Unformatted text preview: to form water and another oxide of vanadium weighing 3.782 g. The second oxide was treated further with hydrogen until only 2.573 g of vanadium metal remained. (a) What are the simplest formulas of the two oxides? (b) What is the total mass of water formed in the successive reactions? 6) The term "alum" refers to a class of compounds of general formula MM*(SO 4 ) 2 . 12H 2 O, where M and M* are different metals. A 20.000-g sample of a certain alum is heated to drive off the water; the anhydrous residue weighs 11.123 g. Treatment of the residue with excess NaOH precipitates all the M* as M*(OH) 3 , which weighs 4.388 g. Calculate the molar mass of the alum and identity the two metals, M and M*. 7) 0.158 g of a barium halide is completely precipitated with H 2 SO 4 and 0.124 g of BaSO 4 is collected. What is the formula of the barium halide?...
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- Spring '09
- 1.74 g, 1.234 g, 2.573 g, 3.782 g