A blood sample was submitted for electrolyte analysis. The Mg²* content (known as "ionized magnesium" orIMg") of the blood was determined using an ion-selective electrode that is known to have an electromotiveefficiency of 0.9452+When placed in a solution containing 10.0 mM Mg", the electrode produced a potential of 175.0 mV.When placed in the blood sample, the electrode produced a potential of 138.7 mV.Calculate the concentration of Mg?* in the blood sample. (For a healthy human, IMg* is between 0.53 and 0.67mM.) (Report the answer to two significant figures.)2+

Response of an ion-selective electrode in given as: E=constant+β0.05916nlog[Analyte] where, E is…

A blood sample was submitted for electrolyte analysis. The Mg content (known as "ionized magnesium" or IMg") of the blood was determined using an ion-selective electrode that is known to have an electromotive efficiency of 0.945 When placed in a solution containing 10.0 mM Mg²", the electrode produced a potential of 175.0 mV. When placed in the blood sample, the electrode produced a potential of 138.7 mV. Calculate the concentration of Mg?+ in the blood sample. (For a healthy human, IMG2 is between 0.53 and 0.67 mM.) (Report the answer to two significant figures.)

A blood sample was submitted for electrolyte analysis. The Mg content (known as "ionized magnesium" or IMg") of the blood was determined using an ion-selective electrode that is known to have an electromotive efficiency of 0.945 When placed in a solution containing 10.0 mM Mg²", the electrode produced a potential of 175.0 mV. When placed in the blood sample, the electrode produced a potential of 138.7 mV. Calculate the concentration of Mg?+ in the blood sample. (For a healthy human, IMG2 is between 0.53 and 0.67 mM.) (Report the answer to two significant figures.)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.15QAP

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An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
Consider only the species (at standard conditions) Na+, Cl, Ag+, Ag, Zn2+, Zn, Pb in answering the following questions. Give reasons for your answers. (Use data from Table 17-1.) a. Which is the strongest oxidizing agent? b. Which is the strongest reducing agent? c. Which species can be oxidized by SO42 (aq) in acid? d. Which species can be reduced by Al(s)?
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At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction PbC2O4(s)+2ePb(s)+C2O42(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/PbC2O4 electrode in a 0.025 M solution of Na2C2O4.
An electrolytic cell is set up with Cd(s) in Cd(NO3)2(aq) and Zn(s) in Zn(NO3)2(aq). Initially both electrodesweigh 5.00 g. After running the cell for several hours theelectrode in the left compartment weighs 4.75 g. (a) Which electrode is in the left compartment? (b) Does the mass of the electrode in the right compartmentincrease, decrease, or stay the same? If the masschanges, what is the new mass? (c) Does the volume of the electrode in the right compartment increase, decrease, or stay the same? If the volumechanges, what is the new volume? (The density of Cd is8.65 g/cm3.)
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