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Answer :
Final answer:
The molarity of sulfuric acid in the diluted solution is calculated by determining the mass and moles of sulfuric acid in the initial solution, then using the total volume after dilution. The final molarity is 1.836 M.
Explanation:
To find the molarity of sulfuric acid in the diluted solution, we must first determine the mass of sulfuric acid in the original solution. Since the solution is 49.5% H2SO4 by mass and has a density of 1.39 g/cm3, the mass of H2SO4 in the original 26.0 cm3 sample can be calculated. The mass of the solution is 26.0 cm3 × 1.39 g/cm3 = 36.14 g. The mass of sulfuric acid in this solution is 36.14 g × 49.5% = 17.89 g. The molecular mass of H2SO4 is approximately 98.12 g/mol, so the moles of H2SO4 in the original solution are 17.89 g / 98.12 g/mol = 0.1823 mol. After dilution, the total volume of the solution is 99.3 cm3, or 0.0993 L. The molarity (M) of H2SO4 in the diluted solution is thus 0.1823 mol / 0.0993 L = 1.836 M, rounding to three significant figures.
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