Dissolution of goethite FeOOH ?
952998
The reductive dissolution of goethite ( -FeOOH) and hematite ( -Fe 2 O 3 ) by phenolic reductants has been examined in order to improve the understanding of iron transformations in soils, sediments and aquifers. Rates of goethite reductive dissolution by hydroquinone increased as the pH was increased from pH 1.8 to 4.65, arid the following reaction stoichiometry was obeyed: 2 - FeOOH + QH 2 = 2 Fe 2+ + Q + 4 OH - . As the pH was increased from pH 4.5 to 6.0, the reductive dissolution rate decreased to below the detection limit. At pH 3.4, the reductive dissolution of hematite was two orders of magnitude slower than goethite. The relationship between structure and reactivity was examined for a series of mono-, di-, and tri-hydroxybenzene reductants. Rates of reductive dissolution decreased in the following order: catechol ~- hydroquinone 〉 3,4-dihydroxybenzoic acid 〉 resorcinol-phenol-4-hydroxybenzoic acid.
723259
This lab involves putting iron (steel wool) into a solution of copper sulphate. The reaction produces metallic copper and iron sulphate solution. I've never been really sure if it's iron(II) sulphate or iron(III) sulphate as the product. I've used both equations with good results. \n\n   Fe   +  CuSO4   --->  Cu  +  FeSO4\n   2 Fe   +  3 CuSO4   --->  3 Cu  +  Fe2(SO4)3\n\n\nFor prelab, make up a saturated copper(II) sulphate solution\nTrust me. Otherwise, the kids will be filtering for hours.  \n\nHave containers available for appropriate disposal of reagents. And make sure they clean up all of the bits of steel wool from the lab benches. Those little bits will haunt you for weeks if they don't.\n\n\n\n\nMethod\n\n1. Obtain 100 mL of copper (II) sulphate solution in\n   a clean, dry beaker. \n\n2. Obtain about 10 g of steel wool. Record the exact mass.\n \n3. Place the steel wool into the copper(II) sulphate solution.  Stir with a glass rod. When the solution loses its blue colour, add more copper(II) sulphate solution.\n\n4. Continue stirring (and adding solution, if necessary)until the strands of steel wool are no longer apparent, and only particles of a reddish brown solid are visible.\n\n5. Record the mass of a piece of filter paper.\n   Place it into a funnel.\n \n6. Pour the mixture through filter paper in a funnel.\n   Rinse any residue in the beaker into the filter        paper      with distilled water. Rinse the solid in the filter paper with distilled water.\n\n7. Allow the solid and filter paper to dry, then find the combined mass.\n\n\nAnalysis\n\n1. If iron was the limiting reactant, predict the mass of copper which should have been formed. Show work.\n  \n2. Calculate the percentage difference between  the mass of copper predicted in question 1 and the actual amount of copper produced. Show all work.\n\n3. Discuss possible explanations for your results in question 2.\n\n\n\nGood luck !
103867
NaClO + 2FeSO4 + H2O -> NaCl + 2 Fe(3+) + 2 (SO4)(2-) + 2 OH(1-)
831776
A few are:\nMg, Zn, Al, Fe, and Cu.  They will dissolve at different rates according to the activity series of the metals.
412530
1) H3COCH3 (or C2H6O) + 3O2 (g) --> 2CO2 (g) + 3H2O (g)\n2) HNO2 (aq) + NaOH (aq) <--> NaNO2 (aq) + H2O (l)\n3) 2K+ + Cr2O7(2-) + Fe(NO3)2 + 2H+ <--> CrO4(-) + Fe3+ + 2K+ + 2NO3(-) \n4) Na3PO4 + NH4NO3 = No reaction, all soluble salts.\n5) 2HCl (aq) + Na2S (s) --> 2NaCl (aq) + H2S (g)
838309
b a solution, the salt will dissolve
770691
CoCl2(aq) + FeSO4(aq) = CoSO4 (aq) + FeCl2(aq)
599313
Refer to the electrohemical series (see source).  The answer depends on whether the conditions are such that iron is oxidized to Fe2+ or Fe3+.  In the case of iron metal being oxidized to Fe2+, the correct order is:\n\nMg, Zn, Fe, Sn, Pb
425555
this depends on what you analysis is for.\n\nI presume you are using HCl and HNO3 (this mixture is aqua regia, and is an old mixture used by alchemists to dissolve metals) which would produce a solution containing metals contained in the flyash. This is the safest method.\n\nFurther analysis for getting rid of organics and further getting to the metals (flyash is made of coal) is also dangerous, as it uses H3PO4 and HNO3, this combination if heated is explosive so should be done by experienced chemists.\n\nNow... if you want to analyise the actual organic components in flyash then this beocmes more difficult as you now are dealing with highly complex organic structures... you should be careful with acid as it could destroy a lot of the flyash molecules. Such analysis is complicated, requiring many steps.
821724
Rusting of iron is an oxidation/reduction process which means there is a transfer of electrons.  Any soluble ionic compound will facilitate the transfer of the electrons and accelerate the oxidation process.
308525
Yes.  If carried to the extreme, you would see the aluminum strip dissolve, copper metal precipitating, and the solution color will fade from blue to colorless.\n\n2Al + 3Cu(2+) ---> 2Al(3+) + 3 Cu
590452
(NH4)2 SO4  + (FeSO4)2 + 2H2O____(\nNH4)2SO4Fe2(SO4)3.24H2O\n\nAmmonium ferric sulphate
476743
Rust is made of Iron (III) Oxide, not pure iron.  As for its crystal structure, I'm not completely sure.
1187122
ferric oxide, or rust, is the product
861653
treat the mixture with sodium carbonate solution and then filter it to separate iron. the filtrate contains sodium benzoate. Liberate benzoic acid by just adding any mineral acid like sulfuric acid. Then u will get the crystals of benzoic acid. This can be filtered off
893153
2Fe (s) + 3F2 (g) ---> 2FeF3(s)
812692
Ferric sulfite, or iron (III) sulfite