1. Complex ion formation: Potential, E Potential, E cell cell before adding 6 M NH 3 2+ after Cu(NH3)4 formed 2+ Use Equation (10) to calculate the residual concentration of free Cu² ion in equilibrium in the solution. Take [Ag*] = 1M. Show your calculations 2+ with Cu(NH3)4 Equation 10: E = E cell cell 0.0592 2 ● log 0.4089 V 0.8012 V [Cu²+] [Ag]²

1. Complex ion formation: Potential, E Potential, E cell cell before adding 6 M NH 3 2+ after Cu(NH3)4 formed 2+ Use Equation (10) to calculate the residual concentration of free Cu² ion in equilibrium in the solution. Take [Ag*] = 1M. Show your calculations 2+ with Cu(NH3)4 Equation 10: E = E cell cell 0.0592 2 ● log 0.4089 V 0.8012 V [Cu²+] [Ag]²

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: 5. Calculate the standard potential of the Redox reaction of Ni(CN) complex Ni(CN)2+2e → Ni(s) +…

A: The formation constant of any complex/ equillibrium constant can be expressed in terms of reaction…

Q: Which one of the following reagents is capable of reducing Cu²+(1 M) to Cu(s)? Ag(s) F^- (1 M) Ni(s)…

A: Answer:-This question is answered by using the simple concept of standard reduction potentials of…

Q: Calculate AG and K at 25°C for the reactions. a. 7H₂O + 2 Cr³+ + 3 Cl₂ ⇒ Cr₂O7²- + 6 Cl¯ + 14H+ εº…

Q: Calculate AG and K at 25°C for the reactions. 7H2O+2 Cr43 Cl2 Cr20,2- +6 Cl +14H+ e = 0.03 V a. cell…

Q: Using these metal ion/metal standard reduction potentials: Cd2+ lCd : -0.38 V ; Zn2+ lZn : -0.76 V…

Q: For the following reaction, electrons are moving from which to which? Cu(s) + Ag+(aq) >>> Cu2+(aq)…

A: Given :- Cu(s) + Ag+(aq) ----> Cu2+(aq) + Ag(s) To be determined :- Direction of flow of…

Q: Determine the equilibrium constant of the following reaction at 298 K +2Fe3+ + Sn 2FE2+ Sn4 .From…

A: According to electro chemical series, which metal has higher reduction potential, reduces itself…

Q: 1. write a chemical equation for the reaction that occurs in the ff cells Ag/ Ag+//CU^2+/cu

A: Identifying anode and cathode from the cell representation: In cell representation reaction at anode…

Q: Set up a cell that has a Mg electrode in a 1.0 M aqueous Mg2+Mg2+ solution on the left side and a Ag…

Q: Balance the following reactions by half reaction method 1) Sn(OH) 4 -2 + MnO 4 -1 =>MnO 2 + Sn(OH) 6…

Q: Write the half-reaction and calculate the electrode potential of 1. a zinc electrode in 0.0400 M…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: Does the cell voltage increase or decrease when 5 mL of 6 MNH3 was added to the half-cell containing…

A: Given : Concentration of NH3 added = 6 M Volume of NH3 solution added = 5 mL And the half cell is…

Q: Calculate the Eqalibium constant (K) with the complexation reaction, In a galvanic cell. Ammonia was…

A: The information provided describes a galvanic cell with a copper electrode and a copper ammonia…

Q: Fez++ Mn Oq- Fe3tA My2t >Fe3t + Mn2t OXO

A: Step by step solution are below

Q: Al + Cu^2+ —> Al^3+ + Cu Standard reduction potential for Cu^2+ / Cu is +0.16 V, and for Al^3+ / Al…

A: In the given cell reaction the electrode with a higher reduction potential (copper electrode) acts…

Q: 16) Balance the following reactions with respect to base using half-reaction method. Label oxidant…

A: Reaction (a): Se (s) → SeO3^2- (aq) and Cr(OH)3 (aq) → Cr (s)Step 1: Write the unbalanced…

Q: Consider the following list of possible concentration cells. Which ones listed would have a positive…

A: for the concentration cell: Standard potential of the cell (E0cell) = 0V E0Cu2+/Cu = 0.34V E0Cu2+/Cu…

Q: Balance the equation in acidic conditions. Phases are optional. equation: C,0 + MnO, Mn²+ + CO2

Q: The voltaic cell Ca(o)Ca²+ (aq) || Ni?+(1.0 M)|Ni(s) has a cell potential of 0.300 V at 25°C. What…

A: Given : Ecell = 0.300 V Temperature = 25 oC Concentration of Ni2+, [Ni2+ ] = 1.0 M And Eocell =…

Q: The free energy change for the following reaction at 25 °C, when [Pb²*] = 1.15 M and [Fe²*] =…

A: #1: In the given reaction, Fe(s) is oxidized to Fe2+(aq), whereas Pb2+(aq) is reduced to Pb(s).…

Q: r The cell potential (Ecell) is 1.80 V for a galvanic cell made using the redox couples H+/H₂ and…

Q: Considering the reaction and the information in the Excel table below, what should be entered into…

Q: 28). What statement about a galvanic cell constructed with Cu*/Cu and Fe2+/Fe is correct? Standard…

A: Given : reduction potential of Cu+/Cu reaction = 0.52 V and reduction potential of Fe2+/Fe reaction…

Concept explainers

Spectroanalytical Methods

Spectroanalytical methods measure the wavelength and intensity of radiations that are either emitted or absorbed by a molecular or atomic species. These methods are useful for evaluating the electronic or atomic arrangement of the molecules of a given analyte.

Question

1. Complex ion formation:
Potential, E before adding 6 M NH
cell
3
2+
after Cu(NH3)4
Potential, E
cell
O
Equation 10: E = E
cell
formed
2+
Use Equation (10) to calculate the residual concentration of free Cu ion in equilibrium
in the solution. Take [Ag*] = 1M. Show your calculations
2+
with Cu(NH3)
cell
0.0592
2
●
[Cu²+]
[Ag]²
0.4089 V
0.8012 V
log-

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

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

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

Eºcell calculation, reaction quotient, e cell calculation
What is E° for the cell Mn | Mn²*(aq) 2+ || Ag*(aq) | Ag?
How many Faradays are required to convert one mole of Cr₂O7-² to Cr+³?
A 100.0 mL solution of 0.0200 M Fe3+ in 1 M HClO4 is titrated with 0.100 M Cu+, resulting in the formation of Fe2+ and Cu2+. A Pt indicator electrode and a saturated Ag∣∣AgCl electrode are used to monitor the titration. Calculate the values of ? for the cell after each of the given volumes of the Cu+Cu+ titrant have been added. 10.0 ml E = ? V 19.5 ml E = ? V
The reduction potential to the metal of Ba 2+ is -1.57 V and that of Cu 2+ is +0.34 V. The cell potential for the reaction Ba(s) + Cu 2+ (aq) → Ba 2+ (aq) + Cu(s) is therefore: a. (+1.57) + (+0.34) b. (+1.57) + (-0.34) c. (-1.57) + (+0.34) d. 2 x (-1.57) + 2 x (0.34) e. (-1.57) + (0.34)
Calculate the potential at the equivalence point for titration of 0.100MFe^2+ with 0.100M Ce^4+.Given the formal potential for the reduction E^0 of Fe^3+ to Fe^2+ is +0.77V, and the formal potential for the reduction of E^0 Ce^4+ to Ce^3+ is 1.45V.
A solution prepared by mixing 60.0 mL of 0.360 M AGNO, and 60.0 mL of 0.360 M TINO, was titrated with 0.720 M NaBr in a cell containing a silver indicator electrode and a reference electrode with a constant potential of 0.175 V. The reference electrode is attached to the positive terminal of the potentiometer, and the silver electrode is attached to the negative terminal. The solubility constant of TIBr is Kp = 3.6 × 10-6 and the solubility constant of AgBr is = 5.0 x 10-13. Ksp Which precipitate forms first? O TIBI O AgBr Which of the expressions shows how the cell potential, E, depends on [Ag*]? E = 0.175 V – [0.799 V – 0.05916log ([Ag+])] 1 E = |0.799 V – 0.05916log - 0.175 V [Ag*) E = [0.799 V – 0.05916log ([Ag*]D] – 0.175 V E = 0.175 V - |0.799 V – 0.05916log [Ag* * (ল) Calculate the first and second equivalence points of the titration. first equivalence point: mL second equivalence point: mL What is the cell potential after each of the given volumes of 0.720 M NaBr have been…
What is the standard electrode potential for the reaction 2 Cr + 3 Pb2* →3 Pb + 2 Cr+? Standard Reduction E° (V) V Potentials Pb2+(aq) + 2e Pb(s) -0.13 1 4 6. Cr3+(aq) + 3e- - Cr(s) -0.74 8. 6. +/- 0. 2. 7.
Considering the reaction and the information in the Excel table below, what should be entered into cell D3 to calculate Kc? A B C D 1 Equilibrium Concentration (M) 2 Fe3+ SCN- Fe(SCN)2+ Equilibrium Constant 3 9.70E-04 1.70E-04 2.60E-05 =C3/(A3*B3)^2 =C3/(A3^2*B3) =A3*B3^2/C3 =C3/(A3*B3) =C3/(A3*B3^2)