Formula Positive ion Negative ion Name Cu2S Cu+ S2- Copper(I) sulfide Fe203 Iron(III) Oxide CuCl2 Copper(II) Chloride Fes Ferrous Sulfide Ag20 Silver(1) Oxide FeBr2 Iron(1I) Bromide
Q: 15). Write the name of each of the following ionic substances, using -ous or- ic endings to indicate…
A: The suffixes are placed on the bases of their ionic charge. Like prefix-suffix of acid are in order…
Q: Name Iron(III) chloride Iron(II) oxide |Copper(I) sulfide Positive Ion Negative Ion Formula Fe+ CI…
A: i am supposed to answer only one question from the above so pls do repost for the next question.
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A: We have give names. As per rule, only 3 subparts can be attempted.
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A: Name and formula of molecules.
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Q: Which of the following is the correct name for N2O5 Dinitrogen Hexoxide Nitrogen Oxide…
A: The correct name for N2O5 is given in step two.
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Q: 3. Names of ionic compounds Formula Positive ion Negative ion Name Cu,S Cu* |Copper(I) sulfide Fe,O3…
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Q: FeSO4 + Potassium phosphate à Iron (II) phosphate + K2SO4 Write the chemical formula for…
A: Given reaction is, FeSO4 + Potassium phosphate ----> Iron (II) phosphate + K2SO4
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A: Applying rule of IUPAC nomenclature of inorganic compounds.
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A: On careful observation of the table following points can be inferred :
Q: dinitrogen
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- A 3.03-g petroleum specimen was decomposed by wet ashing and subsequently diluted to 500 mL in a volumetric flask. Cobalt was determined by treating 25.00-mL aliquots of this diluted solution as follows: Assume that the Co(II)-ligand chelate obeys Beer’s law, and calculate the percentage of cobalt in the original sample.The accompanying data (1.00-cm cells) were obtained for the spectrophotometric titration 10.00 mL of Pd(II) with 2.44 10-4 M Nitroso R(O. W Rollins and M. M. Oldham, Anal. chem .,1971, 43, 262, DOI: 10.1021/ac60297a026). Calculate the concentration of the Pd(II) solution, given that the ligand-to-cation ratio in the colored product is 2:1For the aqueous [PbC1]2- complex K=2.5 × 10^15 at 25 °CSuppose equal volumes of 0.0014 M Pb(NO), solution and 0.20 M KCI solution are mixed. Calculate the equilibrium molarity of aqueous Pb2+Round vour answer to 2 sianificant digits
- Ammonium iron(II) sulfate crystals have the following formula: (NH4)2SO4.FeSO4.nH2O . In an experiment to determine n 8.492g of the salt were dissolved and made up to 250cm^-3 of solution with distilled water and sulphuric acid. A 25.0cm^-3 portion of the solution was titrated against 0.0150 mol dm^-3 KMnO4. A volume of 22.5cm^-3 was required. Find the value of n1. A Cr3+ solution is electrolyzed using a current of0.365 A. What mass of Cr(s) (51.9661) is plated outafter 10 hours?2. When an aqueous solution of CuSO4 is electrolyzedcopper metal is deposited. If a constant current waspassed for 5.00 h and 404 mg of Cu (63.546) metal wasdeposited, what was the current?complex formation equilibria with Ag+ for EDTA, CN-, NH3, I-
- A 25.00 mL aliquot of a solution containing Cu2+ and Fe3+ was titrated with 17.08 mL of 0.05095 M EDTA. A second 25.00 mL aliquot of the Cu/Fe mixture was treated with NaF to form a stable iron-fluoride complex. This mixture was then titrated with EDTA and the endpoint volume was found to be 5.47 mL. Calculate the amounts of Cu2+ and Fe3+ in mg/L. Molar mass (g/mol): Fe = 55.85 and Cu = 63.55Write the formula for each complexion or coordination compound- Hexa-aqua-nickel(II) chloride-,. penta-carbony-lchloromanganese(I),. ammonium diaquatetrabromovanadate(III), tris(ethylenediamine)cobalt(III) trioxalatoferrate(III)?When I was a boy, I watched Uncle Wilbur measure the iron content of runoff from his banana ranch. He acidified a 25.0-mL sample with HNO3 and treated it with excess KSCN to form a red complex. (KSCN itself is colorless.) He then diluted the solution to 100.0 mL and put it in a variablepathlength cell. For comparison, he treated a 10.0-mL reference sample of 6.80 3 1024 M Fe31 with HNO3 and KSCN and diluted it to 50.0 mL. The reference was placed in a cell with a 1.00-cm pathlength. Runoff had the same absorbance as the reference when the pathlength of the runoff cell was 2.48 cm. What was the concentration of iron in Uncle Wilbur’s runoff ?
- The concentration of iron in a solution can be determined using UV?Vis spectrophotometry by reacting the iron with 1.10-phenanthroline to produce a colored complex. The following data were obtained for a series of standard solutions of iron/1,10-phenanthroline complex measured in a 1.00 cm cell. Concentration (M) Absorption 0.50x10-4 0.109 1.0x10-4 0.218 2.0x10-4 0.436 3.0x10-4 0.656 4.0x10-4 0.872 a.Prepare a Beer’s law plot using the above data b.Calculate the concentration of an iron 1, 10-phenanthroline complex solution that has an absorbance of 0.317 c.Calculate the molar absorptivity of the iron/1, 10-phenanthroline complexMatching Type a monodentate ligand a bidentate ligand a hexadentate a chelating indicator a polydentate a metal ligand complex ion A. ammonia B. silver diammine C. EBT D. ethylenediaminetetraacetic acid E. oxalateGiven A, B, and C… [A] U(VI) as uraninite; UO2 (where Fe2+= reductant; Fe(OH)3 ferrihydrite= product): 2Fe2+ + UO22+ +3H2O + H+ ---- > 2Fe(OH)3 + U4+ +2H2O [B] U(VI) as uraninite; UO2 (where Mn2+= reductant; MnO2 pyrolusite= product): 2H2O + UO22+ + Mn2+ ---- > UO2 + B - MnO2 + 4H+ [C] U(VI) as as uraninite; UO2 (where HS-= reductant; S0= product): UO22+ + Hs- ---- > UO2 + S + H+ QUESTION: Use thermodynamic calculations [use redox potential (Eh)] to predict which of the three reductants below is most favorable at pH 3 ? (1) Fe2+ (2) Mn2+ (3) HS-
