Given the following calibration curve data recorded from a F-ion selective electrode. The unknown and samples have a TISAB buffer (NaCl/glacial acetic acid/CDTA) added toprevent changes in the ionic strength impacting the results. The pH of the unknown and sample was adjusted to 6 to prevent interference or selectivity issues from OH-log [F, mol/L] Potential E vs RefpFmV5100.04341.5-17.0If the potential of an unknown F* solution is E vs REf=4.03.Assume the original unknown sample was diluted by the following: A 7 aliquot of the original unknown was diluted to a total volume of 58 mL.Report the original concentration of F in ppm F to 3 decimal places

potential of an unknown F- solution is E vs REf= 4.037 aliquot of the original unknown was diluted…

Given the following calibration curve data recorded from a F-ion selective electrode. The unknown and samples have a TISAB buffer (NaCl/glacia revent changes in the ionic strength impacting the results. The pH of the unknown and sample was adjusted to 6 to prevent interference or sele og [F, mol/L] Potential E vs Ref PF mV 5 100.0 4 3 41.5 -17.0 the potential of an unknown F solution is E vs REf=4.03. ssume the original unknown sample was diluted by the following: A 7 aliquot of the original unknown was diluted to a total volume of 58 mL.

Given the following calibration curve data recorded from a F-ion selective electrode. The unknown and samples have a TISAB buffer (NaCl/glacia revent changes in the ionic strength impacting the results. The pH of the unknown and sample was adjusted to 6 to prevent interference or sele og [F, mol/L] Potential E vs Ref PF mV 5 100.0 4 3 41.5 -17.0 the potential of an unknown F solution is E vs REf=4.03. ssume the original unknown sample was diluted by the following: A 7 aliquot of the original unknown was diluted to a total volume of 58 mL.

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: 16. In the gas deposition electrode cell with the cell diagram: Pt | H2 (P1) | HCl | H2 (P2) | Pt…

A: Given cell : Pt | H2 (P1) | HCl | H2 (P2) | PtStandard Reduction Potential E°(2H+/H2) = 0 V Cathode:…

Q: Refer to the following standard reduction potential table as needed. Electrode reaction Eº, V Lit+…

A: Oxidising agent is the species which oxidises other species and reduces itself. Reducing agent is…

Q: When an ion-selective electrode for X* was immersed in 0.0565 M XC1, the measured potential was…

A: Cell potential = E Standard cell potential = E0 Reaction quotient = Q = oxidised speciesreduced…

Q: The value of K, for AgBr is 5.4 x 10-13, For the Ag/AgBr electrode, AgBr{s) +€ = Ag{s) + Br (aq)…

A: Given:Concentration of HBr = 0.010 MCalculate EcellCell potential, also known as electromotive force…

Q: 4. In the galvanic cell below, the anode is: Zn | Zn²*(1 M)|Ag*(1M)|Ag ]None of the other answers…

A: Hi, as you have posted multiple questions and have not mentioned which one you want us to solve for…

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: A Zn wire and Ag/AgCl reference electrode saturated with KCl (E = 0.197 V) are placed into a…

Q: Enter a balanced equation for the overall reaction.

A: The electrode with the smaller electrode potential tends to undergo oxidation and thus is an anode.…

Q: Q10. At 25 oC the standard electrode potential for the Ag+|Ag electrode is 0.7991 V, and the…

A: The standard electrode potential for the electrode = The solubility product for we have to…

Q: › At 25 °C, a titration of 15.00 mL of a 0.0280 M AgNO3 solution with a 0.0140 M Nal solution is…

Q: When an ion-selective electrode for X+ was immersed in 0.0686 M XCI, the measured potential was…

Q: Given the following calibration curve data recorded from a K-ion selective electrode. The unknown…

A: Given: The Calibration data recorded from a K-ion selective electrode.

Q: When the potential a half reaction was measured against a Ag|AgCl reference electrode, the potential…

A: Reference electrode is one which behave as ideal electrodes, i.e. do not undergo polarization, under…

Q: ++ -0.10 -0.05 Standard Hydrogen Electrodo 0.0 0.05 0.10 0.15 AglAgCl Saturated Electrode Calomel…

A: Standard electrode potential of hydrogen electrodes = 0.00 V Standard electrode potential of…

Q: What Range of cathode potentials versus the saturated calomel electrode can be used to…

A: The expression of Nernst equation is shown below: Ecell = E0cell - 0.0591nlog Q Where; Ecell= cell…

Q: A B In a standard hydrogen electrode: AG° 0 с AG° = 0

A: Approach to solving the question: I analyzed the question before answering it. Key…

Q: 20 mL of 0.01 M V2+ is titrated by 0.01 M Ce4+ in 1 M HCI using SHE reference electrode to find the…

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

Q: Please don't use AI solution and don't use hend raiting

A: The Nernst equation can be used to calculate the electrode inertia for different concentrations of…

Q: Define standard electrode potential Given: Pb2+ / Pb Eθ = +0.13V Cu2+ / Cu Eθ = +0.34V…

Q: A voltaic cell is constructed in which the anode is a Mg|Mg²+ half cell and the cathode is a NiNi2+…

A: The oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation…

Question

Given the following calibration curve data recorded from a F-ion selective electrode. The unknown and samples have a TISAB buffer (NaCl/glacial acetic acid/CDTA) added to
prevent changes in the ionic strength impacting the results. The pH of the unknown and sample was adjusted to 6 to prevent interference or selectivity issues from OH
-log [F, mol/L] Potential E vs Ref
pF
mV
5
100.0
4
3
41.5
-17.0
If the potential of an unknown F* solution is E vs REf=4.03.
Assume the original unknown sample was diluted by the following: A 7 aliquot of the original unknown was diluted to a total volume of 58 mL.
Report the original concentration of F in ppm F to 3 decimal places

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1: Given

VIEW

Step 2: Solving

VIEW

Solution

VIEW

Step by step

Solved in 3 steps with 3 images

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

When a fluoride selective electrode was immersed in a solution that is 1.0 x 10-4 M in F-, the potential that developed (versus SCE) was 41.5 mV. What will be the potential that will develop if the same electrode is immersed in a solution that is 5.0 x 10-5 M in fluoride? -51 mV -47 mV -59 mV -32 mV
A gallium electrode and a Ag/AgCl reference electrode (+0.197 V vs SHE) are immersed in a solution containing Ga*. The cell voltage is -0.766 V. Calculate the molar concentration of Ga3+. 3. Ag/AgCl ref. || Ga³+ | Ga(s) Ga+ + 3e Ga(s) E° = -0.560 V
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…
Addition of both Bi3+ and Sn2+ by the method by studying the cathode potential to be made for molding of those in a buffered solution to 0.100 M and pH 1.5. Find the concentration of the more difficult-to-make species or the more easily-reducible species. Sn2+ + 2 e- ↔ Sn (k) E0 = - 0.136 V BiO+ + 2 H+ + 3 e- ↔ Bi (k) E0 = 0.320 V A. 3.2x10-2MB. 2.33 x 10-22MC. 1x10-6MD. 6.2x10-22M
Consider the titration of 60.00 mL of 0.100 M Co3+ with 0.130 M MnO²- . What is the potential after 30.00 mL of 0.130 M MnO²- has been added in units of Volts? The potential is measured against the Ag|AgCl reference electrode (E(saturated KCI) = 0.197 V). Co 3+ + e =Co 2+ E°= 1.92 V MnO¯ + e ¯ = MNO2- E°= 0.56 V
I’m having difficulties answering 4b.