A 3650-mg sample containing bromate and bromide was dissolved in sufficient water to give 250.0mL. After acidification, silver nitrate was added to a 25.00 mL aliquot where the resulting precipitatewas filtered, washed and then redissolved in an ammoniacal solution of potassiumtetracyanonickelate(II) according to the reaction:Ni(CN), + 2 AgBr) → 2 Ag(CN), + Ni? + 2 BrThe liberated nickel ion required 26.73 mL of 0.02089 M EDTA. The bromate ion in a 10.00 mLaliquot was reduced to bromide with As* prior to the addition of silver nitrate. The same procedurewas followed and the released nickel ion was titrated with 21.94 mL of the EDTA solution. Calculatethe percentage of impurity in the sample. Br (79.904)a. 24.45%b.34.38%c. 41.17%d. 65.62%

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Answered: A 3650-mg sample containing bromate and…

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

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A 1.250 g sample of cheese was subjected to a Kjeldahl analysis to determine the amount of protein. The sample was digested, the nitrogen is oxidized to NH₄⁺, and was then converted to NH₃ with NaOH, and distilled into a collection flask containing 50.00 mL of 0.1050 M HCl. The excess HCl is back titrated with 0.1175 M NaOH, this required 21.65 mL to reach the bromothymol blue end point. Report the %protein of the cheese sample, assuming that there are 6.4 grams of protein for every gram of nitrogen. a. 41% b. 91% c. 66% d. 25%
Milk contains lactic acid. Calculate concentration of a 10.0 ml milk sample when it is titrated against 0.09 M of NaOH solution. The pale pink colour was obtained at 13.5 ml. Write the reaction involved
Please explain
Excess solid Ni(OH)2 was added to water and the resulting solution was allowed to stand for several days. The solution was then filtered to remove excess solid Ni(OH)2. A 0.250 L aliquot of the solution was then titrated with 10.54 mL of a standardized 0.000500 M HCl solution. What is the Ksp of Ni(OH)2?
A student dissolved 0.3101 g of Na2C2O4 in 30 mL of water and 15 mL of 3 mol/L H2SO4. She titrated this solution with a KMnO4 solution. What was the molarity of the KMnO4 if it took 24.90 mL of titrant to reach a permanent pale pink equivalence point? The net redox reaction is 2 KMnO4 (aq) + 5 Na2C2O4 (aq) + 8 H2SO4 (aq) → 8 H2O (l) + 10 CO2 (g) + K2SO4 (aq) + 2 MnSO4 (aq) + 5 Na2SO4 (aq) (2 digit response) Answer: 0.037
2. A 0.4912-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced was collected in H2O2. 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 HCl. Calculate the sulfur concentration in parts per million.
What is the precipitate which forms when solutions of Na 3PO 4 and Fe(NO 2) 3 are mixed?
A 1.250 g sample of cheese was subjected to a Kjeldahl analysis to determine the amount of protein. The sample was digested, the nitrogen is oxidized to NH₄⁺, and was then converted to NH₃ with NaOH, and distilled into a collection flask containing 50.00 mL of 0.1050 M HCl. The excess HCl is back titrated with 0.1175 M NaOH, this required 21.65 mL to reach the bromothymol blue end point. What is the reaction for the back titration for this analysis? a. NH₄⁺ + NaOH ⇌ NH₃ + H₂O + Na⁺ b. NaOH + HCl ⇌ NaCl + H₂O c. NH₃ + HCl ⇌ NH₄⁺ + Cl⁻ d. N₂ + 3 H₂ ⇌ 2 NH₃ How many moles of N is present in the cheese sample? a. 544 x 10⁻³ b. 706 x 10⁻³ c. 250 x 10⁻³ d. 794 x 10⁻³ Report the %N of the cheese sample. a. 851% b. 884% c. 033% d. 736%
A 4.908-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced was collected in 2% H2 O2. Reaction: SO2 (g) + H2O2 → H2SO4 A 27.00-mL portion of 0.00826 M NaOH was introduced into the solution of H2 SO4, following which the excess base was back-titrated with 15.15 mL of 0.01165 M HCl. Calculate the sulfur concentration in the sample in parts per million. Concentration ppm
What is the formula for the precipitate formed when Ca(CN)2(aq) reacts with Na3PO4(aq)?
The iron content of iron ore can be determined by titration with K₂Cr₂O₇ according to the equation 14H⁺(aq) + Cr₂O₇²⁻(aq) + 6Fe²⁺(aq) → 6Fe³⁺(aq) + 2Cr³⁺(aq) + 7H₂O(l) Diphenyl amine is used as an indicator as it changes color from green to purple when the endpoint is reached. A sample of iron ore with a mass of 3.255 g was dissolved with HCl and then treated with a reducing agent to convert any Fe³⁺ in the ore to Fe²⁺. Titration with 0.0645 M K₂Cr₂O₇ solution required 45.65 mL of the solution to reach the endpoint. The molar mass of Fe is 55.85 g/mol. Calculate the mass percent iron in the ore.
A sample consisting of Na2CO3 (105.96), NaOH (39.99) and inert matter weighs 1.179 g. It is titrated with 0.300 N HCI with phenolphthalein as the indicator, and the solution becomes colorless after the addition of 48.16 ml. Methyl orange is then added and 24.08 ml more of the acid are needed for the color change. What is the percentage of NaOH and N22CO3? *

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