Prepare a Potential Diagram for pH=1.0 and 10.0 based on the following Selenium Pourbaix Diagram. Label the oxidation state of selenium at each step in your potential diagram. Generate a Frost-Ebsworth Diagram for pH = 1.0 and 10.0.
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- One of the types of first generation pesticides contained arsenic. An analytical analysis for arsenic was to convert to AsO4-3 and precipitate with Ag+, yielding Ag3AsO4(s). What is the oxidation state of arsenic in this precipitate? Group of answer choices -5 -3 0 +3 +5a) Chlorine is disproportionate in basic medium. And in an acid medium? Write both reactions and calculate the final potential, indicating if they are thermodynamically favorable (See Frost diagram) ClO- /Cl2 = 0.42 V HClO /Cl2 = 1.63 V Cl2 /Cl- = 1.36 V b) Use the Latimer diagram of chlorine in acid medium to determine the potential corresponding to the reduction of ClO4 - to Cl2. Write the fitted equation of this reaction.The iodine produced when excess of KI was added to the solution containing 0.1259 g K2Cr2O7 required a 41.26 mL titration with Na2S2O3 required a 41.26 mL titration with Na2S2O3. P.S. Be able to answer numbers 1 and 2 ONLY. 1. Determine if it is basic or acidic and write the balance redox reaction for the reaction of dichromate ion with iodide ion in acidic medium. Unbalance equation: Cr2O72- (aq) + I- (aq) → Cr3+ + I2 (aq) 2. Determine if it is basic or acidic and write the balance redox reaction of iodine with sodium thiosulfate in acidic medium. Unbalance equation: S2O3 2- (aq) + I2 (aq) → S4O6 2- (aq) + I- (aq) 3. (i) What are the oxidizing agents in #1 and #2? (ii) What is the stoichiometric ratio between dichromate and thiosulfate? 4. Calculate the molar concentration of the thiosulfate solution.
- The F− concentration of a solution was determined by measurements with a liquidmembrane electrode. The electrode system developed a potential of 0.5021 V when immersed in 25.00 mL of the sample, and 0.4213 V after the addition of 2.00 mL of 5.45 x 10−2 M NaF. Calculate pF for the sample.Note: pF is the negative logarithm of [F].A cell consisting of a saturated calomel electrode and a lead ion electrode developed a potential of -0.3257 V when immersed in a 60.00 mL lead solution of unknown concentration. A 10.00 mL addition of 0.02500 M lead standard solution caused the reduction potential to shift to -.2897 V. Calculate the molar concentration (in units mM) of lead in the sample. Please make sure to perform necessary calculations to have a final answer in mM.A glass / calomel electrode system was found to develop a potential of - 0.0412 V when used I a buffer of pH 6.00; with an unknown solution the potential was observed to be - 0.204 V. Calculate the pH and the [H+] of the unknown. The following cell was employed for the determination of pCrO4: SCE // CrO4 2-(xM) / Ag2CrO4 (s) / Ag (s) Find the pCrO4 if the cell potential is - 0.402 V (E0 Ag/Ag2CrO4 = - 0.316 V ; E SCE = 0.241 V)
- please answer what you can. thank you so much in advance. :) Standardisation of EDTA using zinc metal Mass of zinc = 1.050 g. Calculate the number of moles of zinc in the 250 mL flask (show workings) Calculate the concentration zinc in the 250 mL flask (show workings) Calculate the number of moles of Zn2+ in the 20 mL aliquot (show workings) Calculate the number of moles of EDTA in the average titre (show workings) Calculate the concentration of the DILUTED EDTA solution (show workings) Sample No. 1 2 3 4 Final Burette reading (mL) 20.25 42.75 22.90 44.50 Initial Burette reading (mL) 0.05 20.25 1.50 22.90 Final-Initial Titre (mL) 20.20 22.50 21.40 21.60Give only typing answer with explanation and conclusion 0.1745 g of primary standard Na2C2O4 is used to set a freshly prepared KMnO4 solution and 30.24 mL of KMnO4 solution is spent at the turning point. Since 36.92 mL of this KMnO4 solution is consumed for the determination of iron in 0.5618 g ore sample, calculate the amount of iron in the ore in terms of % iron (III) oxide and % iron (III) chloride. (Fe: 56, K: 39, Mn: 55, O: 16, Na:23, C: 12, Cl: 35.5 g/mol)For indicator electrodes, which statements are true?I Indicator electrodes are made from relatively inert metals.II Indicator electrodes work best when the electrode surface is large and clean.III Platinum is a common indicator electrode.IV Platinum electrodes are more inert than gold electrodes. A. I, III, and IV B. I, II, and III C. I, II, III, and IV D. II and III E. I, II, and IV
- The cell SCE//Ag2CrO4(sat’d), CrO4-2 (x M)/Ag is used for the determination of pCrO4. The half reaction at indicator electrode Ag2CrO4 (s) + 2 e- -> 2 Ag(s) + CrO4 -2(aq) E=0.446 Calculate pCrO4 when the cell potential is 0.402 V. Show your calculations by uploading your solutions.acid dissociation constants for H3PO4 (Ka1 = 7.11 × 10-3, Ka2 = 6.32 × 10-8, Ka3 = 7.1× 10-14), calculate standard reduction potential for the half reactionH2PO4- + H+ + 2e HPO32- + H2OWrite a charge balance for H2SO4 in water.