Pls pls provide the right answer w.com/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take[References]A solution is prepared by adding 0.19 mole of Ni(NH3). Cl2 to 0.50 L of 3.9 M NH3. Calculate Ni (NH3),* and Ni²+in this solution. Koverallfor Ni (NH3)+ is 5.5 x 10°. That is,[NI(NH,),2+5.5 x 108 =for the overall reactionNi?+ (aq) + 6NH3 (aq) = Ni(NH3)6* (ag)%3D[N*] =[MTry Another Version3 item attempts remainingSubmit Answer4:44 PM3/30/20search远

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A solution is prepared by adding 0.19 mole of Ni(NH3), Cl2 to 0.50 L of 3.9 M NH3. Calculate Ni (NH3),*| and Ni?+ for Ni (NH3),+ is 5.5 x 10$. That is, in this solution. Koverall Ni(NH,), [N²-] INH" 5.5 x 108 = for the overall reaction Ni2+ (ag) + 6NH3 (aq) = Ni(NH3),* (ag) [NI(NH,),]-C 2+ M [N*]-C M 3 item attempts remaining Submit Answer Try Another Version

A solution is prepared by adding 0.19 mole of Ni(NH3), Cl2 to 0.50 L of 3.9 M NH3. Calculate Ni (NH3),| and Ni?+ for Ni (NH3),+ is 5.5 x 10$. That is, in this solution. Koverall Ni(NH,), [N²-] INH" 5.5 x 108 = for the overall reaction Ni2+ (ag) + 6NH3 (aq) = Ni(NH3), (ag) [NI(NH,),]-C 2+ M [N*]-C M 3 item attempts remaining Submit Answer Try Another Version

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter21: Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 21.199QP

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A 0.7336-g sample of an alloy that contains copper and zinc is dissolved in 8 M HCl and diluted to 100 mL in a volumetric flask. In one analysis, the zinc (At. Mass = 65.38 g/mol) in a 25.00-mL portion of the solution is precipitated as ZnNH4PO4, and isolated as Zn2P2O7 (FM = 304.70g/mol), yielding 0.1163 g. The copper (At. Mass = 63.55 g/mol) in a separate 25.00-mL portion of the solution is treated to precipitate CuSCN (121.63 g/mol), yielding 0.2383 g. Calculate the %w/w Zn and the %w/w Cu in the sample.
Suppose 0.010 mol of each of the following compounds isdissolved (separately) in 1.0 L water: BaCl2, K4[Fe(CN)6],[Cr(NH3)4Cl2]Cl, [Fe(NH3)3Cl3]. Rank the resulting four solutions in order of conductivity, from lowest to highest.
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