95. Manganese is derived from pyrolusite ore, animpure manganese dioxide. In the procedure used toanalyze a pyrolusite ore for its MnO2 content, a 0.533 gsample is treated with 1.651 g oxalic acid(H;CO, 2 H2O) in an acidic medium. Followingthis reaction, the excess oxalic acid is titrated with0.1000 M KMNO, 30.06 mL being required. What isthe mass percent MnO2 in the ore?H;C;O4 + MnO2 + H* →Mn2+ + H;0 + CO; (not balanced)H;C,O, + MnO, +H* •-Mn* + H20 + CO2 (not balanced)

Here , Oxalic acid is back titrated with KMnO4 , so concept of back Titration will be used here as…

Manganese is derived from pyrolusite ore, an impure manganese dioxide. In the procedure used to analyze a pyrolusite ore for its MnO2 content, a 0.533 g sample is treated with 1.651 g oxalic acid (H;C;O4•2 H¿O) in an acidic medium. Following this reaction, the excess oxalic acid is titrated with 0.1000 M KMNO, 30.06 mL being required. What is the mass percent MnO2 in the ore? H;C¿O4 + MnO2 + H* Mn2+ + H;0 + CO: (not balanced) H;C,O, + MnO, +H* Mn + H;O + CO; (not balanced)

Manganese is derived from pyrolusite ore, an impure manganese dioxide. In the procedure used to analyze a pyrolusite ore for its MnO2 content, a 0.533 g sample is treated with 1.651 g oxalic acid (H;C;O4•2 H¿O) in an acidic medium. Following this reaction, the excess oxalic acid is titrated with 0.1000 M KMNO, 30.06 mL being required. What is the mass percent MnO2 in the ore? H;C¿O4 + MnO2 + H* Mn2+ + H;0 + CO: (not balanced) H;C,O, + MnO, +H* Mn + H;O + CO; (not balanced)

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...

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2) ) A student who wants to make the determination of calcium, and he dissolved impure 0.1453 g CaCO3 solid by pretreatment, then precipitated calcium ions by adding ammonium oxalate. He then titrated the released oxalate ions with the adjusted 0.01923 M KMNO4 solution, spending 15 mL of KMNO4 for titration. In this case, find the mass percentage of calcium in the sample. (Ca: 40 g/mol; CaCO3:100 g/mol) 5C,0,2- (aq) + 2MNO4 (aq) + 16H* (aq) > 10CO2 (g) + 2MN2* (aq) + 8H20(aq)
A sample consisting of Na2CO3 and NaHCO3, and inert matter weighs 6.7447 grams. It is titrated with 0.16 N HCI with phenolphthalein as the indicator, and the solution became colorless after the addition of 22.65 mL. Another duplicate sample was titrated with HCI using methyl orange as indicator. It required 56.94 mL of the acid for the color change. What is the percentage of NaHCO3 (84g/mole) in the sample? (Answers should be written in 2 decimals place and do not include the UNIT)
Ca(ClO3)2 (aq) + NH4F (aq) -> CaF2 (s) + ? A.) Determine the product. B.) Balance the equation C.) Write the net ionic reaction D.) Identify the spectator ions
Tungsten trioxide (WO,) has a rich yellow color and is often used as a pigment in ceramics and paints. To test a ceramic vase for its WO, content, a 10.15 g sample of the vase was ground and reduced with Pb(Hg) to convert any WO, to W³+. The resulting W3+ was transferred to 500.0 mL of 1.00 M HCI. A 100.00 mL aliquot of the HCl solution required 14.78 mL of 0.08271 M potassium permanganate (KMNO,) to reach the purple endpoint. A blank required 0.26 mL. Balance the redox reaction. redox reaction: MnO, + W3+ Mn2+ + WO3+ Determine the percent WO, in the ceramic sample. percent WO3: %
3. A 4.912-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced was collected in 3% H₂O₂. Reaction: SO2(g) + H₂O2 → H₂SO4. A 25.00-mL portion of 0.00873 M NaOH was introduced into the solution of H₂SO4, following which the excess base was back-titrated with 15.17 mL of 0.01102 M HCI. Calculate the sulfur concentration in the sample in parts per million.
The amount of protein in a sample of cheese was determined by a Kjeldahl analysis. After digesting a 0.9814-g sample of cheese, the nitrogen is oxidized to NH4+, converted to NH3 with NaOH, and distilled into a collection flask containing 50.00 mL of 0.1047 M HCI. The excess HCI is then back titrated with 0.1183 M NaOH, requiring 22.84 mL to reach the bromothymol blue end point. Report the %w/w protein in the cheese. Conversion factor from nitrogen to protein: General/meats: 6.25 Dairy: 6.38 Cereals: 5.70 Nuts and seeds: 5.30 I may be reproduced for classroom purposes
Solution X containing 0.020 mol of iron(II) sulfate requires 22.5 mL of potassium manganate(VII) for a complete reaction. The equation for the reaction is: 5Fe^2+ + MnO4^- + 8H^+ → Mn^2+ + 4H2O + 5Fe^3+. What is the molarity of the KMnO4 solution?
When 50.0mL of a 0.335M potassium carbonate solution is mixed with 0.045L of a 0.390M nickel(II) chloride solution the following reaction occurs: K2CO3 (aq) + NiCl2 (aq) → a. Complete the reaction equation b. Calculate the mass of precipitate formed c. Calculate the concentration of each ion in the mixture when the reaction is complete
1.
A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach the endpoint, a total of 18.8 mL of HNO3 was required. Given that 0.00639 mol of HNO3 are used in the titration, What quantity in moles of Ca(OH)2 had to be present in the initial reaction?
A 25.00 mL aliquot is withdrawn from the liquid portion of saturated Manganese (II) hydroxide and transferred to an Erlenmeyer flask. After the addition of methyl orange, a titration with 0.0045 M HCl was performed. The endpoint was reached after 8.72 mL of the acid was added. What is the balanced chemical equation? How many moles of hydroxide ions were neutralized in the reaction? What is the molar concentration of hydroxide in the saturated solution? What is the molar concentration of Magnesium ion in solution?
The reaction of sulfuric acid with sodium hydroxide is described by the equation: H₂SO4 + 2NaOH → Na₂SO4 + 2H₂O Suppose 50 mL of NaOH with an unknown concentration is placed in a flask, then a few drops of bromthymol blue were added. A solution of 0.20 M H₂SO4 is dripped into the NaOH solution. After exactly 25.0 mL of H₂SO4 is added, the color changes from blue to yellow. The Titrant in this experiment is