why bail blue of [Cu(H2O)6]^2+ can turn dark blue when ammonia solution is added?
When ammonia is slowly added to a light blue solution of CuSO4 (aq), at first a white precipitate forms. What is the formula of that precipitate? After more ammonia is added, a dark blue solution forms. What is the formula of the compound or ion responsible for the dark blue color?
1.25 g of CuSO4.5 H2O is treated with excess ammonia, when a deep blue solution is obtained. To this solution 5 mis of ethanol is added and the solid copper sulfate tetramine sulfate is obtained on filtration using a Buchner filter. On drying, the mass of the filter paper (085g) and compound is found to be 1.12 grams Calculate the percent yield? [6]
When concentrated ammonia is added to acidic copper solution, the pale-blue precipitate forms, followed by formation of bright blue soluble compound. Write formulas of the precipitate and of colored complex.
In experiment 7, when concentrated ammonia is added to acidic copper solution, the pale-blue precipitate forms, followed by formation of bright blue soluble compound. Write formulas of the precipitate and of colored complex. When potassium iodide is added to copper(II) nitrate solution, a brown precipitate forms. Write and balance the corresponding reaction equation. This brown precipitate is titrated with sodium thiosulfate solution. Write and balance the corresponding equation. After titration, a white precipitate is left in the solution. Write the...
1. in the copper cycle experiment when a solution of NaOH(aq) is added to a solution of Cu(NO3)2, what happens? a. no reaction occurs b. a blue copper (II) hydroxide precipitate forms along with a solution of NaNO3(aq) c. a reddish copper solid forms and the solutions bubbles because the presence of H2 gas d. a black copper (II) oxide solid forms and H2O molecules are released in a decomposition 2. Put these in order in how to safely light...
why is a solution of Cu (II) sulfate blue? Explain with electrons and orbitals.
2. Consider the following equilibrium represent by the reversible equation below: Cu?"(aq) + 4 NH OH(aq) = [Cu(NH3)4]?" (aq) + 4 H2O(1) Blue Colorless Navy blue Predict the shift (explain why) and indicate the color of the solution when a. Drops of strong acid is added b. H2S gas is bubbled in the solution. Note: H2S reacts with transition metal cations. c. Water is added to the mixture at equilibrium.
2. Consider the following equilibrium represent by the reversible equation below: Cu²+(aq) + 4 NH4OH(aq) = [Cu(NH3)4]2+(aq) + 4 H2O(1) Blue Colorless Navy blue Predict the shift (explain why) and indicate the color of the solution when a. Drops of strong acid is added b. H2S gas is bubbled in the solution. Note: H2S reacts with transition metal cations.
When ammonia is added to Zn(NO3)2 solution, a white precipitate forms, which dissolves on the addition of excess ammonia; but when ammonia is added to a mixture of Zn(NO3)2 and NH4NO3 no precipitate forms at any time. Suggest an explanation for this difference in behavior.
In step1, aqueous ammonia is added to a solution of the three ions. The equilibrium for the ammonia is 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...