The potential of the following voltaic cell is 0.490 V. Given this information, determine the Kb for the organic base (RNH₂) dissolved in the left cell.Cell notation:\[ \text{Pt (s)} \mid \text{H}_2 (\text{g}) (0.85 \text{ atm}) \mid \text{RNH}_2 (\text{aq}) (0.10 \text{ M}), \text{RNH}_3\text{Cl} (\text{aq}) (0.050 \text{ M}) \parallel \text{SHE} \]Table of standard electrode potentials:\[\begin{array}{|c|c|}\hline\text{Half-reaction} & E^\circ (\text{V}) \\\hline2 \text{H}^+ (\text{aq}) + 2 \text{e}^- \rightleftharpoons \text{H}_2 (\text{g}) & 0.000 \\\hline\text{Hg}_2\text{Cl}_2 (\text{s}) + 2 \text{e}^- \rightleftharpoons 2 \text{Hg} (\text{l}) + 2 \text{Cl}^- (\text{aq}) & 0.268 \\\hline\end{array}\] The goal is to determine the base dissociation constant, \(K_b\), for the organic base \( \text{RNH}_2 \).

Ecell=Ecathode-Eanode0.490 V=EH+/H2-ERNH2/RNH3Cl0.490 = 0-EanodeEanode=-0.49 VThus, Since Ecell is related to pH as:Ecell=-0.059 pHSo,pH=-0.49 -0.059=8.3 Since,pH+pOH=14pOH=(14-8.3)pOH=5.7 The dissociation equilibrium of the base RNH2 can be written as: RNH2+H2O→RNH3++OH-Dissociation constant:Kb=[RNH3+][OH-][RNH2] Since, pOH=5.7=-log [OH-] [OH-]=1.99×10-6 Thus, the dissociation constant of the base: Kb=[RNH3+][OH-][RNH2] Kb=0.050×1.99×10-60.10Kb=9.95×10-7

Science

Chemistry

The potential of the following voltaic cell is 0.490 V. Given this information, determine the Kb for the organic base (RNH2) dissolved in the left cell. Pt (s) | H2 (g) (0.85 atm) | RNH2 (aq) (0.10 M), RNH;Cl (aq) (0.050 M) || SHE

The potential of the following voltaic cell is 0.490 V. Given this information, determine the Kb for the organic base (RNH2) dissolved in the left cell. Pt (s) | H2 (g) (0.85 atm) | RNH2 (aq) (0.10 M), RNH;Cl (aq) (0.050 M) || SHE

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: What is the cell potential of the following voltaic cell at 25°C?…

Q: Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at…

Q: Enter your answer in the provided box. of the following cell is 0.835 V, what is the pH in the anode…

A: To find pH

Q: Sketch the voltaic cell represented by this notation. You must include labels for the anode,…

A: We have to sketch the voltaic cell represented by this notation. You must include labels for the…

Q: The following galvanic cell is constructed at 273 K. Each aqueous phase reactant and product has a…

A: graphite(s) | X2 (g) | XO4- , H+ || YO3-, YO2- , H+ | graphite(s)

Q: For the cell reaction, Zn(s) | Zn2+(aq, 1 M) || Cu2+(aq, 1 M) | Cu(s), the electrode potential of…

A: In the given question we have to calculate the cell potential. cell Reaction, Zn(s) + Cu2+(aq)…

Q: The standard reduction potential of the Pb2+/Pb electrode is -0.13 V and the standard cell potential…

Q: What is the correct cell notation for the reaction 2Cr(s) + 3Cl₂(g) -> 2Cr³+ (aq) + 6Cl¯(aq)? Pt(s)…

A: Rules of electrochemical cell notation1. The anode (negative electrode) is written on the left hand…

Q: Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at…

A: Given that, an electrochemical cell is Cus|Cu2+0.11 M||Fe2+0.0063 M|Fes. Also, the standard…

Q: (a) Draw a schematic representation of the galvanic (electrochemical) cell that is described by the…

A: A galvanic cell is defined as the electrochemical cell which converts chemical energy into…

Q: Consider the following reaction and its AG° at 25.00 °C. Fe2+ (aq)+Zn(s) → Fe(s) + Zn²*(aq) AG° =…

Q: Using these metal ion/metal standard reduction potentials: Cd2+ (aq)|Cd(s): -0.41 V; Zn²+ (aq)…

Q: The following reaction occurs in a galvanic cell. What is the shorthand notation of this cell?…

A: It is based on the concept of electrochemical cell Here we are required to write the…

Q: For the following cell reaction, the standard cell potential is 1.34 V. To determine the cell…

A: The answer is n = 10. See solution below: Half cell reactions: Oxidation: 5 H2SO3 + 5 H20 => 5…

Q: What are the overall cell reaction and the cell potential for this voltaic cell? Mg(s)|Mg+ (aq) ||…

Q: Consider the following electrochemical cell:…

A: In electrochemical cell redox reaction occur

Q: For the cell shown, the measured cell potential, ?cell, is −0.3553 V at 25 °C. Pt(s) |…

Q: A) Write half-reactions and overall cell reaction for the following cell: Zn(s)| Zn?* (aq) ||…

A: Half Cell Reaction is the way of writing both oxidation and reduction half part of the reaction and…

Q: An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag+| = 1.0…

A: Since Ag+(aq) has a higher reduction potential, Ag+(aq) will undergo reduction to Ag(s) and act as…

Q: The following voltaic cell is made: Sn(s) | Sn2(aq) II Fe*2(aq) | Fe(s) The tin electrode is placed…

Q: What is the cell reaction for the following voltaic cell? Al(s) | Al3+(aq) || Cl2(g) | Cl–(aq) |…

A: First of all, we will write both half-cell reactions and then, on adding them we will get the…

Q: Fe(s) | Fe2+(aq) (0.325 M) || Ag+(aq) (0.150 M) | Ag(s) Calculate E°cell. In which direction do the…

A: Given -> Fe(s)/Fe2+(aq)(0.325M)//Ag+(aq)(0.150M)/Ag(s)

Q: Enter the anode reaction for the voltaic cells Al(s)|Al^3+(aq)||Cd^2+(aq)|Cd(s) . Enter the…

A: For a given cell representation anode is written on the left hand side and cathode is written at the…

Q: Using these metal ion/metal standard reduction potentials: Cd2+ (aq)| Cd(s): -0.36 V; Zn2+ (aq)|…

A: The standard half cell reactions are Cu+2 (aq)+ 2 e− ⇌ Cu (s) E° = 0.29 V Cd+2 (aq)+ 2 e− ⇌…

Q: Consider the following galvanic cell: Li (s) | 0.095M LICI (aq) || 0.032M Sn(NO3)2 (aq) | Sn (s)…

A: E°cell indicates standard potential value but Ecell indicates potential value at given conditions.…

Q: (b) Fe(s) | Fe²*(aq) || Ce³+ (aq), Ce**(aq) | Pt

Q: Using these metal ion/metal standard reduction potentials: Cd²+ (aq)| Cd(s): -0.38 V; Zn²+ (aq…

A: To determine the standard cell potential, we use- E∘cell = E∘cathode -E∘anode Cathode is the…

Question

The potential of the following voltaic cell is 0.490 V. Given this information, determine the Kb for the organic base (RNH₂) dissolved in the left cell.

Cell notation:
\[ \text{Pt (s)} \mid \text{H}_2 (\text{g}) (0.85 \text{ atm}) \mid \text{RNH}_2 (\text{aq}) (0.10 \text{ M}), \text{RNH}_3\text{Cl} (\text{aq}) (0.050 \text{ M}) \parallel \text{SHE} \]

Table of standard electrode potentials:
\[
\begin{array}{|c|c|}
\hline
\text{Half-reaction} & E^\circ (\text{V}) \\
\hline
2 \text{H}^+ (\text{aq}) + 2 \text{e}^- \rightleftharpoons \text{H}_2 (\text{g}) & 0.000 \\
\hline
\text{Hg}_2\text{Cl}_2 (\text{s}) + 2 \text{e}^- \rightleftharpoons 2 \text{Hg} (\text{l}) + 2 \text{Cl}^- (\text{aq}) & 0.268 \\
\hline
\end{array}
\]

The goal is to determine the base dissociation constant, \(K_b\), for the organic base \( \text{RNH}_2 \).

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

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 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

4. Write the overall net ionic equations for the following voltaic cells: (a) Zn(s)|Zn²"(aq)||Fe²*(aq)|Fe(s): (b) Zn(s)|Zn**(aq)||Fe**,Fe²*(aq)|C(s); (C = graphite is not involved in the reaction)
Consider the following galvanic cell: Li (s) | 0.095M LiCl (aq) || 0.032M Sn(NO3)2 (aq) | Sn (s) Using Appendix H in the textbook, determine the Ecell of this galvanic cell. 2.54 V - 2.88 V O -2.92 V 2.88 V 2.92 V
What is the net reaction for the cell? Is it .44V or .22V?
The potential of the following voltaic cell is 0.55 V. Given this information, determinethe Kb for the organic base (RNH2) dissolved in the left cell.
Consider the following galvanic cell at 25°C. Pt | Cr²+ (0.25 M), Cr³+ (2.0 M) || Co²+ (0.17 M) | Co The overall reaction and equilibrium constant value are given below. 2 Cr²+ "(aq) + Co2+ Calculate the cell potential & for this galvanic cell and AG for the cell reaction at these conditions. + (aq) → 2 Cr³+ (aq) + Co(s) K = 2.79x107
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
Consider the voltaic cellZn(s) | Zn2+(aq, 0.100 mol L−1) || Cu2+(aq, 1.200 mol L−1) | Cu(s)with the concentrations in the compartments as indicated. The circuit is closed and the battery is discharged until the concentration of Cu2+(aq) is 0.850 mol L−1. What is the electromotive force of the cell at that stage in the discharge?A) 1.048 VB) 0.508 VC) 0.434 VD) 1.132 VE) 1.108 V
Name: NetID: 5. Determine the standard cell potential (in V to two decimal places) for the following redox reactions. 2+ (a) Al(s) | Al³+ (aq, 1 M) || Cu²+ (aq, 1 M) | Cu(s) (b) Al(s) + NO3(aq) + 4H+ (aq) - Al³+ (aq) + NO(g) + 2H₂O(1) 13+ A: 2.00 A: 2.62
The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?t (1.0 M) || H* (test solution) H2 (1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn+ is –0.76 V. (Enter your answer to two significant figures.) pH =
Given the voltaic cell, what is the cell potential at the non standard conditions given in the cell schematic?