A sample is a mixture of AgNO3, CuCl2, and FeCl3. When a 1.0000- g sample of the mixture is dissolved in water and reacted with excess silver nitrate, 1.7809 g of precipitate forms. When a separate 1.0000- g sample of the mixture is treated with a reducing agent, all the metal ions in the mixture are reduced to pure metals. The total mass of pure metals produced is 0.4684 g. Calculate the mass percent of AgNO3, CuCl2, and FeCl3 in the original mixture.
Answer to relevant QuestionsThree students were asked to find the identity of the metal in a particular sulfate salt. They dissolved a 0.1472-g sample of the salt in water and treated it with excess barium chloride, resulting in the precipitation of ...List the formulas of three soluble bromide salts and three insoluble bromide salts. Do the same exercise for sulfate salts, hydroxide salts, and phosphate salts (list three soluble salts and three insoluble salts). List the ...The thallium (present as Tl2SO4) in a 9.486-g pesticide sample was precipitated as thallium(I) iodide. Calculate the mass percent of Tl2SO4 in the sample if 0.1824 g of TlI was recovered. Assign oxidation states to all atoms in each compound. a. KMnO4 b. NiO2 c. K4Fe(CN)6 (Fe only) d. (NH4)2HPO4 e. P4O6 f. Fe3O4 g. XeOF4 h. SF4 i. CO j. C6H12O6 Consider the following ionization energies for aluminum. Al(g) → Al+(g) + e- I1 = 580 kJ/mol Al+(g) → Al2+(g) + e- I2 = 1815 kJ/mol Al2+(g) → Al3+(g) + e- I3 = 2740 kJ/mol Al3+(g) → Al4+(g) + e- I4 = 11,600 kJ/ ...
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