The cation M²+ reacts with NH3 to form a series of complex ions as follows: M²+ + NH3 M(NH3)²+ K₁ = 10² M(NH3)2+ + NH3= M(NH3)2²+ K₂ = 10³ M(NH3)22+ + NH3 = M(NH3)3²+ K3 = 10² A 1.0 × 10-³ mol sample of M(NO3)2 is added to 1.0 L of 15.0 MNH3 (Kb = 1.8 x 10-5). Choose the dominant species in this solution. M²+ O M(NH3)²+ O M(NH3)22+ O M(NH3)3²+ O M(NO3)2

The cation M²+ reacts with NH3 to form a series of complex ions as follows: M²+ + NH3 M(NH3)²+ K₁ = 10² M(NH3)2+ + NH3= M(NH3)2²+ K₂ = 10³ M(NH3)22+ + NH3 = M(NH3)3²+ K3 = 10² A 1.0 × 10-³ mol sample of M(NO3)2 is added to 1.0 L of 15.0 MNH3 (Kb = 1.8 x 10-5). Choose the dominant species in this solution. M²+ O M(NH3)²+ O M(NH3)22+ O M(NH3)3²+ O M(NO3)2

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The composition of a hydrated sodium-salt of a chromium(III)-oxalate complex ion conforms to the general formula: NaxCr(C2O4)3·wH2O A 0.2547-g sample of this compound required 21.99 mL of 0.02925 M KMnO4 solution for the titration of all of the oxalate. a)What is the value of x? b)What is the value of w?
Cyanide ion is toxic because it forms stable complexes with Fe3* in iron-containing proteins important in energy production. To study this effect, a biochemist prepares one liter of a solution that contains 0.025 mol Fe3+ and 0.80 mol CN. What is the final molar concentration of Fe3+ in the solution? K, of Fe(CN)g3- is 4.0 x 1043.
Choose the best answer below. Consider the following complex ion formation equilibrium and it's equilibrium constant, Kf. Which of the following statements is FALSE? Cu2* (aq) + 4CN" (aq) Û Cu(CN)4² (aq) K = 1.0x1025 Cu2* is a Lewis acid in the reaction, and CN' is a Lewis base Removing some of the Cu2* (e.g., by precipitation) will cause some of the complex ion to dissociate O If enough CN is added, the equilibrium mixture would contain zero Cu²+ The complex ion is a Lewis acid-base adduct Adding more CN" will cause more complex ion to form ) The equilibrium lies in favor of the complex ion
Given the equation Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq)Kf=2.00×107Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq)Kf=2.00×107 determine the concentration of NH3(aq) that is required to dissolve 669669 mg of AgCl(s) in 100.0 mL of solution. The KspKsp of AgCl is 1.77×10−101.77×10−10.
A student was given two vials and each contained a chromium salt. The vial labeled CrCl,-6 H,0 contained a dark green solid and the one labeled Cr(NO,)3-9 H,0 contained a purple solid. She made aqueous solutions of these solids and the colors of these solutions were the same as the solids (see image below). Initial appearance of aqueous solutions (0.05 M) of Cr(NO3); 9 H,0O (left) and CrCl; 6 H,O (right) After preparing these solutions, she had to leave the lab and the solutions remained sitting on the bench for 24 hours. When she returned the next day, she found that the aqueous solution of CrCl, had changed color and was now purple like the solution containing Cr(NO3);'9 H,0 (see image below). Appearance of the same aqueous solutions (0.05 M) of Cr(NO3); 9 H,O (left) and CrCl;'6 H,O (right) after 24 hours Based upon this observation, please describe what happened in the solution. Write out reactions that describe the changes that took place in the CrCl3-6 H,O solution over the course…
Give detailed Solution with explanation
Give correct handwritten answer
The formation constant of a complex ion [M(NH3)4]2+(aq) is 1.8E8. If a solution is prepared by adding 0.3 mol of [M(NH3)4]Cl2 to 850.0 mL of water, what is the equilibrium concentration of free M2+(aq) ions?
Calculate the number of milliliters of 0.761 M KOH required to precipitate all of the Cr* ions in 167 mL of 0.502 M CrClg solution as Cr(OH)3. The equation for the reaction is: CrCl3(aq) + 3KоНаq) —Cr(OH)3(5) + зКС{aq) mL KOH
Suppose, in an experiment to determine the amount of sodium hypochlorite in bleach, you titrated a 21.63 mL21.63 mL sample of 0.0100 M KIO30.0100 M KIO3 with a solution of Na2S2O3Na2S2O3 of unknown concentration. The endpoint was observed to occur at 14.66 mL14.66 mL . How many moles of KIO3KIO3 were titrated?
1.Calculate the normality of the solutions containing 5.267g/L K2Cr2O7 (the Cr is reduced to Cr3+).(FW=294.19 g/mol) 2.A and B react as follows: A + B 2C. The equilibrium constant is 5.0 x 106. If 0.40 mol of Aand 0.70 mol of B are mixed in 1L, what are the concentrations of A, B and C after reaction? 3. The following data is given at a certain temperature:(1) 2N2 (g) + O2 (g) 2N2O (g) K1 = 1.2 x 10-35(2) N2O4 (g) 2NO2 (g) K2 = 4.6 x 10-3(3) ½N2 (g) + O2 (g) NO2 (g) K3 = 4.1 x 10-9Calculate the molar equilibrium constant, K for the reaction:2N2O (g) + 3O2 (g) 2N2O4 (g)
What is the molality of ions in a 0.265 m solution of (NH₄)₃PO₄ assuming the compound dissociates completely?