why is a solution of Cu (II) sulfate blue? Explain with electrons and orbitals.
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why is a solution of Cu (II) sulfate blue? Explain with electrons and orbitals.
The deep blue compound Cu(NH3)4SO4 is made by the reaction of copper(II) sulfate and ammonia. CuSO4(aq) + 4NH3(aq) → Cu(NH3)4SO4(aq) If you use 47.0 g of CuSO4 and excess NH3, what is the theoretical yield of Cu(NH3)4SO4? If you isolate 38.2 g of Cu(NH3)4SO4, what is the percent yield of Cu(NH3)4SO4? ______ g Cu(NH3)4SO4 _______ %
why bail blue of [Cu(H2O)6]^2+ can turn dark blue when ammonia solution is added?
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...
The deep blue compound Cu(NH)4SO4 is made by the reaction of copper(ll) sulfate and ammonia Cu(NHs)4SO4 (aq) CuSO4(aq) 4 NHs (aq) > If you use 18.0 g of CuSO4 and excess NH3. what is the theoretical yield of Cu(NHs)4SO4? g Cu(NHs)4SO4 If you isolate 15.3 g of Cu(NH3)4SO4, what is the percent yield of Cu(NH3)4S04?
(i) Draw the electron distribution in the d orbitals of an octahedral Cu(II) complex and show the electronic transition responsible for the absorptions observed. (ii) Assign the transition you observe for each complex and give the value of (in cm-1 ) (ii) is based on the complexes from (i)
(ii) Explain the Jahn-Teller distortion in [Cu(H2O)2 (ii) If a solution with a dissolved octahedral complex appears yellow to the eye, what wavelength of light does it absorb? Is this complex expected to be low spin or high spin?
A solution of copper (II) sulfate (CuSO_4) in water is 11.00% copper (II) sulfate by mass. Its density is 1.1186 g cm^3 at 20 degree c. Compute its molarity, mole fraction, and molality at this temperature. Molarity CuSO_4 = M Mole fraction CuSO_4 = Molality CuSO_4 = m.
A solution was found to contain 5.21% copper (II) sulfate. How many grams of solution would contain 25.0 g of copper (II) sulfate?
What is the concentration of Cu2+ when 0.025 moles of copper (II) sulfate are added to one liter of a solution that is 1.0M CN-? Cu2+ + 4CN- —> <— Cu(CN)4 2-