2. Sketch (as accurately as you can) steady state i vs E curves for solutions prepared from: a) 1 mM SnV and 2 mM Cel b) 1 mM Fell and 2 mM Celv c) 1 mM Fell and 2 mM Sn" Eº (Cel) = 1.41 V, reversible Eº (Fe) = 0.77 V, reversible Eº (Sn¹V) = 0.15 V, irreversible For (a) assume Eeq = 0.20 V and io/ilim = 0.001, for (c) assume io/ilim = 0.01.

2. Sketch (as accurately as you can) steady state i vs E curves for solutions prepared from: a) 1 mM SnV and 2 mM Cel b) 1 mM Fell and 2 mM Celv c) 1 mM Fell and 2 mM Sn" Eº (Cel) = 1.41 V, reversible Eº (Fe) = 0.77 V, reversible Eº (Sn¹V) = 0.15 V, irreversible For (a) assume Eeq = 0.20 V and io/ilim = 0.001, for (c) assume io/ilim = 0.01.

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

Similar questions

give me solution within half hour give you multiple upvote
Data: T/ °C E/V 25 35 45 55 65 0.458 0.455 0.452 0.449 0.446 Calculations: 1. Determination of the solubility of AgCl in 0.5 M KCl at all temperature 2. Determination of the solubility product (Ksp) of AgCl in 0.5 KCl at all temperature
Required: Normality of Iodine
How much amount of solids (in grams) do you need to prepare the following solutions? 1. 500.0 mL 0.1000 M stock EDTA solutiona. Weigh an appropriate amount of Na2H2EDTA2H2O (FW=372.24) to the nearest 0.1 mg 2. 100.0 mL 0.0500 M stock Ca2+ solutiona. Weigh appropriate amount of pure CaCO3 (FW=100.09) to the nearest 0.1 mg into a 250 mL beaker.
КНР (ад) + NаОН (ад)- - NAKHP (aq) + H20 (1) Trial V; (mL) V; (mL) 33.87 45.73 2 A student masses out 1.019 grams of KHP, which is dissolved in 25.00 mL of DI water. This KHP solution is titrated with NAOH, as shown in the equation above. Calculate the molarity of the NaOH solution. RE FS F6 F7 FB F10
#6. Thank you. answer on bracket
Calculate the % relative error in solubility by using concentrations instead of activities for the Ag3AsO4 in 7.3 x 10 aAg = 0,25 a AsO4 = 0,4 alfa 0.05 M KNO3 (Ksp (Ag3AsO4) = -22
Approximately 6.0mL of concentrated perchloric acid (70%) was transferred to a bottle and diluted with about 1.0L of water. A sample containing 251.5 mg of primary standard Na2B4O7.10H2O required 27.41 mL of the HClO4 solution to reach the methyl red end point. Calculate the molar concentration of the HClO4 (Fwt = 382g/mole)
A 10.0 g sample of KC3H504 (A)(MW = 204.23 g A) was titrated with 50.00 mL of KOH (B) to endpoint. What is the molarity of the KOH solution? Use A and B to show compounds in the working. Given: KCgHsO4 (s) + КОН (аq) ----> K2C8H4O4 (aq) + H2O (1I) 1. 10.0 g Ax 3. 5. 7. 9 2._ 4. X 6. 8. 1.--- 2.__--- 3._---- 4._- 5. A 6.
Please send me the question in 30 minutes it's very urgent plz
A sample containing iron is approximately 99.0% w/w Fe. Using ammonia, iron is precipitated as Fe (OH)3 which is ignited to Fe203. (a) What is the gravimetric factor for analyte Fe (AW=55.85 g/mol) and precipitate Fe203 (FW=159.69 g/mol)? (b) What mass of sample is needed to ensure that the Fe203 precipitate would weigh at least 1.00 g?
SO4 -two content in 7689mL of a water sample was precipitated as Na2SO4. The precipitated was filtered, washed and calcined in an empty crucible with a mass of 27.0234g. The mass of the crucible plus Na2SO4 (142g/mol) was 27.7708g. Calculate the %m/v of Na (23g/mol) and the concentration of Na in the sample in ppm.