None b. (i)A green solid has the empirical formula FeBr3-5NH3 H₂O. Upon reaction withan excess of aqueous AgNO3 it is found that 1 mole of the solid precipitates 3moles of AgBr. Heating the green solid leads to loss of 1 mole of H2O to yielda blue solid with the same ratio of Fe:Br:NH3 as found in the green solid.The reaction of 1 mole of the blue solid with excess of aqueous AgNO3produces 2 moles of AgBr. Draw and name the octahedral green and bluecomplexes.[2 marks]

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Answered: b. (i) A green solid has the empirical…

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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A 4.912-g sample of a petroleum product was burnedin a tube furnace, and the SO2produced was collectedin 3% H2O2.Reaction:SO2(g)+H2O2→H2SO4A 25.00-mL portion of 0.00873 M NaOH was introducedinto the solution of H2SO4, following whichthe excess base was back-titrated with 15.17 mL of0.01102 M HCl. Calculate the sulfur concentrationin the sample in parts per million.
A pink solid has the formula CoCl3 5NH3 H2O. A solution of this salt is also pink and rapidly precipitates 3mol AgCl(s) on titration with silver nitrate solution. When the pink solid is heated, it loses 1mol H2O to give a purple solid with the same mole ratio of NH3:Cl:Co as the pink solid. The purple solid releases two of its chloride ions rapidly; then on dissolution and titration with AgNO3, release one of its chloride ions slowly. Deduce the structures, draw and name 2 octhahedral complexes
What is the water solubility of BaCO3 (Kep = 2.6 x 10-9) in a solution containing 0.40 M CO, (aq)? %3D
The digestion of a 0.1432 g sample of a compound containing phosphorous in a mixture of HNO3 and H2SO, resulted in the formation of CO2, H2O and H3PO4 Addition of ammonium molybdate yielded a solid having the composition (NH)3PO, 12M0O3 (MW=1876.3 g/mol). This precipitate was filtered washed, and dissolved in 50 00 mL of 0.2000 M NaOH: (NH,)3PO4-12MO03(s)+ 26OH (aq) HPO,2 (aq) +12M00,2 (aq) +14H2O(1) + 3NH3(g) After the solution was boiled to remove NH3, the excess NaOH was titrated with 14.71mL of 0.1741 M HCI to a phenolphthalein end point (back titration). Calculate the percentage of phosphorous in the solid sample. 6.19% 10.6% O 27.6% O0 238% O 19.5
2. An iron ore was analyzed by dissolving a 1.1324 g sample in concentrated HC. The resulting solution was diluted with water, and the iron(III) was precipitated as hydrous oxide Fe,03 .XH20 by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.5394 g of pure Fe,03 (FW = 159.69). Calculate (a) the percent Fe (FW = 55.847) and (b) the percent Fe;04 (FW = 231.54) in the sample.
Like heavy water (D₂O), so-called “semi-heavy water”(HDO) undergoes H/D exchange. The scenes below depict aninitial mixture of HDO and H₂ reaching equlibrium.(a) Write the balanced equation for the reaction. (b) Is the valueof Kgreater or less than 1? (c) If each molecule depicted repre-sents 0.10 M, calculate K.
A scientist was tasked to extract Fe from an aqueous suspension that contains 106 g of Fe2O;. The following steps detail the transformation of Fe,O; (a9) to elemental iron. I Enough sulfur trioxide gas was bubbled to Fe,O; aqueous suspension to completely yield ferric sulfate. IL Then, 5.00 M nitric acid was added to ferric sulfate yielding aqueous solution of ferric nitrate I. Excess magnesium powder was added to the aqueous solution of ferric nitrate precipitating the solid iron. and the type of chemical reaction for [I], [II], [III]. Do not forget to indicate the states of the reactants and products а. Write the balanced chemical reaction (s, 1, g). (CHOICES: COMBINATION, SINGLE DISPLACEMENT, DOUBLE DISPLACEMENT) b. What is the final mass of iron? Express your answers in 3 significant figures. High-concentration HCl is supposed to be added at the last part of the procedure. с. Briefly state its purpose.
4- Mo in a 0.2711 g sample was precipitated giving 1.1682 g of (ΝH)2PO,. 12 MoO Find percentage Mo , P (at wt = 30.97) .N=14,Mo= 95.9,H=1 , O= 16
3. Write balanced formula equations for each of the following reactions. Physicai states of reactants and products need not be shown. (i) The combustion of ethane gas, C2H6, in excess air to form carbon dioxide and water. (ii) oxide andcarbon dioxide. The decomposition of solid całcium carbonate by heat to form calcium (iii) The decomposition of hydrogen peroxide to form water and oxygen(iv) The reaction of iron with chlorine to form iron(III) chloride.
5. 0.1500 g sample of chromium ore was dissolved and the chromium oxidized to chromate ion. The solution was treated with 25.00 mL of 0.3500 M AGNO3. The resulting precipitate, from the reaction of the excess and analyte in 1: 1 mole relationship, Ag2CrO4 was removed and discarded. The excess AGNO3 required 30.50 mL of 0.200 M KSCN for titration in a 1:1 mole relationship. Calculate the % Cr2O3 in the ore if the mole relationship between Cr2O3 and CrO42- is 1:2 respectively.
The digestion of a 0.1159 gram sample of a phosphorous-containing compound in a mixture of HNO3 and H2SO4 resulted in the formation of CO2, H2O, and H3PO4. Addition of ammonium molybdate yielded a solid having the composition (NH4)3PO4·12MoO3 (FW = 1876.3). This precipitate was filtered, washed, and dissolved in 50.00 mL of 0.2000 M NaOH: (NH4)3PO4•12MoO3(s)+26OH-(aq)->HPO42-(aq)+12MoO42-(aq)+14H2O(l)+3NH3(g) After the solution was boiled to remove the NH3, the excess NaOH was back-titrated with 14.84 mL of 0.1626 M HCl to a phenolphthalein end point. Calculate the percent phosphorous (FW = 30.9737) in the sample.
An aqueous solution of SO2 reduces (a) aqueous KMnO4 toMnSO4(aq), (b) acidic aqueous K2Cr2O7 to aqueous Cr3 + ,(c) aqueous Hg2(NO3)2 to mercury metal. Write balancedequations for these reactions.

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