Chemistry
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Transcribed Image Text:Consider the insoluble compound copper(II) carbonate , CuCO3 . The copper(II) ion also forms a complex with ammonia . Write
a balanced net ionic equation to show why the solubility of CUCO3 (s) increases in the presence of ammonia and calculate the
equilibrium constant for this reaction.
2+
For Cu(NH3),* Kf= 6.8×102 . Be sure to specify states such as (aq) or (s).
K =
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- Consider the insoluble compound zinc cyanide, Zn(CN)2. The zinc ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Zn (CN)2 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Zn(NH3)4²+, K₁ = 2.9×10⁹. Be sure to specify states such as (aq) or (s). K = + Submit Answer + Retry Entire Group 1 more group attempt remainingarrow_forwardConsider the insoluble compound copper (II) carbonate, CuCO3. The copper(II) ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of CuCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3)42+, K = 6.8x1012. Be sure to specify states such as (aq) or (s). K = [Review Topics] [References] Use the References to access important values if needed for this question. Submit Answer ? + Retry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical Support Previous Email Instructor Next> Save and Exitarrow_forwardess Consider the insoluble compound silver hydroxide, AgOH. The silver ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of AgOH (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Ag(NH3)2+, Kf = 1.1×107. Be sure to specify states such as (aq) or (s). Knet + +arrow_forward
- The generic metal A forms an insoluble salt AB(s) and a complex AC, (aq). The equilibrium concentrations in a solution of AC, were found to be [A] = 0.100 M, [C] = 0.0270 M, and [AC5] = 0.100 M. Determine the formation constant, Kf, of AC5. K₁ = x100 The solubility of AB(s) in a 1.000 M solution of C(aq) is found to be 0.174 M. What is the Ksp of AB? Ksp= 6.59 x10-8arrow_forward27) Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products): (a) AgI (b) Ag2SO4 (c) Mn(OH)2 (d) Sr(OH)2·8H2O (e) the mineral brucite, Mg(OH)2arrow_forwardThe blue complex Cu(H,O);+ and the yellow complex CuCl- exist in equilibrium. Cu(H, O);+(aq) + 4 CI¯(aq) = CuCl (aq) + 4 H, O(1) Upon addition of LiCl to this equilibrium in solution, which observation would be expected? The solution turns blue. The solution turns yellow. The Cu2+ salts precipitate out of solution. The volume of water decreases. Incorrect O O Oarrow_forward
- Consider the insoluble compound zinc carbonate, ZnCO3. The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnCO3 (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Zn(OH)4²-, Kf = 2.9×10¹5. Be sure to specify states such as (aq) or (s). K = + Submit Answer + Retry Entire Group 2 more group attempts remainingarrow_forwardCalculate the solubility product, Ksp, of both compounds. Fluorite (CaF₂) is slightly water soluble and dissolves according to the following equation: Caf Ca² 2F ²(s) (aq) (aq) A saturated fluorite solution is measured as having a calcium ion concentration of 2.1 x 10 M. What is the solubility product for fluorite? /arrow_forwardWrite a balanced net ionic equation to show why the solubility of Mg(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.Be sure to specify states such as (aq) or (s). Mg(OH)2(s) + 2HCl(aq) MgCl2(aq) + 2H2O(l) K =arrow_forward
- Copper(I) ions in aqueous solution react with NH₂ (aq) according to Cu+ (aq) + 2NH₂ (aq) → Cu(NH3)2(aq) Kf6.3 x 10¹0 x Calculate the solubility (in g-L) of CuBr(s) (Ksp = 6.3 × 10%) in 0.88 M NH₂ (aq). solubility of CuBr(s):arrow_forwardConsider the insoluble compound zinc sulfide, ZnS . The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnS (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Zn(OH)4²-, Kf = 2.9×1015. Be sure to specify states such as (aq) or (s). K= + +arrow_forwardI need helparrow_forward
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