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Chapter 4: 4.3 CYL (page 183)
Which solution could be used to precipitate barium ion Ba2+, in a water sample, Sodium chloride, sodium hydroxide, or sodium sulfate. What is the formula for the expected precipitate?
Sodium Sulfate is used to precipitate a barium ion.
The formula for the expected precipitate is BaSO4.
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Identify the atoms that are oxidized and reduced, the change in the oxidation state for each, and the oxidizing and reducing agents in each of the following equations:
(a)\(Mg\left( s \right) + NiC{l_2}\left( {aq} \right) \to MgC{l_2}\left( {aq} \right) + Ni\left( s \right)\)
(b)\(PC{l_3}\left( l \right) + C{l_2}\left( g \right) \to PC{l_5}\left( s \right)\)
(c)\({C_2}{H_4}\left( g \right) + 3{O_2}\left( g \right) \to 2C{O_2}\left( g \right) + 2{H_2}O\left( g \right)\)
(d)\(Zn\left( s \right) + {H_2}S{O_4}\left( {aq} \right) \to ZnS{O_4}\left( {aq} \right) + {H_2}\left( g \right)\)
(e) \(2{K_2}{S_2}{O_3}\left( s \right) + {I_2}\left( s \right) \to {K_2}{S_4}{O_6}\left( s \right) + 2KI\left( s \right)\)
(f) \(3Cu\left( s \right) + 8HN{O_3}\left( {aq} \right) \to 3Cu{\left( {N{O_3}} \right)_2}\left( {aq} \right) + 2NO\left( g \right) + 4{H_2}O\left( l \right)\)
Sodium bicarbonate (baking soda), NaHCO3, can be purified by dissolving it in hot water (60掳C), filtering to remove insoluble impurities, cooling to 0 掳C to precipitate solid NaHCO3 , and then filtering to remove the solid, leaving soluble impurities in solution. Any NaHCO3 that remains in solution is not recovered. The solubility of NaHCO3 in hot water of 60 掳C is 164 g/L. Its solubility in cold water of 0 掳C is 69 g/L. What is the percent yield of NaHCO3 when it is purified by this method?
What mass of Ca(OH)2 will react with 25.0 g of propionic acid to form the preservative calcium propionate according to the equation?
Uranium can be isolated from its ores by dissolving it as UO2(NO3)2, then separating it as solid UO2(C2O4). Addition of 0.4031 g of sodium oxalate, NaC2O4, to a solution containing 1.481 g of uranyl nitrate, UO2(NO3)2, yields 1.073 g of solid
\(Na{C_2}{O_4} + U{O_2}{\left( {N{O_3}} \right)_2} + 3{H_2}O \to U{O_2}\left( {{C_2}{O_4}} \right) \cdot 3{H_2}O + 2NaN{O_3}\)
What is the percent of chloride ion in a sample if 1.324g of sample produces 1.0881g of AgCl when treated with excess Ag+\(A{g^ + } + C{l^ - } \to AgCl\)
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