Chemistry, 04.05.2021 14:40 TheOneandOnly003
In a reaction vessel, 0.600 mol of Ba(NO3)2 and 0.300 mol of H3PO4 are combined with deionized water to a final volume of 2.00 L. The reaction represented below occurs: 3 Ba(NO3)2(aq) +2 H3PO4(aq) - Baz(POA)(s) + 6 HNO3(aq) (a) Calculate the mass of Ba3(PO4)2 formed. (b) Calculate the initial molarity of Ba(NO3)2 and H3PO4 (c) Calculate the molarity of the NO3 ion after the reaction reaches completion.β
Answers: 2
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Consider the reduction reactions and their equilibrium constants. cu+(aq)+eββ½βββcu(s)pb2+(aq)+2eββ½βββpb(s)fe3+(aq)+3eββ½βββfe(=6.2Γ108=4.0Γ10β5=9.3Γ10β3 cu + ( aq ) + e β β½ β β β cu ( s ) k =6.2Γ 10 8 pb 2 + ( aq ) +2 e β β½ β β β pb ( s ) k =4.0Γ 10 β 5 fe 3 + ( aq ) +3 e β β½ β β β fe ( s ) k =9.3Γ 10 β 3 arrange these ions from strongest to weakest oxidizing agent.
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In a reaction vessel, 0.600 mol of Ba(NO3)2 and 0.300 mol of H3PO4 are combined with deionized water...
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