selectivity coefficient Kot immersed in 1.00 mM NaCl at pH 8.00, a potential of -38 mV (versus S.C.E.) was recorded. (a) Neglecting activity coefficients, calculate the potential with Equation 14-10 if the electrode were immersed in 5.00 mM NaCl at pH 8.00. (b) What would the potential be for 1.00 mM NaCl at pH 3.87? You can see that pH is a critical variable for the sodium electrode 36. When this electrode was H*

selectivity coefficient Kot immersed in 1.00 mM NaCl at pH 8.00, a potential of -38 mV (versus S.C.E.) was recorded. (a) Neglecting activity coefficients, calculate the potential with Equation 14-10 if the electrode were immersed in 5.00 mM NaCl at pH 8.00. (b) What would the potential be for 1.00 mM NaCl at pH 3.87? You can see that pH is a critical variable for the sodium electrode 36. When this electrode was H*

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: 6. The corrosion rate of iron in deaerated HCl of pH = 3 is 3.0 gmd. Calculate the corrosion…

A: The objective is to calculate the corrosion potential of iron in this acid solution compared to a…

Q: Q5: Answer with True or False for the following statements (only 7 statements) 1. If the reduction…

A: Following are the appropriate answers (True/Fulse) of the given questions. According to…

Q: The selectivity coefficient of the fluoride ion-selective electrode is kF-,OH- = 0.15. How does the…

A: Given as kF-,OH- = 0.15. [F- ]=1.4 x 10-5 M

Q: 19. Given Fe + 2e → Fe, o° =-0.440 v, and Fe +eFe", o° = 0.771 V, cal- culate o° for Fe* + 30 Fe 20.…

A: 19) Fe2++2e - ➡️ Fe. ¢°=-0.440V Fe3+ +e- ➡️Fe2+. ¢° =0.771V Adding both the…

Q: 2) A cyanide ion selective electrode obeys the equation : E (volts) = constant - 0.05916 log [CN-]…

A: We will first calculate the numerical constant because we have to use this constant for solving the…

Q: What would the potential of a standard hydrogen electrode (S.H.E.) be under the given conditions?…

A: Standard hydrogen electrode (S.H.E.): The standard reduction potential of a standard hydrogen…

Q: help please answer in text form with proper workings and explanation for each and every part and…

A: To calculate the potential ( E ) for the (Fe3+/Fe2+) electrode when the concentration of (Fe3+) is…

Q: (8) The cell: SCE//HA(0.250M), NaA(0.170M)/H2(1.00bar), Pt has a poten- tial of -0.721V at 298K.…

A: The objective of the question is to Sketch the cellCalculate the Potential of the CellCalculate the…

Q: Solve the following queries. Make sure to show complete procedure a) Would H₂O₂ behave as oxidant or…

A: H2O2 can behave as oxidant or reductant .

Q: 4. Calculate the EMF of a cell made up of a hydrogen electrode (PH2 1 atm) and an oxygen electrode…

A: The objective of this question is to calculate the EMF of the cell, determine its polarity, and plot…

Q: What is the potential of this cell? Enter you answer to the hundredths place (x.xx V). Pt | Pb²+…

Q: What would the potential of a standard hydrogen electrode (S.H.E.) be under the following…

Q: From the calibration curve using standard F solutions, the slope of the curve is -58.5 mV. When a…

A: Solution- Data Given- Slope of the curve (S) = -58.5 mV, E(potential) = 100.0 mV, K = Coulomb…

Q: 1. Solve the following queries. Make sure to show complete procedure At equal concentrations of Fe²+…

A: #1: #(b): (a): Given [Fe2+] = [Fe3+] half-reactions: Anode: Fe2+ → Fe3+ + 1e- ; Eoanode = 0.77 V…

Q: Which electrode material (silicon vs glassy carbon) give reversible signals for the electrochemical…

A: Solutions- Electrochemical reduction of Dinitrobenzene.

Q: Consider the titration of 25.0 mL of 0.010 0 M Sn21 by 0.050 0 M Tl31 in 1 M HCl, using Pt and…

A: According to Q&A guidelines of Bartleby, we are supposed to answer only the first 3 sub-parts of…

Q: What would the potential of a standard hydrogen electrode (S.H.E.) be under the following…

A: Answer:Here, n is equal to number of electrons gained by the specie in the balanced cell reaction.

Q: Convert each of the potentials. The silver-silver chloride and calomel reference electrodes are…

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

Q: Hi, can you write which is oxidation and which reduction with equation for Fe/Sn, Fe/Zn, Fe/Al,…

A: Oxidation takes place when there is an increase in the oxidation state or loss of electrons.…

Question

100%

14-D. One glass-membrane sodium ion-selective electrode has a
selectivity coefficient KH = 36. When this electrode was
immersed in 1.00 mM NaCl at pH 8.00, a potential of – 38 mV
(versus S.C.E.) was recorded.
(a) Neglecting activity coefficients, calculate the potential with
Equation 14-10 if the electrode were immersed in 5.00 mM NaCl at
pH 8.00.
(b) What would the potential be for 1.00 mM NaCl at pH 3.87? You
can see that pH is a critical variable for the sodium electrode.

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

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

Indicate the option that is true:(1). An indicator electrode has an upper limit of measurement; That is, it does not serve as a precise analytical instrument when the concentrations of the analyte are very high.(2). Some electrodes take a long time to respond, but that is usually not an insurmountable drawback.(3). The representation of the potential of an indicator electrode against the analyte concentration is a straight line for analyte concentrations below a certain value.(4). For activities lower than the lower detection limit, the electrode always measures the same potential.
e) Using the half reaction below sHE Pou3- HPO,2 + 2H* + 2e HPO+H;O E--0,234 V and acid dissociation constants for H3PO4 (K=7.11 × 10°; K2 = 6.32 × 10*, K7.1 x 1014), calculate standard reduction potential for the half reaction he Oy H2POª + H* + 2e HPO + H;O
6. f. Consider the following coupled redox reaction. O₂ + 2NADH + 2H* = 2H₂O + 2NAD+ Calculate AG" (at 310 K) if the standard reduction potentials for O2 and NAD+ are 0.815V and -0.315V respectively. g. If you wanted to shift the above reaction in f. to the left, how would you adjust the pH? Explain briefly. Lab-related questions. a. In lab, you made a 5 M NaCl stock solution. How would you make a 10- mL 0.5 M NaCl solution from your stock solution? i. 9 mL 5 M NaCl and 1 mL water ii. 5 mL 5 M NaCl and 5 mL water iii. 1 mL 5 M NaCl and 9 mL water iv. 0.1 mL 5 M NaCl and 9.9 mL water b. In the first week of lab, you made a pH 7.4 phosphate buffer by mixing some H₂PO4 with HPO4². The pK₂ of H₂PO4 is 7.2. Which of the following is true? i. ii. iii. iv. 7 More H₂PO4* needs to be added because the pH > pKa More HPO4²- needs to be added because the pH > pKa More H₂PO4 needs to be added because more acid is needed to maintain a pH of 7.4. More HPO4²- needs to be added because it is more…
help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working
Please do this ASAP