In aqueous solution, the Co 2+ ion forms a complex with six ammonia molecules. Write the...
In aqueous solution, the Co 2+ ion forms a complex with six ammonia molecules. Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the last step in the formation of the complex.
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![2+ (NH3] Winen hydrated co2t ,ie. [co (H2O)]²+ forum Complex with NH3 ligand then each of H₂o ligand displaced by NH3 ligand](http://img.homeworklib.com/questions/f3dc60e0-74e3-11ea-b317-af4574da5840.png?x-oss-process=image/resize,w_560)
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In aqueous solution, the Co 2+ ion forms a complex with six
ammonia molecules. Write the...
In aqueous solution the Hg ion forms a complex with four iodide anions. Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that,...
In aqueous solution the Hg ion forms a complex with four iodide anions. Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the first step in the formation of the complex. Write the First Step: First Step:
In aqueous solution the Hg ion forms a complex with four iodide anions. Write the formation constant expression for the equilibrium between the hydrated metal ion and...
In aqueous solution the Pb2+ ion forms a complex with four chloride anions. Write the formation...
In aqueous solution the Pb2+ ion forms a complex with four chloride anions. Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the first step in the formation of the complex.
In aqueous solution the Ag+ ion forms a complex with two cyanide anions. Write the formation...
In aqueous solution the Ag+ ion forms a complex with two cyanide anions. Write the formation constant expression (Kf) for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the first step in the formation of the complex.
Hello! Thank you for taking the time to help me with this question it is very challenging and eas...
Hello! Thank you for taking the time to help me with this
question it is very challenging and easy to make small mistakes
with the coefficients etc.
In aqueous solution the Ag ion forms a complex with two cyanide anions Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the last step in the formation of the complex. Write the Last Step: Last Step:...
Consider the insoluble compound cobalt(II) hydroxide, Co(OH)2.The cobalt(II) ion also forms a complex with ammonia. Write...
Consider the insoluble compound cobalt(II) hydroxide, Co(OH)2.The cobalt(II) ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of Co(OH2 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Co(NH), K-.7x10. Use the pull-down boxes to specify states such as (aq) or (s). K- 9 more group attempts remaining Retry Entire Group Submit Answer
A) Consider the insoluble compound cobalt(II) hydroxide , Co(OH)2. The cobalt(II) ion also forms a complex...
A) Consider the insoluble compound cobalt(II) hydroxide , Co(OH)2. The cobalt(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Co(OH)2(s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Co(NH3)62+, Kf = 7.7×104. Use the pull-down boxes to specify states such as (aq) or (s). _____ + _____ = _____ + _____ K = B) Consider the insoluble compound nickel(II) carbonate ,...
In an ammonia solution, the silver ion, Ag, forms the colorless, but soluble diamminesilver(I) complex ion,...
In an ammonia solution, the silver ion, Ag, forms the colorless, but soluble diamminesilver(I) complex ion, Ag(NH3)2. If ammonia is added to a solution that contains an AgCI precipitate, the solid dissolves completely. Write a net-ionic equation for the equilibrium involved and explain the shift that takes place. Choose the best answer. AgCl(s) +2 NH3(a)Ag(NH3)2 (aa) C(aq) Adding ammonia to AgCl(s) dissolves the solid by displacing chloride ions with ammonia molecules, forming a soluble complex ion Ag (a2 NH3(aq) Ag(NH32...
Consider the insoluble compound cobalt(II) carbonate , CoCO3 . The cobalt(II) ion also forms a complex with ammonia . Wr...
Consider the insoluble compound cobalt(II) carbonate , CoCO3 . The cobalt(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of CoCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Co(NH3)62+ , Kf = 1.3×105 . Use the pull-down boxes to specify states such as (aq) or (s). Knet = Consider the insoluble compound silver chloride, AgCl. The silver ion also...
Question 5: The cation, Co2+, is able to form a complex ion, [Co(SCN)4] 2–, with the...
Question 5: The cation, Co2+, is able to form a complex ion, [Co(SCN)4] 2–, with the thiocyanate anion, SCN–. (a) Write the chemical equation for the (a) Write the chemical equation for the formation of this complex ion with the corresponding expression for the formation constant, Kf, and (b) Given Kf for [Co(SCN)4] 2– = 1 x103, explain how having SCN– in solution would affect the solubility of Co(OH)2 (Ksp for Co(OH)2 = 1.3 x 10–15).
Aluminum ion in solution reacts with water to form aqueous hexaaguaaluminum ()ion. Write this reaction below,...
Aluminum ion in solution reacts with water to form aqueous hexaaguaaluminum ()ion. Write this reaction below, remember phases. Aluminum is more likely to form a hydrated complex than the other four ions remaining in solution, because of its relatively small size and high charge To separate the Group B2 ion, the solution first is made basic by adding ammonia. In the presence of this weak base the pH is adjusted to 9-10 and the group B ions form insoluble hydroxides....
In aqueous solution the Hg ion forms a complex with four iodide anions. Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the first step in the formation of the complex. Write the First Step: First Step:
In aqueous solution the Hg ion forms a complex with four iodide anions. Write the formation constant expression for the equilibrium between the hydrated metal ion and...
Hello! Thank you for taking the time to help me with this
question it is very challenging and easy to make small mistakes
with the coefficients etc.
In aqueous solution the Ag ion forms a complex with two cyanide anions Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the last step in the formation of the complex. Write the Last Step: Last Step:...
Consider the insoluble compound cobalt(II) hydroxide, Co(OH)2.The cobalt(II) ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of Co(OH2 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Co(NH), K-.7x10. Use the pull-down boxes to specify states such as (aq) or (s). K- 9 more group attempts remaining Retry Entire Group Submit Answer
In an ammonia solution, the silver ion, Ag, forms the colorless, but soluble diamminesilver(I) complex ion, Ag(NH3)2. If ammonia is added to a solution that contains an AgCI precipitate, the solid dissolves completely. Write a net-ionic equation for the equilibrium involved and explain the shift that takes place. Choose the best answer. AgCl(s) +2 NH3(a)Ag(NH3)2 (aa) C(aq) Adding ammonia to AgCl(s) dissolves the solid by displacing chloride ions with ammonia molecules, forming a soluble complex ion Ag (a2 NH3(aq) Ag(NH32...
Aluminum ion in solution reacts with water to form aqueous hexaaguaaluminum ()ion. Write this reaction below, remember phases. Aluminum is more likely to form a hydrated complex than the other four ions remaining in solution, because of its relatively small size and high charge To separate the Group B2 ion, the solution first is made basic by adding ammonia. In the presence of this weak base the pH is adjusted to 9-10 and the group B ions form insoluble hydroxides....
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