If we choose to use a standard oxidant for determining iron, we must first treat the sample solution with a/an _____________ to convert all of the iron to iron (II). a. Auxiliary reducing agent b. Auxiliary oxidizing agent c. Standard reductant d. Standard oxidant If we plan to titrate the analyte with a ___________, pretreatment with an auxiliary oxidizing reagent is needed. a. Auxiliary reducing agent b. Auxiliary oxidizing agent c. Standard reductant d. Standard oxidant Which of the following is the strongest oxidants? a. I2 b. K2Cr2O7 c. KBrO3 d. Na2S2O3

If we choose to use a standard oxidant for determining iron, we must first treat the sample solution with a/an ___ to convert all of the iron to iron (II). a. Auxiliary reducing agent b. Auxiliary oxidizing agent c. Standard reductant d. Standard oxidant If we plan to titrate the analyte with a _, pretreatment with an auxiliary oxidizing reagent is needed. a. Auxiliary reducing agent b. Auxiliary oxidizing agent c. Standard reductant d. Standard oxidant Which of the following is the strongest oxidants? a. I2 b. K2Cr2O7 c. KBrO3 d. Na2S2O3

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.16QAP

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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.
A precipitate of AgCl + AgBr weighs 0.8132 g. On heating on a current of Cl2, the AgBr is converted to AgCl, the mixture loses 0.1450 g in wt. Find the percentage Cl in the original sample.
Hello, I am trying to balance a tricky (skeleton) reaction using the half reaction method: CrI3 (s) + H2O2 (aq) → CrO42- (aq) + IO4- (aq) I ended up using H2O to balance the peroxide for the reduction half and pulled the rest of the equation down for the oxidation half since Cr and I both lose electrons. The final result was: 27H202 + 2CrI3 -----> 2CrO4^2- +6IO4^- + 22H2O + 10H+ for acidic and... 27H202 + 2CrI3 +10 OH^- -----> 2CrO4^2- +6IO4^- + 32H2O for basic Atoms and charges look balanced but I am feeling a bit uncertain about my method. Can you please confirm whether this is correct? Thank you, Carolyn
Chapter #10, Question #10-1: Consider the following equilibrium system: MnO4− + 4 H+ + 3 e− ⇌ MnO2(s) + 2 H2O(l) (a) Calculate the pEo value. (HINT: Consult this standard reduction potential table (b) Calculate the actual pE of a 50.0-L neutral aqueous solution containing 10.0 g of potassium permangante (KMnO4). Assume that only chemistry in the equilibrium system above determines the pE. (HINTS: In an equilibrium constant (K) or reaction quotient (Q) expression, pure solids and liquids behave has if they have values of 1. Concentrations in these expressions must be in mol L−1.)
Make the total number of electrons lost and gained equal by writing appropriate coefficients for both reducing and oxidizing reagents. Then balance the rest of the equation by inspection H2O2 + KMnO4 + H2SO4 -> K2SO4 + MnSO4 + H2O + O2
17. Consider the reaction of 0.161 g of aluminum metal with 50.0 mL of 0.235 M Co(NO₃)₂. a. Which metal, Al or Co, is more easily oxidized? b. Write the balanced chemical equation that occurs for the oxidation reaction. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction. c. What quantity in moles of Co(NO₃)₂ do you start with? d. What quantity in moles of metal product are generated if all of the Co(NO₃)₂ is consumed? e.What quantity in moles of Al do you start with? f. What quantity in moles of metal product are generated if all of the Al is consumed? g. Which reactant is limiting? h. What mass (in grams) of metal is formed when the limiting reactant is considered?
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Rank in decreasing strength of Reducing agent: Au(s), N2(g) ,Cr(s)
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Which of the following statements is/are correct for coulometry? I. Coulometric methods count the electrons used in a chemical reaction to measure the analyte. II. Coulometry uses constant current or constant potential conditions. III. An advantage of coulometric methods is low reproducibility and a disadvantage is low sensitivity. IV. Coulometric titrations are constant potential methods. V. Constant potential methods using a three-electrode cell are more selective than constant-current methods.
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