Answer to Question #159115 in General Chemistry for Dexther Villanueva

Question

The sulfur from 4.0000g of steel is evolved as H2S and titrated with 1.60ml of 0.0500M iodine solution. What is the percentage of S in the steel? What is the value of 1.000ml of the iodine in terms of grams As2O3? How many milliliters of the iodine will be reduced by 40.00ml of Na2S2O3 solution of which 1.000ml ≈ 0.006354g Cu? What volume of iodate-iodide solution containing 10.0mmol of KIO3 and 50.0g of KI per liter would be required to titrate the H2S from 5.0000g of the above steel? The equations involved are as follows:

H2S + I2 → S + 2I- + 2H+

AsO3 -3 + 2HCO3 - + I2 → AsO4 -3 + 2I- + 2CO2 + H2O

2Cu+2 + 4I- → 2CuI + I2

IO3 - + 6I- + 6H+ → 3I2 + I- + 3H2O

Answer 1

The sulfur from 4.0000g of steel is evolved as H2S and titrated with 1.60ml of 0.0500M iodine solution. What is the percentage of S in the steel? What is the value of 1.000ml of the iodine in terms of grams As2O3? How many milliliters of the iodine will be reduced by 40.00ml of Na2S2O3 solution of which 1.000ml ≈ 0.006354g Cu? What volume of iodate-iodide solution containing 10.0mmol of KIO3 and 50.0g of KI per liter would be required to titrate the H2S from 5.0000g of the above steel?