i Melting point of Nacl is lower than Mgo why? ii. Br is less reactive than F, why? I iil. Complete and balance the following two reactions and derive your conclusion, what do they indicate? a. Al(OH)3s) + H b. Al(OH)as) *+ HO (aq) (ag)

i Melting point of Nacl is lower than Mgo why? ii. Br is less reactive than F, why? I iil. Complete and balance the following two reactions and derive your conclusion, what do they indicate? a. Al(OH)3s) + H b. Al(OH)as) *+ HO (aq) (ag)

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

Chapter21: Transition Metals And Coordination Chemistry

Section: Chapter Questions

Problem 106IP: The ferrate ion, FeO42, is such a powerful oxidizing agent that in acidic solution, aqueous ammonia...

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The ferrate ion, FeO42, is such a powerful oxidizing agent that in acidic solution, aqueous ammonia is reduced to elemental nitrogen along with the formation of the iron(III) ion. a. What is the oxidation state of iron in FeO42, and what is the electron configuration of iron in this polyatornic ion? b. lf 25.0 mL of a 0.243 M FeO42 solution is allowed to react with 55.0 mL of 1.45 M aqueous ammonia, what volume of nitrogen gas can form at 25C and 1.50 atm?
The amount of sodium hypochlorite in a bleach solution can be determined by using a given volume of bleach to oxidize excess iodide ion to iodine; ClO- is reduced to Cl-. The amount of iodine produced by the redox reaction is determined by titration with sodium thiosulfate, Na2S2O3; I2 is reduced to I-. The sodium thiosulfate is oxidized to sodium tetrathionate, Na2S4O6. In this analysis, potassium iodide was added in excess to 5.00 mL of bleach (d=1.00g/cm3) . If 25.00 mL of 0.0700 M Na2S2O3 was required to reduce all the iodine produced by the bleach back to iodide, what is the mass percent of NaClO in the bleach?
Solve 4th and 5th sub questions
One of the steps for refining silver involves converting silver into dicyanoargenate(I) ions: 4Ag(s) + 8CN−(aq) + O2(g) + 2H2O(l) ⟶ 4[Ag(CN)2]−(aq) + 4OH−(aq)Explain why oxygen must be present to carry out the reaction. Why does the reaction not occur as: 4Ag(s) + 8CN−(aq) ⟶ 4[Ag(CN)2−(aq)?
1. Which would you expect to produce an aqueous solution with a lower pH? A 0.1 M solution of Cr(NO3)3, Mo(NO3)2, Fe(NOs)2, or TIO2? Explain your reasoning.
Mass of KxFe(C2O4)y · zH2O : 4.70 g Mass of sample : 0.175 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 7.750 mL V2, volume of standard NaOH required for second equivalence point : 19.70 mL Calculate the mass of iron in the sample :
Mass of KxFe(C2O4)y · zH2O : 4.70 g Mass of sample : 0.175 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 7.750 mL V2, volume of standard NaOH required for second equivalence point : 19.70 mL Calculate the mass of iron in the sample : Calculate the percent of iron in the sample :
How do you find the oxidation numbers of Cr and P in the formula unit Cr(PO4)2?
Why is the oxidation state of Fe 2.5?
5. Write a balanced equation to represent a. the roasting of nickel (II) sulfide to form nickel (II) oxide b. the reduction of nickel(II) oxide by carbon monoxide
2) What are the oxidation state for As and Cl in AsCl from this reaction? 2 As (s) + 3 Cl2 (g) -> 2 AsCl3
Consider the balanced reaction: 2Cr3+(aq)+3PbO2(s)+6H2O(l)→2CrO42-(aq)+3Pb2+(aq)+4H3O+ (aq) a.Which species is the oxidizing agent b.What is the oxidation state of the O in CrO42- c.What is the oxidation state of the Pb in PbO2? d.How many valence electrons are in the CrO42- ion? e. How many moles of electrons, ne, are transferred per mole of this reaction? f. At a certain point the measured free energy is ∆?. Adding more PbO2 will cause the free energy change of the reaction, ∆G, to choose...(Increase, Stay the same, Decrease) g. At a certain point the measured ∆G is –5 kJ/mol. Lowering the pH will cause the free energy change of the reaction, ∆?, to choose... (become less negative, stay the same, become more negative) h. The reaction is used to set up an electrochemical cell. What is true about the cell if the measured voltage is negative? Choose ? < ?, ? = ?, ? > ?, Need more info I. At 298.2 K, this reaction has an equilibrium constant K = 1.6 × 1013 . What is the…