# A 1.50 g sample of an ore containing silver was dissolved, and all of the Ag+ was converted to0.124 g of Ag2S. What was the percentage of silver in… A 1.50 g sample of an ore containing silver was dissolved, and all of the Ag+ was converted to0.124 g of Ag2S. What was the percentage of silver in…

A 1.50 g sample of an ore containing silver was dissolved, and all of the Ag+ was converted to0.124 g of Ag2S. What was the percentage of silver in…

A 1.50 g sample of an ore containing silver was dissolved, and all of the Ag+ was converted to0.124 g of Ag2S. What was the percentage of silver in…
When `Ag^+` was converted to `Ag_2S` we will get the `Ag_2S` precipitate and we can measure the weight of it as it is done here. `2Ag^++S^(2-) rarr Ag_2S`Molar mass of `Ag_2S = 247.8g/(mol)` Mass of `Ag_2S` obtained `= 0.124g` Moles of `Ag_2S ` obtained `= 0.124/247.8 = 0.0005` Mole ratio`Ag^+:Ag_2S = 2:1` Amount of Ag in ore `= 0.0005xx2 = 0.001mol` Molar mass of Ag `= 107.86g/(mol)` Mass of Ag in ore `= 0.001xx107.86 = 0.1079g` Percentage of Ag in ore `= 0.1079/1.5xx100% = 7.19%` So the percentage of Ag in ore is 7.19%