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Question- The sulfur in a 0.575 g sample of a organic thiamine was converted to H2S, which was then absorbed in 15.00 mL of 0.0320 M I2. This amount of I2 was in excess of that required to oxidize the H2S to elemental sulfur; I- was the reaction product. H2S + I2 --> S + 2I- + 2H+. The excess I2 was determined by titration with thiosulfate [S2O3]2- with the reaction products being tetrathionate [S4O6]2- and I-. 26.29 mL of 0.0175 M Na2S203 was required to reduce the excess I3. What was the mass of the sulfur in the original sample?
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the concentration of nitrogen in water at 25degc was determined to be 7.2 times 10-6 m. calculate the partial pressure
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