We are given that it is a 5.25% (wt./vol.) solution.
5.25% (wt./vol.) means that 5.25 g of NaOCl is present in 100 mL (or 0.100 L) of solution.
Step 7: Calculate the concentration of NaOCl in moles per liter.
5.25 g of NaOCl is equal to 5.25/74.44 mol (using the molar mass of NaOCl).
Concentration (molarity) = (amount of solute in moles) / (volume of solution in liters)
Concentration = (5.25/74.44) mol / 0.100 L = 0.070478 mol/L
Step 8: Calculate the volume of NaOCl solution required.
Given that we have 0.000556 mol of NaOCl required, we can calculate the volume using the formula:
Volume = (moles of solute) / (concentration)
Volume = 0.000556 mol / 0.070478 mol/L = 0.00789 L = 7.89 mL (rounded to the nearest hundredth)
Therefore, approximately 7.89 mL of the 5.25% NaOCl solution is required to oxidize 100 mg of 9-fluorenol to 9-fluorenone.