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![1. Name the following compound and create ionization, linkage and optical isomers: [Au(SCN)2(en)2]CI
2. Calculate the value of pK. for lead(II) bromide. One liter of the saturated solution contains 1.1817.10-2 mol of
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- Chemistry how to calculate the formation constant Kf for an iron:phenanthroline complex assuming 0.01% of the iron remains unreacted. the complex formed in the 1:4 iron:phenanthroline molar ratio. initially 9E-6moles iron and 0.015M phenanthroline please help. no idea how to do this.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…The complex formation reaction is given by: Ca^2+ + EDTA = CaY^2- 1.Calculate the concentration of free Ca^2+ in a solution of 0.10M CaY^2- at pH 10.00,given that the formation constant for CaY^2- is 10^10.65 and aY4- =0.30 at a pH of 10.00 2.How would the amount of Ca^2+ in the solution change if the pH of the solution was lowered to the pH of 6.(Note:it is not necessary to do the calculation)
- For the aqueous complex at Fe (CN)6]4-complex Kf= 1.0 x 10^35 Suppose equal volumes of 0.0062M Fe(NO2) solution and 0.10M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Fe^2+ ion. Round your answer to 2 significant digits.Question 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 Conclusion: Describe why each shift occurred using proper terminology1. The solubility of Ag₂SO₄ in water at 25 °C is 0.0155 M. What is Ksp for Ag₂SO₄? 2. What is the solubility of La(IO₃)₃ in a solution that contains 0.100 M La³⁺ ions? (Ksp of La(IO₃)₃ is 7.5 × 10⁻¹²)
- Consider the following reaction:Al + 3KOH + 3H2C2O4 ∙ 2H2O → K3Al(C2O4)3 ∙ 3H2O + 6HO + (3/2)H21.00 g 20.0 mL 14.0 g6.00 M What is the theoretical yield of the complex formed in the reaction?A solution is prepared such that the initial concentration of A2+ is 1.50×10-3 M and the initial concentration of X is 4.60×10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9×10-4 M. A2+ (aq) + X (aq) AX2+ (aq) What is Kf, the formation constant, for this complex?7.00 grams of Cobalt (II) nitrate are dissolved in 1.00 liter of water. What is the initial concentration of CO (2+) in moles per liter? Then, 0.22 moles of solid KOH are added to this solution. The solution volume remains 1.00 liter. Given that Kf = 5.0 x 10^9 for the complex ion, Co(OH)4 (2-) find the final concentrations of Co (2+), Co(OH)4 (2-), and OH-. Also find the pH of this final solution.