EQ1: NH3(aq + H2O(l) ßà NH4+(aq) Kb=1.8x10-5
The bismuth(III) ion is precipitated out of the solution as Bi(OH)3. The equilibrium involved is related to the one provided below:
EQ2: Bi(OH)3(s) ßà Bi3+(aq) +3OH(aq)- Ksp =3.2x10-40
Manipulate EQ 1 and 2 to solve for the net equation, EQ3:
EQ3 (net): 3H2O+ Bi3+(aq) +3NH3(aq) ßàBi(OH)-(s) +3NH4+(aq)
Write the mass law expression for the net reaction and calculate the K. Does the reaction form mostly products, or mostly reactants? EXPLAIN.
EQ4: Cu2+(aq)+ 4NH3(aq)ßà[Cu(NH3)4]2+(aq) Kf = 1.1x1013
A blue precipitate initially forms and then dissolves in the excess NH3. The precipitate that forms initially is Cu(OH)2.
EQ5: Cu2+(aq) + 2OH-(aq) ßà Cu(OH)2(s) K=2.08x1019
The needed OH-to dissolve the Cu(OH)2(s) comes from the ionization of ammonia in water:
EQ 6: NH3(aq) + H2O(l) ßà NH4+(aq)+ OH-(aq) Kb =1.8x10-5
Manipulate EQ 5 and 6 to find the net reaction (EQ 7) for the precipitation of the copper(II) hydroxide. Write the mass law expression and calculate the Knet.
EQ 7: Cu2+(aq) +2NH3(aq) + 2 H2O(l)ßàCu(OH)2(s) +2 NH4+(aq)
EQ 8: Cu(OH)2(s) + 2OH-(aq) + 4 NH4+(aq) ßà [Cu(NH3)4]2+(aq) + 4 H2O(l)
Manipulate EQ 4, 5, and 6 to solve for the net reaction, EQ 8. Write the mass law expression and calculate Knet. Compare the K for equation 8 and equation 7. Which lies further to the right? How does excess ammonia helps dissolve the Cu(OH)2?
EQ 9: [Cu(NH3)4]2+(aq) + 4CH3CO2H(aq)ßà Cu2+ + 4 NH4+(aq) + 4CH3CO2-(aq)
Explain in terms of leChatelier’s principle and EQ9
Cd2+(aq) + 4CN-(aq)ßà [Cd(CN)4]2 Kf =7.7x1016
Compare your answer to the answer from question 6. Which complex ion is more stable explain.
Please Show Work!
According to LeChatelier principle, if an equilibrium is put under stress then equilibrium will shift in that direction such that the stress is minimised.
The value of equilibrium constant of EQ8 is greater than that of EQ7. Hence EQ8 will lies further to the right. The excess of ammonia can dissolve Cu(OH)2 , because Copper can form a stable complex with ligand(NH3).
Acetic acid is used to release Cu2+ from the complex because acetic acid neutralize the liquid ammonia. And concentration of ammonia decrease and equilibrium will shift backward i.e. dissociation of complex.
In step1, aqueous ammonia is added to a solution of the three ions. The equilibrium for...
40. Concentrated aqueous ammonia is added to a solution of copper(II) sulfate. A white precipitate forms. The precipitate dissolves as more ammonia is added, generating an intensely blue solution. Which combination of net ionic equations, in the appropriate order, describes this chemistry?! I Cu?* (aq) + 2OH(aq) Cu(OH)2 (19) II Cu?" (aq) + 2OH(aq) = Cu(OH)2 (8) III Cu(OH)(aq) + 4 NH, (aq) Cu(NH3),?* () + 2OH(aq) IV Cu(OH)2 (8) + 4NH, (aq) Cu(NH3)*(14) + 2OH(aq) V NH3(aq) + H20...
I am sort of confused on what these are asking? An explination of the concepts would really help, I will give thumbs up :) 3. Consider the following reactions: a) The formation of tetraaqua copper (Il) ion in solution Cu2+ + 4H2O(l) = [Cu(H2O)4](aq) b) The reaction of ammonia with water. NH3(aq) + H2O(l) = NH4+ (aq) + OH(aq) c) The self ionization of water 2H2O(0) — H3O*(aq) + OH(aq) d) The formation of copper (II) hydroxide [Cu(H20)4]2+ (aq) +...
When aqueous solutions of NH4OH(aq) and CuCl2(aq) are mixed, the products are NH4Cl(aq) and Cu(OH)2(s). What is the net ionic equation for this reaction? Select the correct answer below: 2NH4OH(aq)+CuCl2(aq)⟶Cu(OH)2(s)+2NH4Cl(aq) 2NH+4(aq)+2OH−(aq)+Cu2+(aq)+2Cl−(aq)⟶Cu(OH)2(s)+2NH+4(aq)+2Cl−(aq) Cu2+(aq)+2OH−(aq)⟶Cu(OH)2(s) NH+4(aq)+Cl−(aq)⟶NH4Cl(s)
please help What is the approximate concentration of free Cu* ion at equilibrium when 1.57x102 mol copperII) nitrate is added to 1.00 L of solution that is 1.380 M in NH3. For [Cu(NH3)4j2, Kf 2.1 1013 [Cu2 м What is the approximate concentration of free Fe2* ion at equilibrium when 1.42x102mol iron(II) nitrate is added to 1.00 L of solution that is 1.38so M in CN. For [Fe(CN)6]4, Kf=1.0x1035 [Fe"]= In the presence of excess OH, the Al*(aq) ion forms...
When aqueous solutions of NH4OH(aq) and CuCl2(aq) are mixed, the products are NH4Cl (aq) and Cu(OH)2(s). What is the net ionic equation for this reaction? Select the correct answer below: Question 12 options: 2 NH4OH(aq)+CuCl2(aq)⟶Cu(OH)2(s)+2NH4Cl(aq) 2NH+4(aq)+2OH−(aq)+Cu2+(aq)+2Cl−(aq)⟶Cu(OH)2(s)+2NH+4(aq)+2Cl−(aq) Cu2+(aq)+2OH−(aq)⟶Cu(OH)2(s) NH+4(aq)+Cl−(aq)⟶NH4Cl(s)
What are the equilibrium concentrations of NH3, NH4+, and OH- in a 0.95 M solution of ammonia? Kb = 1.8x10^-5 What is the pH of the solution? pH =
Which of the reactions involving metal ions (Equations 1A – 6B ) represent redox reaction(s)? Write down the entire equation(s) AS WELL AS their corresponding balanced oxidation half-reaction(s) AND reduction half-reaction(s). Ag+(aq)+ HCl(aq)+ H2O(l) -> AgCl(s, white)+ H3O+(aq) Eq. 1A AgCl(s)+ 2NH3(aq) -> [Ag(NH3)2]+(aq)+ Cl–(aq) Eq. 2A Fe3+(aq)+ 3NH3(aq)+ 3H2O(l) -> Fe(OH)3(s)+ 3NH4(aq) Eq. 3A Fe3+(aq)+ 6SCN–(aq) -> Fe(SCN)63–(aq, blood-red) Eq. 4A Co2+(aq)+ 7NO2–(aq)+ 3K+(aq)+ 2H3O+(aq) -> NO(g)+ 3H2O(l)+ K3[Co(NO2)6](s, yellow) Eq. 6A 2 NO(g, colorless)+ O2(g) →2NO2(g, red-brown) Eq....
Balance the following redox reaction occurring in basic solution. Ag(s) + CN- (aq) + O2(g) → Ag(CN), (aq) 2 Ag(s) + 4CN (aq) +202 + H2O(l)(9) + 2 Ag(CN)2 (aq) + 2OH(aq) • 2 Ag(s) + 8 CN (aq) + 402 + 2 H20(1)(g) + 4 Ag(CN)2 (aq) +8 OH(aq) 4 Ag(s) + 2 CN (aq) + O2 + 4H2O(1)(9) + 4 Ag(CN)2 (aq) + 8 OH (aq) 4 Ag(s) + 8 CN (aq) + O2 + 2 H20(1)(9) +...
Aqueous solutions of ammonia (NH3) and hydrogen cyanide (HCN) react to produce ammonium cyanide, (NH4CN) according to the following equilibrium reaction. NH3(aq) + HCN(aq) = NH4+ (aq) + CN (aq) Given the following equilibrium constants, which statement best describes the reaction once equilibrium is established? (Kw - 1.01 x 10-14) NH4+ Ka = 5.6 x 10-10 HCN ka = 4.0 x 10-10 reaction is product favored, K<1 reaction is neither reactant nor product favored reaction is product favored, K>1 reaction...
Aqueous solutions of ammonia (NH3) and hydrogen cyanide (HCN) react to produce ammonium cyanide, (NH4CN) according to the following equilibrium reaction. NH3(aq) + HCN(aq) = NH4+ (aq) + CN (aq) Given the following equilibrium constants, which statement best describes the reaction once equilibrium is established? (Kw = 1.01 x 10-14) NH4* Ka = 5.6 x 10-10 HCN Ka = 4.0 x 10-10 reaction is reactant favors, K> 1 O reaction is reactant favors, K <1 O reaction is product favored,...