A lab student analyzed his/her cool nickel-en complex for ethylenediamine, en, content.ted g sample of the synthesized Ni-en complex was dissolved in about 50 mL of water and tirated with 0.186 M HCl (aq). Endpoint required 20.16 mL of the HCI (ag). What is the mass (in grams) of en in the Ni-en complex analyzed? Show ALL work
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- Ammonia and potassium iodide solutions are added to an aqueous solution of Cr(NO3)3. A solid is isolated (compound A), and the following data are collected: i. When 0.105 g of compound A was strongly heated in excess 0 2, 0.0203 g CrO3 was formed. ii. In a second experiment it took 32.93 mL of 0.100 M HCI to titrate completely the NH3 present in 0.341 g compound A. iii. Compound A was found to contain 73.53% iodine by mass. iv. The freezing point of water was lowered by 0.64C when 0.601 g compound A was dissolved in 10.00 g H2O (Kf =1.86Ckg/mol). What is the formula of the compound? What is the structure of the complex ion present? (Hints: Cr3+ is expected to be sixcoordinate, with NH3 and possibly I as ligands. The I ions will be the counterions if needed.)Fill in the blanks : (i) When a ligand has a two-complexing or donor group in its structure, it is said to be————— (ii) ___________are compounds whose colour changes when they bind to a metal ion. (ii) If you double the wavelength, you will observe. ________the energy. (iv) In_____________ titration, we monitor changes in absorbance during the titration to find out the equivalence point. (v) Two liquids are_____________ if they form a single phase when they are mixed in any ratio. (vi) The efficiency of Chromatographic Columns can be described by____________Equation.Give an example of a double salt that can be formed via ligand exchange and give the reactions involved
- Why is the pH of the medium important for the formation of chelated complexes between metal ions and ligands? Choose the best answer: Select one: a. Because the ligands give rise to acid-base reactions that influence the stability of the chelate b. Because if the pH is not very acidic, the ligands do not protonate and the complex cannot form c. Because the pH of the medium is always important for any type of reaction. d. Because in the absence of pH there is no reaction of any kindChemistry A lab student analyzed her nickel-en complex for ethylenediamine, en, content. A 0.288 g sample of the synthesized Ni-en complex was dissolved in about 50 mL of water and titrated with 0.154 M HCl (aq). Endpoint required 27.02 mL of the HCl (aq). What is the mass (in grams) of en in the Ni-en complex analyzed?This is the lab with my data sheet and please answer all of them. Thank you and please answer all of them. If you do it would be appreciated My data to support answers for questions. The equilibrium is Fe3+ + SCN- <--> [FeSCN]2+. The Fe3+ is a pale yellow colour and the complex ion product is red.Stresses:Add KSCN - turned deep redAdd Fe(NO3)3 - turned deep redAdd Na2CO3 - turned yellow/colourlessAdd NaOH - turned yellow/colourlessAdd NH3 - turned yellow/colourlessHeat - turned lighter orange colourCold - turned darker orange colour Addition of NH3(aq) to test tube #6: As a result of the colour change, what can be concluded about the [FeSCN2+(aq)]? Explain. Explain why the addition of NH3(aq) affects the [FeSCN2+(aq)] as indicated in (a). Use chemical reaction in your explanation. Addition of heat/cold to test tube #7 & 8: As a result of the colour change, what can be concluded about the [FeSCN2+(aq)] when the temperature is increased? Explain. As a result of the colour…
- This is the lab with my data sheet and please answer all of them. Thank you and please answer all of them. If you do it would be appreciated My data to support answers for questions. The equilibrium is Fe3+ + SCN- <--> [FeSCN]2+. The Fe3+ is a pale yellow colour and the complex ion product is red.Stresses:Add KSCN - turned deep redAdd Fe(NO3)3 - turned deep redAdd Na2CO3 - turned yellow/colourlessAdd NaOH - turned yellow/colourlessAdd NH3 - turned yellow/colourlessHeat - turned lighter orange colourCold - turned darker orange colour Addition of heat/cold to test tube #7 & 8: As a result of the colour change, what can be concluded about the [FeSCN2+(aq)] when the temperature is increased? Explain. As a result of the colour change, what can be concluded about the [FeSCN2+(aq)] when the temperature is decreased? Explain. What can you conclude about the reaction (i.e. is it endothermic or exothermic) based on the above results?This is the lab with my data sheet and please answer all of them. Thank you and please answer all of them. If you do it would be appreciated My data to support answers for questions. The equilibrium is Fe3+ + SCN- <--> [FeSCN]2+. The Fe3+ is a pale yellow colour and the complex ion product is red.Stresses:Add KSCN - turned deep redAdd Fe(NO3)3 - turned deep redAdd Na2CO3 - turned yellow/colourlessAdd NaOH - turned yellow/colourlessAdd NH3 - turned yellow/colourlessHeat - turned lighter orange colourCold - turned darker orange colour Addition of Na2CO3(s) to test tube #4: d) Explain why the addition of Na2CO3(aq) affects the [FeSCN2+(aq)] as indicated in (a). Use a chemical reaction in your explanation. Addition of NaOH(aq) test tube #5: e) As a result of the colour change, what can be concluded about the [FeSCN2+(aq)]? Explain. f) Explain why the addition of NaOH(aq) affects the [FeSCN2+(aq)] as indicated in (a). Use a chemical reaction in your explanation.This is the lab with my data sheet and please answer all of them. Thank you and please answer all of them. If you do it would be appreciated My data to support answers for questions. The equilibrium is Fe3+ + SCN- <--> [FeSCN]2+. The Fe3+ is a pale yellow colour and the complex ion product is red.Stresses:Add KSCN - turned deep redAdd Fe(NO3)3 - turned deep redAdd Na2CO3 - turned yellow/colourlessAdd NaOH - turned yellow/colourlessAdd NH3 - turned yellow/colourlessHeat - turned lighter orange colourCold - turned darker orange colour Addition of Fe(NO3)3(aq) to test tube #3: a) what can you infer about the system from the colour change of the solution? b)How can this be possible if no additional SCN-(aq) has been introduced? Addition of Na2CO3(s) to test tube #4: c) As a result of the colour change, what can be concluded about the [FeSCN2+(aq)]? Explain. d) Explain why the addition of Na2CO3(aq) affects the [FeSCN2+(aq)] as indicated in (a). Use a chemical reaction in your…
- Write a complete and balanced redox equation for the synthesis of the coordinationcompound. Use iron(II) oxalate (the yellow/orange solid) as a reactant. In other words,complete the following reaction: FeC2O4(s) + H2O2(aq) + ??? → product(s) Assume that the net reaction occurs in an acidic solution: this will make balancing theequation easier. Use the formula of the iron (III) oxalate compound that you found in theliterature to balance the equation ([Fe(C2O4)3]). You must write out the individual half-reactions.Predict how altering the ligand donor/acceptor characteristics will affect Δo and how this is can be seen in the spectrochemical series.i) Silver ion (Ag+) reacts with SCN- ion to form silver thiocyanate (AgSCN). What change will the student observe when a solution containing Ag+ ion is added to the mixture? ii) Briefly explain how your answer to is consistent with Le Chatelier’s principle.