Answer :
the molarity of commercial sulfuric acid is approximately 0.982 moles per 100 milliliters, which can be converted to 9.82 moles per liter or 9.82 M. Therefore, the correct answer is option 2) 8.18 M.
The molarity of commercial sulfuric acid can be calculated using its weight percentage and specific gravity. In this case, the molarity is determined by considering the concentration of sulfuric acid molecules in a given volume of the solution.
To calculate the molarity, we first need to determine the number of moles of sulfuric acid in the solution. The weight percentage of sulfuric acid (H2SO4) is given as 96.4%. This means that 100 grams of the solution contains 96.4 grams of H2SO4. To convert grams to moles, we divide the mass by the molar mass of sulfuric acid, which is 98.1 grams per mole. Thus, we have (96.4 g / 98.1 g/mol) = 0.982 moles of H2SO4 in 100 grams of the solution.
Next, we consider the specific gravity of the solution, which is given as 1.84. Specific gravity is the ratio of the density of the solution to the density of water. Since water has a density of 1 gram per milliliter, the solution's density is 1.84 grams per milliliter.
To calculate the molarity, we need to determine the volume of the solution that contains 0.982 moles of H2SO4. We can use the density of the solution to convert grams to milliliters. Since 100 grams of the solution occupies 100 milliliters, we can set up the following proportion: (0.982 moles / 100 ml) = (0.982 moles / V ml). Solving for V, we find V ≈ 100 ml.
Thus, the molarity of commercial sulfuric acid is approximately 0.982 moles per 100 milliliters, which can be converted to 9.82 moles per liter or 9.82 M. Therefore, the correct answer is option 2) 8.18 M.
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