In the presence of CN", Fe3+ forms the complex ion Fe(CN)63- Theequilibrium concentrations of Fe3+ and Fe(CN)63- are 8.5 × 10¬40 M and1.4 x 10-3 M, respectively, in a 0.12 M KCN solution. Calculate the valuefor the overall formation constant of Fe(CN)63-.Fe"(aq) + 6CN (aq) → Fe(CN)63-K =

Given :- [Fe3+] = 8.5 × 10-40 M [Fe(CN)6]3- = 1.4 × 10-3 M [CN]- = 0.12M

In the presence of CN", Fe3+ forms the complex ion Fe(CN)63-. The equilibrium concentrations of Fe3+ and Fe(CN)63- are 8.5 x 10-40 M and 1.4 x 10-3 M, respectively, in a 0.12 M KCN solution. Calculate the value for the overall formation constant of Fe(CN)63-. Fe3*(aq) + 6CN (aq) → Fe(CN)63- K=

In the presence of CN", Fe3+ forms the complex ion Fe(CN)63-. The equilibrium concentrations of Fe3+ and Fe(CN)63- are 8.5 x 10-40 M and 1.4 x 10-3 M, respectively, in a 0.12 M KCN solution. Calculate the value for the overall formation constant of Fe(CN)63-. Fe3*(aq) + 6CN (aq) → Fe(CN)63- K=

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: The fictitious complex M(SCN)2 can be produced from an aqueous equilibrium in which the M2+ ion is…

Q: For cobalt(II) arsenate, calculate the molar solubility, concentrations of constituent ions, and…

A: Given information: Ksp for Co3(AsO4)2 = 7.6 x 10-29

Q: 4. A solution at 25°C is prepared in which a very small amount of Fe2+ is added to a much larger…

Q: What is the solubility product constant expression or designation for Gold (III) hydroxide? Ksp =…

Q: The Kf for the dicyanosilver complex ion, [Ag(CN)2]-, is 5.6 x 1018. When solid NaCN is added to a…

A: Given [AgNO3] = 0.010 M [CN-] = 0.5 M Kf of [Ag(CN)2]- = 5.6*1018

Q: The fictitious complex M(SCN)2 can be produced from an aqueous equilibrium in which the M2+ ion is…

A: Since the reaction taking place will be M2+ + 2 SCN- ----> M(SCN)2 hence from the above…

Q: QUESTION 7 A solution is prepared such that the initial concentration of A2+ is 1.50x10-3 M and the…

A: Given: The initial concentration of A2+ and X is 1.50×10-3 M and 4.60×10-3 M, respectively. The…

Q: + In aqueous solution the Ag ion forms a complex with two ammonia molecules. Write the formation…

A: ( If you have any queries please feel free to ask me).

Q: When AgCl(s) is dissolved in a solution of NH3, the complex ion Ag(NH3)2+ forms as shown in the…

A: we need to calculate Kf for Ag(NH3)2+

Q: Sufficient sodium cyanide,NaCN , was added to 1.5X10^-2 M silver nitrate,AgNO3 , to give a…

A: Given: Molarity of AgNO3 = 1.5×10−2 M Molarity of CN− ion = 0.229 M Kf for Ag(CN)2− = 5.6×1018

Q: The generic metal A forms an insoluble salt AB(s) and a complex AC5(aq). The equilibrium…

A: Given [A] = 0.100 M[C] = 0.0220 M[AC5] = 0.100 M Kf for AC5 = To be determined

Q: 2+ In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoC142.…

A: Step 1: As we see the product of the reaction is pink colour Cobalt ions , so pink colour is…

Q: A solution is prepared such that the initial concentration of A2+ is 1.50×10-3 M and the initial…

A: The equilibrium constant of a reaction is the ratio between the product's concentration to the…

Q: In aqueous solution the A1³+ ion forms a complex with six fluoride anions. Write the formation…

Q: Sufficient sodium cyanide, N&CN, was added to 1.0 x 10- M silver nitrate, AGNO3, to give a solution…

A: Given that, concentration of AgNO3= 1.0×10-2 M = 0.01 M The NaCN and AgNO3 solution react to form a…

Q: Consider the insoluble compound iron(II) sulfide , FeS . The iron(II) ion also forms a complex with…

Q: Consider the insoluble compound silver bromide, AgBr. The silver ion also forms a complex with…

A: We need to write the equilibrium reactions for the dissolution of AgBr(s) in pure water and in…

Q: Express the equilibrium constant for the following reaction. O O N2(g) + 3H2(g) ⇒ 2NH3(g) K = K = K…

Q: One millimole of Ni(NO3)2 dissolves in 250.0 mL of a solution that is 0.500 M in ammonia. The…

A: The balanced Chemical reaction for given numerical is The formation constant for the reaction is…

Q: The formation constant* of [M(CN)2]¯ is 5.30 × 10'8, where M is a generic metal. A 0.150 mole…

A: Given, [M(CN)2]- M+ + 2CN- ---> [M(CN)2]- Formation constant, Kf = 5.30 x 1018 Kf = [M(CN)2]- /…

Q: What is the equilibrium molar concentration of Cu+ in a solution prepared by adding 0.1558 mol of…

A: The reaction is as follows Cu+(aq) + 2CN-(aq) [Cu(CN)2]-(aq)

Q: Given that the value of Kc is 199.90, calculate the equilibrium concentrations of Fe+3 and SCN- if…

A: Well, First we need to reverse the reaction so that construction of ICE table will be easy. Kc for…

Q: Consider

A: Considering the reaction: Ag+ + 2 NH3 = Ag(NH3)2+

Q: What is the concentration of free Ag+(aq) in a solution that is initially 0.01254 M in AgNO3 and…

A: · Concentration of AgNO3 = 0.01254 M· Concentration of NH3 = 1.04842 M· Kf of AgNH32+ = 1.600×107

Q: For the aqueous [Ni(CN)4] complex K, = 2.00 × 1031 at 25 °C. Suppose equal volumes of 0.0092 M Ni…

A: A complex ion is formed when a metal ion and a ligand react. The reaction is a Lewis acid-base…

Q: Oxalate, C2O42-, forms a complex ion with manganese(II) ion, Mn2+, as shown in the following…

A: Given: Concentration of Mn(NO3)2 = 0.011 M Volume of Mn(NO3)2 = 4500 mL Concentration of Na2C2O4 =…

Q: The ion Hg2+reacts with chloride ions to make the complex HgCl4 2- , which has a Kf = 1.1x1016. In a…

A: The complexation reaction can be represented as: Hg2++4Cl-→HgCl4-2

Q: . You determined the equilbrium constant, K eq^ prime for the reaction using a number of different…

A: K'eq. means equilibrium for the reverse reaction. It is equal to reverse of equilibrium constant.…

Q: Co(NH,), complex K,= 1.58 × 10 at 25 °C. For the aqueous %3D Suppose equal volumes of 0.0028M…

A: As Equal volume are taken Concentration of Co(NO3)3 = 0.0028 M2 = [Co3+]Concentration of Co(NO3)3…

Q: Consider the following reaction 4Fe(s) + 3O2(g) = 2Fe2O3(s). If 2.0 moles of Fe, 0.01 miles oxygen…

A: 4Fe(s) + 3O2(g) =…

Q: iClicker: To 120.0 ml 2.8 x 10-3 M AgNO3 solution 0.030 mol solid NaCN is added. What is the…

A: The reaction that occurs when NaCN is added to solution can be represented as follows:

Q: 6. In an experiment, pH meters were created using indicators and the pH value was found to be 11 for…

A: The dissociation constant of a base gives measure of the strength of the base. More the value of…

Q: Lead (II) fluoride has a Ksp value of 2.7x10-8. What is the concentration of Pb2+ and F- ions in a…

A: The solubility product constant (Ksp) describes the equilibrium between a solid and its constituent…

Q: 3. Complex ion formation. Calculate the equilibrium concentration of Ag+(aq) in a solution that is…

A: We have find out the answer

Q: One millimole of Ni(NO3)2 dissolves in 240.0 mL of a solution that is 0.500 M in ammonia. The…

A: we need to calculate initial concentration of Ni(NO3)2 equilibrium concentration of Ni2+(aq )

Q: (a) The formation constant, K,, of Ni(CN)2(aq) Ni²+ (aq) + 4 CN- (aq) = Ni(CN)²(aq) is 2.1 x 10³¹.…

A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: buse the value of the equilibrium constant you calculated in part a to calculate the solubility (in…

A: Ksp value for Cu(OH)2 = 1.6 10-19Overall formation constant for Cu(NH3)42+) ,Kf = 1.01013The given…

Q: [Fe(CN),] complex K, = 1.0 × 105 For the aqueous at 25 °C. Suppose equal volumes of 0.0090M Fe(NO,)…

Q: Sufficient sodium cyanide, NaCN, was added to 2.5x10^-2 M silver nitrate, AgNO3, to give a solution…

A: Given: Molarity of AgNO3 = 2.5×10-2 MMolarity of CN- ion = 0.193 MKf for Ag(CN)2- = 5.6×1018

Q: Write a balanced net ionic equation to show why the solubility of Fe(OH)3(s) increases in the…

A: The dissociation reaction for Fe(OH)3 is shown below, Fe(OH)3(s) →Fe3+(aq) + 3OH-(aq)

Q: For the aqueous [Hgl, complex K,= 6.76 x 1029 at 25 °C. Suppose equal volumes of 0.0098 M Hg(NO,)…

A: After mixing equal volume of Hg(NO3)2 and KIConcentration of Hg(NO3)2 = 0.0098 M2 = 0.0049 M = [Hg2+…

Q: 2. Given that KspNi(OH)2] = 5.50 x 10-16, Ksp[Mg(OH)2] = 8.9 x 10-12, and Ksp[Ca(OH)2] = 4.7 x 10-4,…

A: correct option [c] Ni(OH)2⇌Ni+2 + 2OH- Ksp=[Ni+2]× [OH-]2 Given Ksp=5.50×10-16Let [Ni+2]…

Q: To 200.0 ml of a solution of Al(NO3)3 with concentration (1.000x10^-3) mol L-1, (3.0x10^2) ml of…

A: Step 1:Given information:Initial volume of Al(NO₃)₃ solution = 200 mL = 0.2 LConcentration of…

Q: The copper(II) ion reacts with phosphate ion to form an insoluble ionic compound, Ksp = 1.40×10-37.…

Q: A solution is prepared such that the initial concentration of A2+ is 1.50×10-3 M and the initial…

Question

100%

In the presence of CN", Fe3+ forms the complex ion Fe(CN)63- The
equilibrium concentrations of Fe3+ and Fe(CN)63- are 8.5 × 10¬40 M and
1.4 x 10-3 M, respectively, in a 0.12 M KCN solution. Calculate the value
for the overall formation constant of Fe(CN)63-.
Fe"(aq) + 6CN (aq) → Fe(CN)63-
K =

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Equilibrium Concepts in Analytical Chemistry

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

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] = 0.0320 M, and [AC5] = 0.100 M. Determine the formation constant, Kf, of AC5. Kf= 5.108 x10-8 Incorrect The solubility of AB(s) in a 1.000 M solution of C(aq) is found to be 0.104 M. What is the Ksp of AB? Ksp = 1.0816 x10-1 Incorrect
What is the approximate concentration of free Ag+ ion at equilibrium when 1.36x10-² mol silver nitrate is added to 1.00 L of solution that is 1.100 M in CN. For [Ag (CN)₂], Kf = = 1.3x1021 [Ag+] = M
Show the effect of complex ion formation on solubility. Consider the insoluble compound silver chloride, AgCl. The silver ion also forms a complex with cyanide ions. Write a net ionic equation to show why the solubility of AgCl(s) increases in the presence of cyanide and calculate the equilibrium constant for this reaction. Solubility product constant data is found in the Chemistry References. For Ag(CN)₂, Kf = 1.3x1021. Be sure to specify states such as (aq) or (s). K = + ? +
I performed an experiment where I mixed KSCN with Fe(NO3)3 and diluted the solution with water. Equation: Fe + SCN <> Fe(SCN)3+ (1) use Le Châtelier's Principle and the “fill in the blank” format provided to explain the effect the added reagent has on the [Fe(SCN)]2+(aq) equilibrium. If an secondary equilibrium is present, support your answer by providing the appropriate balanced net ionic secondary equilibria. How does the addition of NaOH(aq) affect the equilibrium position for reaction (1)? The __________ added will react with the free __________ in solution forming __________, momentarily causing the concentration of __________ to __________. The primary equilibrium will shift __________, restoring Keq by replacing the __________. This shift will result in a(n) __________ in the concentration of __________ causing the color intensity of the solution to __________. Balanced secondary equilibrium:
Write the equilibrium reactions for the formation per step of the Fe complex (CN)6^3- from Fe^3(ac) and CN -(ac) . Write the expression of the training constants for each step and the total training constant of the complex.
Which of the following is the correct Kf expression for the formation of the complex ion tetraiodoplumbate(II) ion, [PbI4]2–? Pb2+ (aq) + 4 I1- (aq) < === > [PbI4]2– (aq) Kf = [PbI4]2– / {[Pb2+] [4 I1-]} Kf = {[Pb2+] 4[I1-]} / [PbI4]2– Kf = {[Pb2+] [I1-]4} / [PbI4]2– Kf = [PbI4]2– / {[Pb2+] [I1-]4}
1. When thallium chloride dissolves in water and forms a saturated solution, it establishes the TI* (aq) + Cl (aq) The solubility of TICI is 0.29 g/ 100 mL solution at 15.6 equilibrium, TICI(s) Celcius. Calculate the molar solubility of each ion at equilibrium. Calculate the Ksp for TICI at this temperature.
I need help with question 15?
Pleaseeeeeeeee explain
Which of the following is more likely to precipitate the hydorxide ion?(a) Cu(OH)2(s) = Cu2+(aq) + 2OH-(aq) K = 1.6 x 10-19 (a) Ca(OH)2(s) = Ca2+(aq) + 2OH-(aq) K = 7.9 x 10-6
what is the molar concentration of Ni³⁺ at equilibrium when 0.15 moles Ni³⁺ is mixed with 1.12 moles NH₃ in 100 mL total volume of solution. Kf Ni(NH₃)₆³⁺ = 9.0 x 10
11. An aqueous solution is made by dissolving 1.1 x 10-³ moles of Zn(NO3)2 and 0.150 moles of NH3 in water to make 1.00 L solution. After the aqueous solution reaches equilibrium, what is the concentration of free Zn²+ (aq) ions? 724