0.9 g Cl^- metal ion excess AgNO3 1.6 g AgCl mass percent

0.9 g Cl^- metal ion excess AgNO3 1.6 g AgCl mass percent

 

 

What is the percent by mass of Cl in original compound

given the 0.9 g sample of ionic compound containing

chloride ions and unknown metal is dissolved in water

and treated with an excess of AgNO3

if 1.6 g of AgCl precipitate forms?

 

 

What is the percent of chloride in a sample

if 0.9 g of the sample produces 1.6 g of AgCl

when treated with excess AgNO3?

Ag = 107.9, Cl = 35.5

 

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AgCl의 몰질량 = 143.4 g/mol 이므로,

( AgCl의 몰질량 = 143.3212 g/mol )

 

1.6 g / (143.4 g/mol) = 0.01116 mol AgCl

( 참고: n=W/M https://ywpop.tistory.com/7738 )

 

 

 

Ag^+(aq) + Cl^-(aq) → AgCl(s)

 

AgCl : Cl^- = 1 : 1 계수비(= 몰수비) 이므로,

Cl^-의 몰수 = 0.01116 mol

 

0.01116 mol × (35.5 g/mol) = 0.396 g Cl^-

 

 

 

(0.396 / 0.9) × 100 = 44%

 

 

 

답: 44%