If the instantaneous concentrations are [A] = 50 μM, B= 10 μM, [A.B] = 5μM, what's the rate of change of the complex d[AB]/dt (μM/s) the options are: a. 46800 b. 0.0468 c. 53200 d. 50000
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- 6. The amount of nickel (FM 58.693) in steel can be determined with the precipitating agent dimethylglyoxime (DMG, C4H8O2N2, FM 116.12). The steel is dissolved in acid, the solution is neutralized, then the DMG is added to precipitate the nickel as the complex bis(dimethylglyoximate)nickel(II) (Ni(C4H7O2N2)2, FM 288.91) according to this reaction: Ni2+(aq) + 2C4H8O2N2(aq) → Ni(C4H7O2N2)2(s) + 2H+(aq) DMG has limited solubility in water and may precipitate with the complex, so it is important to avoid adding an excess of the precipitating agent. a) If the mass percent of nickel in a certain steel sample is believed to be approximately 2.0%, what volume of 1.0 wt% dimethylglyoxime solution with a density of 0.83 g/mL should be used with a 1.5-g steel sample to give a 25% excess of DMG? b) If a 1.458 9-g sample of steel produced 0.150 6 g of precipitate, what was the mass percent of nickel in the sample?A 2.00 mL solution of 0.00800 M Fe(NO3)3 is mixed with 3.00 mL of 0.00300 M NaSCN to form the blood red FeSCN2+ complex. Calculate the concentration of Fe3+ in the combined solution before any formation of the complex.How do you figure out the function of complexed and uncomplexed Fe3+as a function of log(SCN-) in the reaction: (Fe3+)+(SCN^-)=(Fe(SCN)2+ ) The formal question is: Use the value of K eq determined in this experiment to calculate the fraction of Fe(III) that is complexed and the fraction of Fe(III) that is uncomplexed in solutions containing a large excess of thiocyanate ion over Fe(III). Begin by deriving an algebraic equation for these fractions (i.e., f comp and f uncomp) as a function of thiocyanate concentration. I do not need numbers. I just want to know how to approach this problem.
- Sequential formation constants for the water molecule substitution reactionby Br- ions in the hexaaquacadmium complex ion (II) are: Kf1 = 36.3; Kf2 = 3.47; Kf3 = 1.15; Kf4 = 2.34.Explain the factors that influence the formation constant and why Kf4 is greater than Kf3.25c. At a particular temperature, the solubility of In₂(SO₄)₃ in water is 0.0068 M. You have found Ksp to be 1.6 × 10⁻⁹. If solid In₂(SO₄)₃ is added to a solution that already contains 0.150 M In(NO₃)₃, what will the new solubility of the solid be?For a lab to determine the aquation rate of [Co(NH3)5Cl]Cl2: I put 0.05 M HNO3, 0.10 M HNO3, and 0.30 M HNO3 in three different flasks. To each solution, add sufficient [Co(NH3)5Cl]Cl2 to give a 1.2x10-2 M complex concentration. Please explain how to determine how much [Co(NH3)5Cl]Cl2 to add to each solution/flask.
- This is the lab with my data sheet and please answer all of them. Thank you 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 colourThis is the lab with my data sheet and please answer all of them. Thank you 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 What species is responsible for the observed colour change when KSCN(aq) and Fe(NO3)3(aq) are mixed? What can be concluded about the system based on your ~1 minute observation of the mixture. what does the addition of the solid do to the [SCN-(aq)]? What can you infer about the system from the colour change of the solution? How can this be possible if no additional Fe3+(aq) has been introduced?This is the lab with my data sheet and please answer all of them. Thank you 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 question: What can you infer about the system from the colour change of the solution? How can this be possible if no additional Fe3+(aq) has been introduced? What does the addition of the solution do to the [Fe3+(aq)]?
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