Calculate the amount (volume) of 5.25% (wt./vol.) NaOCl solution (commercial bleach) required to oxidize 100mg of 9-fluorenol to 9-fluorenone. Whenever appropriate, use balanced chemical equations as a part of your calculation.
IT seems to me that I would start with the balanced equation.
To calculate the amount of NaOCl solution required to oxidize 100mg of 9-fluorenol to 9-fluorenone, we need to use stoichiometry and the balanced chemical equation for the oxidation reaction.
Let's set up the balanced chemical equation for the oxidation of 9-fluorenol to 9-fluorenone:
2 C13H10O (9-fluorenol) + 4 NaOCl (sodium hypochlorite) → 2 C13H8O (9-fluorenone) + 4 NaCl + 2 H2O
From the balanced equation, we can see that 2 moles of 9-fluorenol react with 4 moles of NaOCl to produce 2 moles of 9-fluorenone.
First, we need to convert the given mass of 9-fluorenol (100 mg) to moles. The molar mass of 9-fluorenol is approximately 180.22 g/mol:
100 mg = 0.1 g
Moles of 9-fluorenol = (0.1 g) / (180.22 g/mol)
Now, using the stoichiometry from the balanced equation, we can determine the moles of NaOCl required to react with the calculated moles of 9-fluorenol. According to the balanced equation, 2 moles of 9-fluorenol react with 4 moles of NaOCl:
Moles of NaOCl = (moles of 9-fluorenol) * (4 moles of NaOCl / 2 moles of 9-fluorenol)
Finally, we need to calculate the volume of 5.25% (wt./vol.) NaOCl solution that contains the calculated moles of NaOCl using the information provided.
To find the volume, we need to know the density or the exact concentration of the NaOCl solution. The percentage concentration alone is not sufficient to determine the volume accurately.