Sulfide (S) salts are notoriously insoluble in aqueous solution. a. Calculate the molar solubility of nickel(II) sulfide in water. K„(NiS) = 3 x 10-16 b. Nickel(11) ions form a complex ion in the presence of ammonia with a formation constant (K) of 2.0 x 10*: Ni* + 6 NH, = [Ni(NH,),12+. Calculate the molar solubility of NiS in 3.0 M NH3. c. Explain any differences between the answers to parts a and b.

Sulfide (S) salts are notoriously insoluble in aqueous solution. a. Calculate the molar solubility of nickel(II) sulfide in water. K„(NiS) = 3 x 10-16 b. Nickel(11) ions form a complex ion in the presence of ammonia with a formation constant (K) of 2.0 x 10: Ni + 6 NH, = [Ni(NH,),12+. Calculate the molar solubility of NiS in 3.0 M NH3. c. Explain any differences between the answers to parts a and b.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section17.6: Equilibria Involving Complex Ions

Problem 1.3ACP: Use the formation constant of [Au(CN)2] in Appendix K to determine the equilibrium concentration of...

See similar textbooks

Similar questions

Ethylenediaminetetraacetate (EDTA4 ) is used as a complexing agent in chemical analysis with the structure shown in Fig. 21.7. Solutions of EDTA4 are used to treat heavy metal poisoning by removing the heavy metal in the form of a soluble complex ion. The complex ion virtually prevents the heavy metal ions from reacting with biochemical systems. The reaction of EDTA4 with Pb2+ is Pb2+(aq) + EDTA4(aq) iPbEDTA2(aq) K = 1.1 1018 Consider a solution with 0.010 mol of Pb(NO3)? added to 1.0 L of an aqueous solution buffered at pH = 13.00 and containing 0.050 M Na1EDTA. Does Pb(OH)2 precipitate from this solution? [Ksp for Pb(OH)2 = 1.2 1015.
The transition metals form a class of compounds called metal carbonyls, an example of which is the tetrahedral complex Ni(CO)4. Given the following thermodynamic data (at 298 K): (a) Calculate the equilibrium constant for the formation of Ni(CO)4(g) from nickel metal and CO gas. (b) Is the reaction of Ni(s) and CO(g) product- or reactant-favored at equilibrium? (c) Is the reaction more or less product-favored at higher temperatures? How could this reaction be used in the purification of nickel metal?
Five-coordinate coordination complexes are known, including [CuCl5]3 and [Ni(CN)5]3. Write the structuralformulas and identify a plausible geometry for thesecomplexes.
insoluble salt AB(s) and a complex AC5(aq). The equilibrium concentrations in a solution of AC5 were found to be [A]=0.100 M[A]=0.100 M, [C]=0.0320 M[C]=0.0320 M, and [AC5]=0.100 M[AC5]=0.100 M. Determine the formation constant, Kf, of AC5. The solubility of AB(s) in a 1.000 M solution of C(aq) is found to be 0.1520.152 M. What is the Ksp of AB?
About the Alfred warner theory of complexation charge (all are correct except Select one: 1-the neutralized ionic complex with a counter ion leading to a non ionizable complex is known to have a secondary 2- the ionized complexes of cationic or anionic charge is known to be of primary or principle valence 3- the complex geometry/ shape is not related to the coordination number 4- each metal have a number of secondary valencies known as coordination number
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 = 7.7×104 . Be sure to specify states such as (aq) or (s).
For the aqueous complex at Fe (CN)6]4-complex Kf= 1.0 x 10^35 Suppose equal volumes of 0.0062M Fe(NO2) solution and 0.10M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Fe^2+ ion. Round your answer to 2 significant digits.
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 = 7.7×104 . Be sure to specify states such as (aq) or (s). + + K =
Describe how the structures of the following can be described in terms of the simple structures types of Table 3.4 but with complex ions: K2PtCl6, [Ni(H2O)][SiF6], CsCN
In photography, unexposed silver bromide was removed from film by soaking the film in a solution of sodium thiosulfate, Na2S2O3. Silver ion, Ag+, forms a soluble complex with the thiosulfate ion, S2O3-2, that has a formula of Ag(S2O3)2-3, and the formation of the complex causes the AgBr in the film to dissolve. The formation of the complex has a Kf of 2.0 x 10^13 while the Ksp of AgBr is 5.0 x 10^-13. How many grams of AgBr will dissolve in 125 mL of 1.20 M Na2S2O3 solution?
How did conductivity help to confirm the structure of complexes?
In a solution that is 0.025 M [Cu(CN)4]3- and 0.400 M in free CN- , the concentration of Cu2+ is 6.10x10-32 M Write the equilibrium equation of the ion complex formation. Calculate the formation constant. Name the complex ion. What is the coordination number?