2.Which way will the equilibrium shift (left or right) in the reaction below:Fe3+(aq, yellow) + SCN-(aq)FeSCN2+(aq, red) + heata. When more SCN-ion (in the form of KSCN) is added to the reaction mixture? Explain why.HINT: Addition of reactants shifts equilibrium toward product; addition of product shiftsequilibrium toward reactant.87

Addition of more KSCN leads to increase in concentration of SCN- ion. According to Le Châtelier’s…

Answered: 2. Which way will the equilibrium shift…

Appl Of Ms Excel In Analytical Chemistry

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ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 3P

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Reaction: CrO42-(aq)+2H+(aq) <--> Cr2O72-(aq)+H2O(l) YELLOW ORANGE If sulfuric acid (H2SO4) is added to this solution, will a color change be observed? If so, how does the addition of sulfuric acid result in a color change? Explain your reasoning by showing the effect of the addition of H2SO4 on the equilibrium for the reaction.
33. The following two isomers of C3H7NO exist in equilibrium with each other in solution:If Kc = 0.57 at 25°C and the initial concentration of the reactant is 0.50 M and the product is 0.70M, what are the concentrations at equilibrium? Hint: compare Q to k to see which direction thereaction will go.
You have a test tube in which the following equilibrium is established. Fe3+ (aq) + SCN- (aq) FeSCN2+ (aq) Describe how concentrations of Fe3+, SCN- and FeSCN2+ will change if a crystal KSCN is added to the mixture above? What would stay constant?
A CHEM student is investigating the equilibrium of iron thiocyanate: Their reaction mixture is prepared by mixing together the following reagents: 2.50 mL of 0.002451 M Fe(NO3)3 6.0 mL of 0.1 M HNO3 1.50 mL of 0.0026721 M KSCNFrom literature, you know that Kc is 134 at 20°C. What will the [Fe(SCN)2+] be at equilibrium, in M?
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) Use your correct answers from #7 to answer this question. What is Kf, the formation constant, for this complex?
When you make up your standard solutions for this experiment: a) How does the concentration of the NaSCN (aq) solution compare to the concentration of the Fe(NO3)3 solution? b) Why would the concentrations of the NaSCN and Fe(NO3)3 solutions have been prepared with these relative concentrations? Invoke equilibrium principles as you answer this question.
"Calcium ions/oxalic acid equilibrium in the kidney" Base on the above statement, give an equilibrium related to that and answer the following questions: What is the K value of the equilibrium if it is available. Base on Le Chatelier's principle, when will that equilibrium will not meet and what negative effects will happen when the equilibrium is not met. Suggest the preventive measures that can be taken to avoid negative effects whem the equilbrium is not met.
10. In Part D, what property will you observe that will allow you to determine the direction of equilibrium shift for the reaction Fe3+(aq) + SCN-(aq) = FeSCN2+(aq)
The equilibrium constant of the reaction A(aq) + B(aq) --> 2C(aq) + D(aq) is 13492.3. This implies that at equilibrium, the concentration of the products will be (much less than, much more than, exactly equal to, about the same as) the concentration of the reactants.
Dinitrogen tetroxide, N2O4, dissociates at room temperature to give nitrogen dioxide, NO2.N2O4 (g) ⇌ 2 NO2 (g) (a) The equilibrium constant Kc at 25°C is 0,125. What percentage of dinitrogen tetroxideis dissociated when 0,0300 mol N2O4 is placed in a 1,00 dm3 flask and left to reachequilibrium?
Consider the insoluble compound nickel(II) carbonate , NiCO3 . The nickel ion also forms a complex with cyanide ions . Write a balanced net ionic equation to show why the solubility of NiCO3 (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction.For Ni(CN)42- , Kf = 1.0×1031 . Be sure to specify states such as (aq) or (s). + + K =
Consider the insoluble compound zinc carbonate , ZnCO3 . The zinc ion also forms a complex with hydroxide ions . Write a balanced net ionic equation to show why the solubility of ZnCO3 (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction.For Zn(OH)42- , Kf = 2.9×1015 . Be sure to specify states such as (aq) or (s). + + K =

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