The mass of silver chloride is 73,487 g.
To determine the mass of silver chloride produced, we need to know the balanced chemical equation for the reaction between silver nitrate (AgNO3) and sodium chloride (NaCl) that produces silver chloride (AgCl) as a precipitate. Once we have the balanced equation, we can use the stoichiometry of the reaction to determine the number of moles of AgCl produced, and then convert that to mass using the molar mass of AgCl.
The silver nitrate solution (AgNO3) provides the silver in silver chloride.
silver chloride
9.11 g
Silver nitrate is soluble in water but chloride and carbonate are insoluble.
42,09 g silver chloride are obtained.
The mass of silver chloride is 68,34 g.
The silver in the Silver Nitrate precipitates the chloride ions out of the ammonium chloride solution, leaving Ammonium Nitrate in solution and a Silver Chloride solid.
5
43.0287
7
Silver chloride precipitates from the solution.
If the silver nitrate and ammonium chloride are both in solution when mixed, the very sparingly soluble silver chloride precipitates as a solid, leaving ammonium nitrate in the solution.
The silver nitrate solution (AgNO3) provides the silver in silver chloride.
58.9g
silver chloride
If chloride is present silver chloride with get precipitated..
Since both chloride anions and nitrate anions have a charge of -1, there will be the same number of moles of silver chloride produced as the moles of silver nitrate reacted. (Since both silver nitrate and silver chloride are ionic compounds, it would be preferable to call their "moles" "formula units" instead.)