help (i)Sodium chromate and iron(II) chloride are mixed in an acidic medium. Assign oxidationnumbers to all elements in the following equation, balance the equation and calculate thenumber of moles of Cr* chloride produced if 15 cm3 of 0.25 M sodium chromate (Na2Cr2O7)are consumed in the reaction.Cr20,2 (aq) + Fe2+Cr3+(aq)+ Fe* (aq) (acidic conditions)(aq)(ii) Assign oxidation numbers to all elements in the following equation, balance the equation andcalculate the volume of 0.15 M potassium permanganate (KMNO4) required to react with 10cm³ of 0.2 M potassium sulfite (K2SO3).MnOa (aq) + S03² (aq)MnO2(s) +SOo (aq) (basic conditions)

(i) Sodium chromate and iron(lI) chloride are mixed in an acidic medium. Assign oxidation numbers to all elements in the following equation, balance the equation and calculate the number of moles of Cr3* chloride produced if 15 cm³ of 0.25 M sodium chromate (Na2Cr2O7) are consumed in the reaction. Cr20,2(aq) + Fe²*(aq) Cr* (aq) + Fe3+ *(aq) (acidic conditions) (ii) Assign oxidation numbers to all elements in the following equation, balance the equation and calculate the volume of 0.15 M potassium permanganate (KMNO4) required to react with 10 cm³ of 0.2 M potassium sulfite (K2SO3). MnOs (aq) + SO3? (aq) MnO2(e) + SO, (aq) (basic conditions)

(i) Sodium chromate and iron(lI) chloride are mixed in an acidic medium. Assign oxidation numbers to all elements in the following equation, balance the equation and calculate the number of moles of Cr3* chloride produced if 15 cm³ of 0.25 M sodium chromate (Na2Cr2O7) are consumed in the reaction. Cr20,2(aq) + Fe²(aq) Cr (aq) + Fe3+ *(aq) (acidic conditions) (ii) Assign oxidation numbers to all elements in the following equation, balance the equation and calculate the volume of 0.15 M potassium permanganate (KMNO4) required to react with 10 cm³ of 0.2 M potassium sulfite (K2SO3). MnOs (aq) + SO3? (aq) MnO2(e) + SO, (aq) (basic conditions)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 80AP

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A 1.1324 g sample of magnetite ore was dissolved in concentrated HCl to give a solution that contained a mixture of Fe2+ and Fe3+. Nitric acid was added and the solution was boiled for a few minutes, which converted all of the iron to Fe3+. The Fe3+ was then precipitated as Fe2O3*xH2O by addition of NH3. After filtration and washing, the residue was ignited at a high temp to give 0.5394 g of pure Fe2O3. What is the percent Fe and the percent Fe3O4 in the sample?
A solution containing 0.402 49 g of CoCl2 ? xH2O (a solid with an unknown number of waters of hydration) was exhaustively electrolyzed to deposit 0.099 37 g of metallic cobalt on a platinum cathode by the reaction Co21 1 2e2¡Co1s2. Calculate the number of moles of water per mole of cobalt in thereagent. A good approach is to find moles of Co, moles of CoCl2, mass of CoCl2, and, by difference, mass of H2O in the sample.
1. What is the gravimetric factor of SO3 in BaSO4? 2. What is the normality of an oxidizing agent of a solution of potassium dichromate (K2Cr2O7) containing 8.906 g per 200 mL in the presence of acid? (Cr2O7-2 + 6Fe+3 + 14H+ → 2Cr3+ + 6Fe3+ + 7H2O) NOTE: Present complete solution with corresponding units.
Magnesium Chloride is available as magnesium chloride hexahydrate in an injectable solution that supplies 1.97 mEq of magnesium per milliliter. What is the percent strength of magnesium chloride hexahydrate in this solution?
For the gravimetric determination of manganese, 1.8762 g of sample containing Mn was dissolved in acid solution and made up to 100 mL in a calibrated volumetric flask. A 25.00 mL aliquot of this solution was transferred to a beaker. The solution was heated to boiling and chemical substances required were added till precipitating MnNH4PO4. After filtering, rinsing, and igniting, 0.5365 g of Mn2P2O7 was obtained. Calculate the % manganese in the sample (Mn: 55, P: 31, O: 16 g/mol).
An analyst was assigned to work a sample with minerals. This iron-containing sample was analyzed by dissolving a 1.3142g sample in concentrated HCl. The resulting solution was diluted with water and iron (III) was precipitated as the hydrated oxide Fe2O3 xH2O by the addition of HN3. After filtration and washing, the residue was calcined at high temperature to produce 0.5488g of pure Fe2O3 (159.69g / mol). Determine the following:a) the% Fe (55.847 g / mol) and the% Fe3O4 (231.54 g / mol) in the sample.
The progress of the reaction between Iodine ions and potassium iodate(V) can be followed by withstanding samples of the reaction mixture at various times, quenching and then titrating with standard thiosulphate solution. The reaction equation is: I(aq) + IO3(aq) + 6H+(aq) + 4e ➡ I2(aq) + 3H2O(l) What other method could be used to follow up this reaction? How could you quench the reaction?
A sample of bleach has a content of about 2.13% (w/v) in “active chlorine”. For perform its analysis by redox volumetry and using a thiosulfate solution of sodium, how much of this sample would be needed to prepare, in a volumetric flask, 500 mL of a 0.0301 M solution in NaClO ? A 25.00 ml aliquot of the solution contained in the flask, was titrated using a standardized 0.0557 M sodium thiosulfate solution. What was the volume of titrant spent?Data: MM NaClO = 74.45 g/mol; MM Cl2 = 70.90 g/mol
The equivalent weight is k2Cr2O7 When reduced, Cr + 3 , O = 36, Cr = 52K = 39
Write the balanced NET ionic equation for the reaction when aqueous KBr and aqueous AgC₂H₃O₂ are mixed in solution to form aqueous KC₂H₃O₂ and solid AgBr
0.1724g of a mineral containing MnO₂ was dissolved and then treated with excess iodide according to the following unbalanced reaction: MnO2(s) + H+ → Mn²+ + I2 + H₂O The I₂ released was titrated with a solution of Na₂S2O3 0.07320 mol/L, requiring 14.65 mL to reach the point end of degree a) Determine the percentage of MnO₂ in the ore. b) When iodine solutions are used as titrants these are prepared by dissolving 1₂ in concentrated KI. Explain the reason for the need for KI in the preparation of these solutions?
A precipitate of AgCl + AgBr weighs 0.8132 gram. On heating in a current of chlorine, the AgBr is converted into AgCl, the mixture losing 0.1450 gram in weight. What was the percentage of chlorine in the original precipitate?

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