Silver is found as Ag2S (Ksp = 6x10-51) in the ore argentite. Given the formation constant...
Silver is found as Ag2S (Ksp = 6x10-51) in the ore argentite. Given the formation constant of silver cyanide
complex Ag(CN) - as 1.0x1021, determine the following: 2
-
(a) The equilibrium constant for the cyanidation of Ag S to Ag(CN) . 2 2- Answer:K=6x10^(-9)
-
(b) Would cyanidation be a practical means of leaching silver from argentite ore? Answer: K<<1; Cyanidation is not practical
-
(c) Silver is found as AgCl in horn silver ore. Determine the equilibrium constant for the cyanidation of AgCl. Answer: K=2x10^(11)
-
(d) Would cyanidation be a practical means of leaching silver from horn silver? Answer: K>>1; Cyanidation could be practical
I have the answer to these problems I just need an explanation on how to get to those answers. Thank you!
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Silver is found as Ag2S (Ksp = 6x10-51) in the ore argentite.
Given the formation constant...
The "insoluble" salt, silver sulfide, has a solubility product, Ksp=6.3*10^-51 at 298 K. Ag2S(s)=2Ag+ (aq)+ S2-(aq)...
The "insoluble" salt, silver sulfide, has a solubility product, Ksp=6.3*10^-51 at 298 K. Ag2S(s)=2Ag+ (aq)+ S2-(aq) What is the concentration of Ag+ at equilibrium, at this temperature?
(20 marks) 5. Consider Agl(s), Ksp -8.3x10-17 a) Calculate the molar solubility of Agl in pure wa...
(20 marks) 5. Consider Agl(s), Ksp -8.3x10-17 a) Calculate the molar solubility of Agl in pure water. b) Considering the complex formation constant K 1.0x1021 for [Ag(CN)2], calculate the equilibrium constant for the reaction: Agl(s) + 2 CN (aq)[Ag(CN2] (aq) + I'(aq) c) Calculate the molar solubility of Agl in a 0.100 M NaCN solution.
(20 marks) 5. Consider Agl(s), Ksp -8.3x10-17 a) Calculate the molar solubility of Agl in pure water. b) Considering the complex formation constant K 1.0x1021...
1) A solution that is 500 molar HCN, K.-6.2 x 10-10 is in equilibrium with solid...
1) A solution that is 500 molar HCN, K.-6.2 x 10-10 is in equilibrium with solid silver (1) cyanide, Ksp - 2.2 x 10. However, it is known that silver (I), Ag'. can complex under certain conditions with CN to produce the silver (1) dicyano complex, Ag(CN)2] . log Kr - 20.48. What are all of the equilibrium reactions that are occurring in this solution? Is there a single overall reaction that can describe the equilibria in this solution?
When species combine to produce a coordination complex, the equilibrium constant for the reaction is called...
When species combine to produce a coordination complex, the equilibrium constant for the reaction is called is the formation constant, Kf. For example, the iron(II) ion, Fe2+, can combine with the cyanide ion, CN−, to form the complex [Fe(CN)6]4− according to the equation Fe2+(aq)+6CN−(aq)⇌[Fe(CN)6]4−(aq) where Kf=4.21×1045. This reaction is what makes cyanide so toxic to human beings and other animals. The cyanide ion binds to the iron that red blood cells use to carry oxygen around the body, thus interfering...
please help!! We were unable to transcribe this imageConsider the insoluble compound silver hydroxide, AgOH.The silver...
please help!!
We were unable to transcribe this imageConsider 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* K = 1.1*10'. Use the pull-down boxes to specify states such as (aq) or (s). Knet = Consider the insoluble compound iron(II) hydroxide. Fe(OH)2. The iron(II) ion also...
Commercial silver plating operations frequently use a solution containing the complex |Ag(CN)_2] ion. Because the formation...
Commercial silver plating operations frequently use a solution containing the complex |Ag(CN)_2] ion. Because the formation constant K_f is quite large, this procedure ensures that the free Ag+ concentration in solution is low to promote uniform electrodeposition. In one process, a chemist added 9.0 L of 1.1M NaCN to 90.0 L of 0.12 M AgN0_3. Calculate the concentration of free Ag+ ions at equilibrium. K_f for this reaction is 1.0 times 10^21. Enter your answer in scientific notation.
Given the following reactions, AgBr(s) = Ag+ (aq) + Br(aq) Ksp = 5.8 x 10-13 Ag+...
Given the following reactions, AgBr(s) = Ag+ (aq) + Br(aq) Ksp = 5.8 x 10-13 Ag+ (aq) + 2 CN"(aq) = Ag(CN)2(aq) Kf = 9.5 x 1021 determine the equilibrium constant for the reaction below. AgBr(s) + 2 CN"(aq) =Ag(CN)2(aq) + Br(aq) Answer: 1.2E21 Check
The reaction for the formation of the diamine-silver son is as follows: A® LÀ NHÀ ANH...
The reaction for the formation of the diamine-silver son is as follows: A® LÀ NHÀ ANH Nha La Write the equilibrium constant expression for this reaction b. An experiment was carried out to determine the value of the equilibrium constant for the shove reaction Show ICE table Total moles of Ag present Total Moles of NH, present Measured AgNH,) a equilibrium Total solution Volume 3.6 x 10 moles 6.9 x 10 moles 3.4 x 10- moles 100 ml i Calculate...
I need help with the formation constant (Kf) in question 3 at the bottom. anything else...
I need help with the formation constant (Kf) in question 3 at
the bottom. anything else you might catch would be greatly
appreciated as wel ?
Please refer to the 'CALCULATIONS' section for help filling in the ponowing uvie. Equilibrium Concentrations anal Initial Concentrations (after mixing."before" rxn) [Fe3+ (SCN) (FeNCS2+1 | [Fe3+] [SCN) (sve question 2) 0.0bolcom/0.colum Tube 1 10.100M 1 (C) 10.ol 1o. oloom/0.000loom 6.43.10" 0.0099 3.65 1.560 Tube 3 |0.00 50omo.coolcom 4.85x100 .00495 5 1.03.10 Tube 4 16.002.500.oooloom...
QUESTION 5 Consider the formation of solid silver chloride from aqueous silver and chloride ions. Given...
QUESTION 5
Consider the formation of solid silver chloride from aqueous
silver and chloride ions.
Given the following table of thermodynamic data at 298 K:
The value of K for the reaction at 25 °C is ________.
a)
1.8 × 104
b)
3.7 × 1010
c)
1.9 × 10-10
d)
810
e)
5.3 × 109
QUESTION 6
Consider the reaction:
NH 3 (g) + HCl (g) → NH 4Cl (s)
Given the following table of thermodynamic data,
...
(20 marks) 5. Consider Agl(s), Ksp -8.3x10-17 a) Calculate the molar solubility of Agl in pure water. b) Considering the complex formation constant K 1.0x1021 for [Ag(CN)2], calculate the equilibrium constant for the reaction: Agl(s) + 2 CN (aq)[Ag(CN2] (aq) + I'(aq) c) Calculate the molar solubility of Agl in a 0.100 M NaCN solution.
(20 marks) 5. Consider Agl(s), Ksp -8.3x10-17 a) Calculate the molar solubility of Agl in pure water. b) Considering the complex formation constant K 1.0x1021...
1) A solution that is 500 molar HCN, K.-6.2 x 10-10 is in equilibrium with solid silver (1) cyanide, Ksp - 2.2 x 10. However, it is known that silver (I), Ag'. can complex under certain conditions with CN to produce the silver (1) dicyano complex, Ag(CN)2] . log Kr - 20.48. What are all of the equilibrium reactions that are occurring in this solution? Is there a single overall reaction that can describe the equilibria in this solution?
please help!!
We were unable to transcribe this imageConsider 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* K = 1.1*10'. Use the pull-down boxes to specify states such as (aq) or (s). Knet = Consider the insoluble compound iron(II) hydroxide. Fe(OH)2. The iron(II) ion also...
Commercial silver plating operations frequently use a solution containing the complex |Ag(CN)_2] ion. Because the formation constant K_f is quite large, this procedure ensures that the free Ag+ concentration in solution is low to promote uniform electrodeposition. In one process, a chemist added 9.0 L of 1.1M NaCN to 90.0 L of 0.12 M AgN0_3. Calculate the concentration of free Ag+ ions at equilibrium. K_f for this reaction is 1.0 times 10^21. Enter your answer in scientific notation.
Given the following reactions, AgBr(s) = Ag+ (aq) + Br(aq) Ksp = 5.8 x 10-13 Ag+ (aq) + 2 CN"(aq) = Ag(CN)2(aq) Kf = 9.5 x 1021 determine the equilibrium constant for the reaction below. AgBr(s) + 2 CN"(aq) =Ag(CN)2(aq) + Br(aq) Answer: 1.2E21 Check
The reaction for the formation of the diamine-silver son is as follows: A® LÀ NHÀ ANH Nha La Write the equilibrium constant expression for this reaction b. An experiment was carried out to determine the value of the equilibrium constant for the shove reaction Show ICE table Total moles of Ag present Total Moles of NH, present Measured AgNH,) a equilibrium Total solution Volume 3.6 x 10 moles 6.9 x 10 moles 3.4 x 10- moles 100 ml i Calculate...
I need help with the formation constant (Kf) in question 3 at
the bottom. anything else you might catch would be greatly
appreciated as wel ?
Please refer to the 'CALCULATIONS' section for help filling in the ponowing uvie. Equilibrium Concentrations anal Initial Concentrations (after mixing."before" rxn) [Fe3+ (SCN) (FeNCS2+1 | [Fe3+] [SCN) (sve question 2) 0.0bolcom/0.colum Tube 1 10.100M 1 (C) 10.ol 1o. oloom/0.000loom 6.43.10" 0.0099 3.65 1.560 Tube 3 |0.00 50omo.coolcom 4.85x100 .00495 5 1.03.10 Tube 4 16.002.500.oooloom...
QUESTION 5
Consider the formation of solid silver chloride from aqueous
silver and chloride ions.
Given the following table of thermodynamic data at 298 K:
The value of K for the reaction at 25 °C is ________.
a)
1.8 × 104
b)
3.7 × 1010
c)
1.9 × 10-10
d)
810
e)
5.3 × 109
QUESTION 6
Consider the reaction:
NH 3 (g) + HCl (g) → NH 4Cl (s)
Given the following table of thermodynamic data,
...
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