Suppose you are studying coordination compounds of Co(II) with the ligand pyridine (py, C5H5N, MW = 79.10). You isolate a crystalline compound and since the only available ions are chloride and nitrate, you hypothesize the empirical formula of the coordinaton compound must be Co(II)w(py)x(Cl)y(NO3)z. Addition of AgNO3 to aqueous solutions of the complex results in a cloudy white precipitate, presumably AgCl. You dissolve 0.1000 g of the complex in water and perform a precipitation titration with 0.0500 M AgNO3 at the titrant. Using an electrode that is sensive to [Ag+], you reach the endpoint after 9.00 mL of titrant are added. How many grams of chloride ion were present in the 0.1000-g sample?
2007-04-21 07:12:36 · 3 answers · asked by alissa f 1 in Science & Mathematics ➔ Chemistry
(9/1000) x 0.05 x 35.5
2007-04-21 19:58:55 · answer #1 · answered by Gervald F 7 · 0⤊ 0⤋
verify what % of the molecule is H2O. If the molecular weight of BaCl2 is 208.23 grams/mole and water is eighteen then the proportion water is eighteen/(18 + 208.23) x a hundred = 7.ninety six%. So the quantity of water pushed off would be 15.0 x 7.ninety six/a hundred = a million.19 grams.
2016-12-10 07:55:22 · answer #2 · answered by nations 4 · 0⤊ 0⤋
Moles of AgNO3 = Moles of Cl- = 0.05*9 = 0.45 millimol
Thus mass of Cl- = 0.45*35.5 x 10^-3 g = 15.98 mg
2007-04-21 20:03:51 · answer #3 · answered by ag_iitkgp 7 · 0⤊ 1⤋