Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride:
Ag+(aq) + Cl- (aq) -> AgCl(s)
Silver Chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25 mL or 0.366Mol AgNO3 solution to completely precipitate the silver?
2007-12-31 09:42:50 · 2 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
I think you mean 0.366M AgNO3
Note: NaCl --> Na+ + Cl-
=0.366molAgNO3/L * 0.025L * (1molCl-/1molAgNO3) * (1molNaCl/1molCl-) * (58.44gNaCl/1molNaCl)
=0.534726g NaOH needed
[Note: All units except #gNaCl cancel out]
2007-12-31 09:57:01 · answer #1 · answered by ¿ /\/ 馬 ? 7 · 1⤊ 0⤋
if reaction goes to completion then for precipation of .366mol of AgNO3 .366 moles of NaCl are required because 1mol of Ag+ ion requires 1mol Cl- ion
i.e. 21.411grams of NaCl are required
2007-12-31 10:01:15 · answer #2 · answered by Ahtisham 1 · 0⤊ 1⤋