[Ni (NH,),*]:[N*]A solution is prepared by adding 0.17 mole of Ni(NH3)6 Cl2 to 0.50 L of 3.7 M NH3. Calculateandin this solution.2+Koverall for Ni (NH3)6is 5.5 × 10°. That is,Ni (NH3)62+5.5 x 108 =Ni2+for the overall reactionNi2+ (ag) + 6NH3 (aq) = Ni (NH3)6* (aq)2+2+3)6M=[N**] - [M

Answered: Image /qna-images/answer/1446744e-3f06-45cd-a20b-c11a3445a7ba.jpg

A solution is prepared by adding 0.17 mole of Ni(NH3)6 Cl2 to 0.50 L of 3.7 M NH3. Calculate Ni (NH3 ),+ and Ni²+ in this solution. 2+ Koverall for Ni (NH3), is 5.5 × 10°. That is, Ni (NH3)6 2+ 5.5 x 108 = [Ni²+] [NH31* for the overall reaction 2+ Ni?+ (aq) + 6NH3 (ag) → Ni (NH3)6* (aq) [Ni (NHL),*] =[ [N**] - M. M =

A solution is prepared by adding 0.17 mole of Ni(NH3)6 Cl2 to 0.50 L of 3.7 M NH3. Calculate Ni (NH3 ),+ and Ni²+ in this solution. 2+ Koverall for Ni (NH3), is 5.5 × 10°. That is, Ni (NH3)6 2+ 5.5 x 108 = [Ni²+] [NH31* for the overall reaction 2+ Ni?+ (aq) + 6NH3 (ag) → Ni (NH3)6* (aq) [Ni (NHL),*] =[ [N**] - M. M =

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.54PAE

See similar textbooks

Similar questions

Calculate the concentration of Cd2+ resulting from the dissolution of CdCO3 in a solution that is 0.250 M in CH3CO2H, 0.375 M in NaCH3CO2, and 0.010 M in H2CO3.
In following these steps . Complete the table and provide th given chemical reactions in the qualitative analaysis of Group 3 Cations. Procedure 1. Place 20 drops of each of the following aqueous solutions to separate centrifuge tubes: 0.1M Cr (NO3)3, 0.1M Al (NO3)3, 0.1M Co (NO3)2, 0.1M Zn (NO3)2, 0.1M Mn (OH)2, 0.1M Ni (NO3)2, 0.1 M Fe (NO3)3. Make each solution basic by adding few drops of 6M NH4OH. Confirm using a litmus paper. 2. Add 5 drops of freshly prepared 6M (NH4)2S to each centrifuge tube. Place the samples in thecentrifuge machine for 3 mins. After centrifuge record results. Decant the supernatant liquid of all the samples. 3. Add one drop of NH4OH in each centrifuge tubes. Add 20 drops of distilled water in eachcentrifuge tubes. Then add a few drops of 6M HCl in each solution. Place the samples in the water bath for 10 mins. After water bath, centrifuge the samples for 3 mins. 4. After centrifuge, add a few drops of 6M NH4Cl in each sample. Decant the supernatant liquid…
Nickel sulfate, NiSO 4 , reacts with sodium phosphate, Na 3 PO 4 , to give a pale yellow-greenprecipitate of nickel phosphate, Ni 3 (PO 4 ) 2 , and a solution of sodium sulfate, Na 2 SO 4.. How manymilliliters of 0.375 M N i SO 4 will react with 45.7 mL of 0.265 M Na 3 PO 4 ? . Show balanced chemicalreaction of the problem.
A solution contains 0.04500.0450 M Ca2+ and 0.09500.0950 M Ag+. If solid Na3PO4 is added to this mixture, which of the phosphate species would precipitate out of solution first? -Ca3(PO4)2 -Ag3PO4 -Na3PO4 When the second cation just starts to precipitate, what percentage of the first cation remains in solution?
Consider the reaction IO4-(aq) + 2 H2O(l) ⇌ H4IO6-(aq); Kc = 3.5 x 10-2. If you start with 25.0 mLof a 0.905 M solution of NaIO4, and then dilute it withwater to 500.0 mL, what is the concentration of H4IO6- atequilibrium?
A similar experiment as this lab is done as following: 0.456 g of solid AgCl is added a 25 mL solution of a 1.05 M ligand L to form complex AgL+. AgCl (s) + L (aq) → AgL+ (aq) + Cl- (aq) When the reaction is complete, 0.315 g of solid AgCl remains. Assume the total volume of the resultant solution is the same as the volume of the ligand solution. Ksp of AgCl in water is 1.83 x 10-10. Answer the following questions. 4. What is the equilibrium constant K of the following reaction? AgCl (s) + L (aq) → AgL+ (aq) + Cl- (aq) K =? Group of answer choices A, 1.54e-3 B, 1.54e3 C, 2.37e-2 D, 2.37e2 plz answe mulitple question
A similar experiment as this lab is done as following: 0.456 g of solid AgCl is added a 25 mL solution of a 1.05 M ligand L to form complex AgL+. AgCl (s) + L (aq) → AgL+ (aq) + Cl- (aq) When the reaction is complete, 0.315 g of solid AgCl remains. Assume the total volume of the resultant solution is the same as the volume of the ligand solution. Ksp of AgCl in water is 1.83 x 10-10. Answer the following questions. 5.What is the formation constant Kf of AgL+. Ag+(aq) + L(aq) → AgL+(aq) Kf= ? Group of answer choices A, 2.35e-5 B, 8.39e-6 C, 2.35e5 D, 8.39e6
14.3 gm of hydrated sodium carbonate Na2CO3 .XH2O dissolved in water, then the volume of the solution is completed to 1 liter, if 25 ml of this solution is neutralized by 25 ml of 0.1M of hydrochloric acid, so the percentage of water crystallization will be Given that (O =16, C=12, Na =23)
A similar experiment as this lab is done as following: 0.456 g of solid AgCl is added a 25 mL solution of a 1.05 M ligand L to form complex AgL+. AgCl (s) + L (aq) → AgL+ (aq) + Cl- (aq) When the reaction is complete, 0.315 g of solid AgCl remains. Assume the total volume of the resultant solution is the same as the volume of the ligand solution. Ksp of AgCl in water is 1.83 x 10-10. 3.What is the equilibrium concentration of [L]eq? Group of answer choices A, 2.01 mol/L B,2.45 mol/L C, 1.01 mol/L D, 0.405 mol/L
A similar experiment as this lab is done as following: 0.456 g of solid AgCl is added a 25 mL solution of a 1.05 M ligand L to form complex AgL+. AgCl (s) + L (aq) → AgL+ (aq) + Cl- (aq) When the reaction is complete, 0.315 g of solid AgCl remains. Assume the total volume of the resultant solution is the same as the volume of the ligand solution. Ksp of AgCl in water is 1.83 x 10-10. 2. What are the equilibrium concentrations of [AgL+]eq and [Cl-]eq? Group of answer choices A, 0.0394 mol/L B, 12.5 mol/L C, 0.0154 mol/L D, 0.394 mol/L
A sample of 0.0500 M barium nitrate solution and 0.0500 M sodium sulfate solution was labeled with radioactive . The radioactivity of the initial sodium sulfate solution was 1.22 x106 counts per second. After the formation of the precipitate and purification by filtration the remaining radioactivity in solution was 250 counts per second. Calculate the Ksp for the following dissociation: BaSO4(s) ↔Ba+2(aq) + SO4-2(aq) Group of answer choices 5.96x104 1.02x10-5 1.05x10-10 5.12x10-7
Describe the preparation of 500 mL 0.50 M K2Cr2O7 solution using solid K2Cr2O7 (purity: 99.8%). What is the volume of NaOH needed to dilute 1.50 M NaOH to 250 mL of 0.10 M. Calculate the volume of 0.1 M HCl needed to react with 50 mL of 0.89 M NaOH.