Question
Please help me to understand how I would make thisdetermination: If I have a 2.50 gram sample of unknown silver salt (possiblyAgClo3, AgClo4,AgNO3, AgF) isdissolved in water. An excess of HCL solution is added and1.88 g of AgCl is collected. Determine the identity of thesilver salt? I know it would not be AgF due to the insolubility, but Ireally do not want to figure it out by elimination. I need toknow how to set it up to determine? Please help me to understand how I would make thisdetermination: If I have a 2.50 gram sample of unknown silver salt (possiblyAgClo3, AgClo4,AgNO3, AgF) isdissolved in water. An excess of HCL solution is added and1.88 g of AgCl is collected. Determine the identity of thesilver salt? I know it would not be AgF due to the insolubility, but Ireally do not want to figure it out by elimination. I need toknow how to set it up to determine?
Explanation / Answer
Molar mass of AgClO4 is = 108 + 35.5 +4 * 16 = 207.5 g Molar mass of AgNO3 is = 108 + 14 + 3 *16 = 170 g Molar mass of AgF is = 108 + 19 = 127 g Molar mass of AgClO4 is = 108 + 35.5 +4 * 16 = 207.5 g Molar mass of AgNO3 is = 108 + 14 + 3 *16 = 170 g Molar mass of AgF is = 108 + 19 = 127 g Molar mass of AgCl is = 108 + 35.5 = 143.5 g Molar mass of AgClO3 is = 108 +35.5 + 3 * 16 = 191.5 g 191.5 g of AgClO3 produces 143.5 g of AgCl 2.5 g of AgClO3 produces X g of AgCl So, X = ( 143.5 * 2.5 ) / 191.5 =1.87 g ~1.88 g So, the desired compound is AgClO3