A0.500-l sample of h2so4 solution was analyzed by taking a 100.0-ml aliquot and adding 50.0 ml of 0.213 m naoh. after the reaction occurred, an excess of oh2 ions remained in the solution. the excess base required 13.21 ml of 0.103 m hcl for neutralization. calculate the molarity of the original sample of h2so4. (sulfuric acid has two acidic hydrogens.)

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%

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