Week 13 Recitation worksheet (Copper in penny, Lab 10)

What charge and how many ‘d’ electrons does copper have in [Cu(OAc)2(H2O)]2 ?

An ore containing magnetite, Fe3O4, was analyzed by dissolving a 1.5419-g sample in concentrated HCl, giving a mixture of Fe2+ and Fe³+. After adding HNO3 to oxidize any Fe²+ to Fe³+, the resulting solution was diluted with water and the Fe³+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 0.8525 g of pure Fe₂O3. Calculate the %w/w Fe3O4 in the sample.

Assign a systematic name to each of the following chemical compounds. Compound Name (a) Na[Mn(CN)5l fill in the blank 1 (b) [Cu(bipy)2l]NO3 fill in the blank 2 (c) [Fe(CO)5] fill in the blank 3 (d) [Cr(NH3)3(CN)3] fill in the blank 4

1. A sample of iron ore weighing 0.6428 g is dissolved in acid The iron is reduced to Fe*2 and titrated with 36.30 mL of a 0.1052 N solution of K2Cr207. (a) Calculate the percentage of iron (Fe) in the sample. (b) Express the percentage as Fe,03 rather than Fe. Hint: The reaction of Fe2+ with Cr,0,2 involves one electron to oxidize it to Fe*.

An ore containing magnetite, Fe3O4, was analysed by dissolving a 4.9 g sample in concentrated HCl, giving a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize any Fe2+ to Fe3+, the resulting solution was diluted with water and the Fe3+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 2.8 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample (Fe3O4 =231.54 g/mol, Fe2O3 = 159.69 g/mol)

3. For the substitution of [Mn(OH;)6J** to form [MnX(OH2)s]*, what experiments could you design to determine if the reaction is d or a?

Use the data provided for stock concentration and mass to calculate the concentrations of each solution.  Solution A) A stock solution of 0.0100 M solution of K3[Fe(CN)6] is provided. Calculate the volume of the stock solution needed to prepare 100.0 ml of .00200 M K3[Fe(CN)6]. Deionized water should be used to dilute the solution. Solution B) Calculate the volume of solution A needed to prepare 50.0 ml of .0010 M K3[Fe(CN)6]. Deionized water should be used to dilute this solution.

Write the balanced NET ionic equation for the reaction when NH₄Cl and Cu(C₂H₃O₂)₂ are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.

How does potassium ferrocyanide K4[Fe(CN)6] prevent any pre-oxidation of the copper(I) ions in quantitative benedict's test?

1) List an oxidizing agent that will: a) oxidize Cu to Cu*2, without oxidizing Cu to Cu*1. b) oxidize Mn to Mn*2, without oxidizing Mg to Mg*2. c) oxidize Br1 to Br2, without oxidizing H20 to O2 with H*1 d) oxidize Cr(OH)3 with OH1 to CrO42, without oxidizing NO21 with OH1 to NO31. e) oxidize La to La*3, without oxidizing Al to Al*3.

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For which of the following starting materials would there be NO reaction: Mn (s) + FeO Mg (s) + Al2S O Cd (s) + Zn(CzH3O2)2 Fe (s) + AGNO3 All will react

5. Copper(II) with Ammonia, NH3 Three equilibria are occurring. ⚫ [Cu(H2O)6]2+(aq) + 2 NH4OH Cu(OH)2(s) . light blue • white solid + 2 NH4*(aq) white precipitate Cu(OH)2(s) + 4 NH3 [Cu(NH3)]4] 2*(aq) + 2 OH-(aq) royal purple -> • H2SO4(aq) + 2 NH4OH(aq) → 2 H2O + 2 NH4+ (aq) + SO4² (aq) neutralization of NH3 NH4*(aq) A. Explain what happen in the first 2 reactions as ammonia is added. Use the equilibria in the equations.

2) a) Write the chemical equation for the dissociation of [Cu(NH3)4]2+ d) Calculate the concentration of free, uncomplexed Cu2+ ions in a solution that originally contains a total of 1.0 × 10-3 M copper (II) ions and an equilibrium concentration of 0.10 M NH3.

Consider the reactions 1. [Cr(H2O)6]** + [C©CI(NH3)s]* → [Co(NH3)s(H2O)]²* + [CrCl(H2O)s]** 2. [Fe(CN)6]* + [Mo(CN)s]-→ [Fe(CN)6]³¯ + [Mo(CN)8]* Which one of the following is the correct statement? (i) Both involve an inner sphere mechanism (ii) Both involve an outer sphere mechanism (iii) Reaction 1 follows inner sphere and reaction 2 follows outer sphere mechanism (iv) Reaction 1 follows outer sphere and reaction 2 follows inner sphere mechanism (A) i (B) ii (C) iv (D) ii

What is the concentration of [Cd2+ (aq)] in a solution made by dissolving 0.020 mol of Cd(NO3)2 in 400 mL of a solution of KCN that is 0.50 M at equilibrium? Kf of [Cd(CN)4]2− = 3.0 × 1018

Write a balanced equation for the reaction between the dichromate ion and zinc metal to yield zinc(II) and chromium(II) in acidic solution. [SHOW ALL STEPS) Zn(s) + Cr20,2 (aq) --> Zn²* (aq) + Cr³+(aq)

How are the acetates bound to copper in [Cu(OAc)2(H2O)]2 ?

Consider the equilibrium reaction below. [Cu(H₂O)6]²+ (aq) + 4 Cl (aq) light blue [CuCl4]² (aq) + 6 H₂O (1) orange A test tube contains a solution of Cu(NO3)2 which is light blue. What is the major species present in the solution responsible for the color?

1. A sample of iron ore weighing 0.6428 g is dissolved in acid The iron is reduced to Fe* and titrated with 36.30 mL of a 0.1052 N solution of K,Cr207. (a) Calculate the percentage of iron (Fe) in the sample. (b) Express the percentage as Fe,03 rather than Fe. Hint: The reaction of Fe2+ with Cr,0,2 involves one electron to oxidize it to Fe*.

Question 3a and 3b

help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working

The equilibrium-constant expression for the reaction Ti (s) + 2CI 2 (g) TICI 4 (1) is given by O [Ti (s)] [Cl2 (g)F [TIC14(1}] [TIC14 (1)] [Ti (s)] [Cl2( g))? [TIC14 (1)] [Ti (s)] [Cl2 (g)] O [TIC14 (1)] [Cl2 (g))? O [Cl2 (g)]2

what happens when you add polished magnesium to each of these solutions : - Al2(SO4)3 -Cu(NO3)2 -Fe(NO3)3  -Zn(NO3)2

Why are there two separate H2O exchange rates observed for [Cu(H 2 O)6]^ 2+ in aqueous solution ? take into account any potential structural "distortions"

Excess of Cu(s) is added to 2.00M solution of Cr3+(aq). Given that: Cr2+(aq) + Cu+ (aq)  Cu (s) + Cr3+ (aq) What are the equilibrium concentrations of the species in solution if at a given temperature Kc = 7.20?

a) Apply MOT to describe bonding in [Fe(H2O)6]³+ and [Fe(CN)6]³- b) Describe extraction of uranium from its ores.

Balance this equation and balanced reaction equation and the quantities included in the procedure to calculate the theoretical yield of K[Cr(C2O4)2(H2O)2]·2H2O.

Dichromate, Cr2O7 2– , and permanganate, MnO4 – , are both common oxidising agents. When mixed, would acidified dichromate oxidise Mn2+ or would acidified permanganate oxidise Cr3+? Explain what you think would happen and write a chemical equation to show this.

what happens when you add polished magnesium to each of these solutions (describe the products for example  what is the color of the solution) : - Al2(SO4)3 -Cu(NO3)2 -Fe(NO3)3  -Zn(NO3)2

Compensate for the following redox reactions using the half reaction method?   In Acidic Solution;   (Fe(CN)6)3- + N2H4         --->            (Fe(CN)6)4- + N2   In Basic Solution;   CrO42- + S2O42-            --->     Cr(OH)3  + SO32-

For the reaction: CuSO4 + NH4OH , [Cu(NH3)6]SO4 + HOH, how many grams of [Cu(NH3)6]SO4 can be produced from 3.08 moles of copper (II) sulfate?

If 2.50 g of CuSO4 is dissolved into 9.0 x 10² mL of 0.30 M NH3, what are the concentrations of Cu²+, [Cu(NH3)4]2+, and NH3 at equilibrium? Note: K₁ for [Cu(NH3)4]2+ is 5.0 × 1013.

For Cd(OH)2, Ksp = 5.9 × 10–15. For [Cd(CN)4]2– Kf = 3 × 1018. What is the molar solubility of Cd(OH)2 when it's dissolved in a 0.23 M NaCN solution? Please round to 2 decimal places. Only report the numerical value, without the unit.