3) Balance the following redox reaction if it occurs in acidic solution.MnO4 (aq) + Fe(s) - Mn2+(aq) + Fe 3+(aq)Understanding1.0-=3V OS.I+ (8Ve0-(A32rli ri bornstersd 91s anorbolo vnsm voH (eSaM+ (e)(A - (pe)A (e)gMai 1led llao yb & ol noitoss llso arT (01)*HS + ()0rMS+ (2)Si Il9p eirdi not Isinsiog llas busbnrde arTI-(Awolloi sri 1ol Istrelog llso ort alslusols (V 10.1 (8V 10.0 (AISBN 1-41A dnsianos m ndiliups art olelole (OnM+ (pa) Sal 2+ (pa)+H 8

You follow a series of steps in order: 1. Identify the oxidation number of every atom. 2. Determine…

3) Balance the following redox reaction if it occurs in acidic solution. MnO4 (aq) + Fe(s) Mn2+(aq) + Fe 3+(aq) LPe) + B5(1) - LPs (ad) + S BL ( Understandi (pe)18- ()si V OS.I+ (8 Vie.0- (A ni borsiensTi 915 2norbols yasm voH (e FaM (A- (peA (e)gM E (8 ei sled llas yb & ol noitoss llso erT (01 HS+ ()0rMS+(2)S Igp eidi not Isiinslog lla busbnrie arlT olloi or 1ol Isitrelog lso orlt alsluols (I V 10.1+ (8 V 10.0 (A ISE dristanos m hdiliups ort oteleole (S OnM (pa) Sol 2+ (pn)+H 8 SE (8

3) Balance the following redox reaction if it occurs in acidic solution. MnO4 (aq) + Fe(s) Mn2+(aq) + Fe 3+(aq) LPe) + B5(1) - LPs (ad) + S BL ( Understandi (pe)18- ()si V OS.I+ (8 Vie.0- (A ni borsiensTi 915 2norbols yasm voH (e FaM (A- (peA (e)gM E (8 ei sled llas yb & ol noitoss llso erT (01 HS+ ()0rMS+(2)S Igp eidi not Isiinslog lla busbnrie arlT olloi or 1ol Isitrelog lso orlt alsluols (I V 10.1+ (8 V 10.0 (A ISE dristanos m hdiliups ort oteleole (S OnM (pa) Sol 2+ (pn)+H 8 SE (8

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter24: Coulometry

Section: Chapter Questions

Problem 24.4QAP: Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose...

See similar textbooks

Similar questions

What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 V
The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
The cell Ag|AgCl(sat’d)||H+(a = x)|glass electrode has a potential of —0.2094 V when the solution in the right-hand compartment is a buffer of pH 4.006. The following potentials are obtained when the buffer is replaced with unknowns: (a) —0.2806 V and (b) —0.2132 V. Calculate the pH and the hydrogen ion activity of each unknown. (c) Assuming anuncertainty of 0.001 Vin the junction potential, what is the range of hydrogen ion activities withinwhich the true value might be expected to lie?
The measurement of pH using a glass electrode obeys the Nernst equation. The typical response of a pH meter at 25 00C is given by the equation where contains the potential of the reference electrode and all other potentials that arise in the cell that are not related to the hydrogen ion concentration. Assume that = 0.250 V and that a. What is the uncertainty in the values of pH and [H+] if the uncertainty in the measured potential is 1 m V ( 0.001 V)? b. To what precision must the potential be measured for the uncertainty in pH to be 0.02 pH unit?
Consider a concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are dissolved in solution B (ignore volume changes), where the reaction M2+(aq)+SO42(aq)MSO4(s) occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25C. Assume that the process M2++2eM has a standard reduction potential of 0.31 V and that no other redox process occurs in the cell. Calculate the value of Ksp for MSO4(s) at 25C.
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Zn|Zn2+(0.50M)Cd2+(0.020M)|Cd (b) Cu|Cu2+(0.0010M)H+(0.010M)|H2(1.00atm)|Pt
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Cu|Cu+(0.80M)Hg22+(0.10M)|Hg|Pt (b) Cr|Cr3+(0.615M)Ni2+(0.228M)|Ni
In the electrolysis of a solution containing Ag+(aq), metallic Ag(s) deposits on the cathode. Using a current of 1.12 A for 2.40 hours, what mass of silver forms?
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)?
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?