Two drops of a 0.35 M imidazole solution were added to a solution in a cuvette c

Question

Two drops of a 0.35 M imidazole solution were added to a solution in a cuvette containing ferrihemoglobin. The mass of the ferrihemoglobin solution in the cuvette was measured before the addition of the imidazole, and then the mass of the total final solution in the cuvette was measured after adding the imidazole. The results are recorded in the following table Assuming that the densities of all solutions are identical, calculate the concentration (in molarity) of imidazole in the final solution after the 2 drops of imidazole were added. Provide answer with correct units and significant figures. (Since the experiment has been designed to ensure that imidazole is the excess reagent, the concentration calculated can be assumed to be the equilibrium concentrations as well.)

Explanation / Answer

If the densities are the same, let's assume that they are both 1g/ml
0.076g imidazole / 1g/ml = 0.076ml imidazole added
0.076ml = 7.6x10^-2ml = 7.6x10^-5L
7.6x10^-5L x 0.2M = 1.52x10^-5moles imidazole added

2.81g / 1g/ml = 2.81ml = 0.00281L = volume of ferrihemoglobin
total volume = 2.81ml + 0.076ml = 2.886ml = 0.002886L
1.52x10^-5moles imidazole / 0.002886L = 0.0053M

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