Question

In: Chemistry

Design a separation scheme for Cu2+, Fe3+, Mn2+, and Ni2+ include equations for all reactions.

Design a separation scheme for Cu2+, Fe3+, Mn2+, and Ni2+ include equations for all reactions.

Solutions

Expert Solution

First dissolve the given mixture of salts and then separate the group (I) cation. here the only one group (I) cation is Cu 2+

First add Aqueous ammonia to the mixture, aq. ammonia reacts with Cu2+ to form a deep blue tetraammine copper(II) complex ion and precipitates out.

Cu2+(aq) + 4NH3(aq) → [Cu(NH3)4] 2+(ppt).

filter out the ppt, thus we separated out Cu2+.

NOW we focus on separation of group (II) cations

The Separation and Confirmation of Group II Ions: Mn2+, Ni2+, Fe3+.

Now take the aqueous soluion of the remaining salt and add one drop of HNO3 in it:

Separation and Confirmation of Mn2+ 1. Place 5 drops of this solution into another clean centrifuge test tube and add a small amount of solid sodium bismuthate (NaBiO3) using a wooden spatula. Use the amount you can fit on the tip of the spatula. 3. Add 20 drops of distilled water, stir, and centrifuge. A purple-colored solution confirms the presence of Mn2+.

The equation for step is: 14H+ (aq) + 2Mn2+(aq) + 5BiO3 – (aq) → 2MnO4 – (aq) + 5Bi3+(aq) + 7H2O(l) purple C.

Separation and Confirmation of Fe3+

1. To the remaining solution from part B above, add 15 drops of 6M NH3·H2O and stir. Centrifuge and decant the supernatant into a clean centrifuge test tube. Label the tube "Nickel" and set it aside for future use. To the precipitate, add 10 drops of 6M hydrochloric acid, stir, and then add 3 drops of 0.1 M NH4SCN. A “blood-red” color confirms the presence of Fe3+. The equations for step 1 are: Fe3+(aq) + 3OH– (aq) → Fe(OH)3(s) Ni2+(aq) + 6NH3(aq) → [Ni(NH3)6] 2+(aq) The equations for step 2 are: Fe(OH)3(s) + 3H+ (aq) → Fe3+(aq) + 3HOH(l) Fe3+(aq) + 6SCN– (aq) → [Fe(NCS)6] 3–(aq) blood-red.

The Confirmation of Ni2+

Add 4 drops of dimethylglyoxime (DMG) to the tube labeled "Nickel" in part C and stir. There is no need to centrifuge, as the nature of the precipitate (sometimes called a “lake”), is more obvious before centrifuging. A strawberry-colored ppt confirms the presence of Ni2+. The equation for step 1 is: [Ni(NH3)6] 2+(aq) + 2H2DMG → [Ni(HDMG)2](s) + 2NH4 + (aq) + 4NH3(aq) pink-red  


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