Silver chloride us very insoluble in water, and by adding a very slight excess of silver nitrate, it is possible effectively to remove all the chloride ion from the sample. First, write the balanced net ionic equation for this reaction. Then assume that a sample has a mass of 1.054 grams contains 21.5% chloride ion by mass. Then calculate the mass of silver nitrate that be used to completely precipitate all the chloride from the sample?
2007-04-25 11:34:54 · 2 answers · asked by herlots 1 in Science & Mathematics ➔ Chemistry
Ag+ + Cl- -> AgCl
mass of Cl- = .215*1.054 g = 0.2266 g
Mass of AgNO3 = 170*0.2266/35.5 = 1.085 g
2007-04-25 22:26:01 · answer #1 · answered by ag_iitkgp 7 · 0⤊ 0⤋
Molar mass of silver nitrate AgNO3 is one hundred seventy. 80 5 grams is a million/2 a mole. you receives a million/2 a mole of silver, which has atomic mass of 108, i.e. fifty 4 grams of silver. EDIT all and sundry giving this answer a thumbs down is courteously requested to STFU.
2016-12-04 21:05:26 · answer #2 · answered by ? 4 · 0⤊ 0⤋