Question

Based on the given lab procedure, write the balanced reaction equation. (Note: this reaction occurs in steps, which should be shown before combining into one overall reaction equation). Introduction Anhydrous nickel (II) fluoride cannot be prepared by simple means. The direct reaction of the elements gives nickel (III) fluoride and attempts to dehydrate the hydrated salt yield basic compounds due to the similarity in size of the F- and OH- ions. The following indirect method of preparation is typical of the way such problems are overcome. An intermediate is prepared which decomposes on heating to give the desired compound and a variety of volatile by-products. The sequence of reactions will also reveal that not all compounds containing the Ni2+ ion are green. Chemicals required Nickel(II) chloride hexahydrate 6.0 g Concentrated ammonium hydroxide 12 mL Ammonium tetrafluoroborate 5.0 g 6 mol/L ammonium hydroxide 12.5 mL Procedure A: Hexamminonickel(II)tetrafluoroborate Dissolve the nickel(II) chloride hexahydrate in 10 mL of warm deionized water in a 150 mL beaker. In a fumehood, add 12 mL of concentrated ammonium hydroxide to the Ni2+ solution, stirring well while solution and violet colored crystals of hexamminonickel(II) dichloride (these may not be visible). Slowly and carefully, add about 15 mL of water with stirring, to just redissolve these crystals at room temperature. If necessary, filter to remove any residue. Cover the beaker with a watch glass and return it to your bench for the next stage. Dissolve about 5 g of ammonium tetrafluoroborate in about 12.5 mL of 6 mol/L aqueous ammonia heating if necessary with a hot plate - stirrer in a fume hood to dissolve the solid, and add this solution to the nickel solution. A pale violet precipitate forms at once but because its refractive index is close to that of water; it is invisible until filtered. Collect the product by suction filtration with a Buchner funnel and wash it with small portions of 3 mol/L ammonia solution until the filtrate runs clear. Wash the violet product with acetone and remove as much liquid from it as possible using an aspirator. Store it in a labeled screw cap vial to prevent loss of ammonia. Determine the mass of product collected and report a percent yield. Place about 1.5 g of the hexamminonickel(II) tetrafluoroborate on a watch glass (record mass!), leave it in your desiccator until the next lab period.

Name: based on the given lab procedure write the balanced reaction equation note this reaction occurs in steps which should be shown before combining into one overall reaction equation introductio 29346
Uploaded: 2022-02-24T07:04:17-08:00
Duration: 1 min 40 s
Channel: Josee Pacheco
Description: based on the given lab procedure write the balanced reaction equation note this reaction occurs in steps which should be shown before combining into one overall reaction equation introductio 29346

Based on the given lab procedure, write the balanced reaction equation. (Note: this reaction occurs in steps, which should be shown before combining into one overall reaction equation).

Introduction
Anhydrous nickel (II) fluoride cannot be prepared by simple means. The direct reaction of the elements gives nickel (III) fluoride and attempts to dehydrate the hydrated salt yield basic compounds due to the similarity in size of the F- and OH- ions.
The following indirect method of preparation is typical of the way such problems are overcome. An intermediate is prepared which decomposes on heating to give the desired compound and a variety of volatile by-products.
The sequence of reactions will also reveal that not all compounds containing the Ni2+ ion are green.

Chemicals required
Nickel(II) chloride hexahydrate 6.0 g
Concentrated ammonium hydroxide 12 mL
Ammonium tetrafluoroborate 5.0 g
6 mol/L ammonium hydroxide 12.5 mL

Procedure A: Hexamminonickel(II)tetrafluoroborate
Dissolve the nickel(II) chloride hexahydrate in 10 mL of warm deionized water in a 150 mL beaker. In a fumehood, add 12 mL of concentrated ammonium hydroxide to the Ni2+ solution, stirring well while solution and violet colored crystals of hexamminonickel(II) dichloride (these may not be visible). Slowly and carefully, add about 15 mL of water with stirring, to just redissolve these crystals at room temperature. If necessary, filter to remove any residue. Cover the beaker with a watch glass and return it to your bench for the next stage.
Dissolve about 5 g of ammonium tetrafluoroborate in about 12.5 mL of 6 mol/L aqueous ammonia heating if necessary with a hot plate - stirrer in a fume hood to dissolve the solid, and add this solution to the nickel solution. A pale violet precipitate forms at once but because its refractive index is close to that of water; it is invisible until filtered. Collect the product by suction filtration with a Buchner funnel and wash it with small portions of 3 mol/L ammonia solution until the filtrate runs clear. Wash the violet product with acetone and remove as much liquid from it as possible using an aspirator. Store it in a labeled screw cap vial to prevent loss of ammonia. Determine the mass of product collected and report a percent yield. Place about 1.5 g of the hexamminonickel(II) tetrafluoroborate on a watch glass (record mass!), leave it in your desiccator until the next lab period.

based on the given lab procedure write the balanced reaction equation note this reaction occurs in steps which should be shown before combining into one overall reaction equation introductio 29346

Added by Esther P.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Josee Pacheco

02/24/2022

Step 1

\[ NiCl_2 \cdot 6H_2O + 6NH_4OH \rightarrow [Ni(NH_3)_6]Cl_2 + 6H_2O \] Show more…

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Based on the given lab procedure, write the balanced reaction equation. (Note: this reaction occurs in steps, which should be shown before combining into one overall reaction equation). Introduction Anhydrous nickel (II) fluoride cannot be prepared by simple means. The direct reaction of the elements gives nickel (III) fluoride and attempts to dehydrate the hydrated salt yield basic compounds due to the similarity in size of the F- and OH- ions. The following indirect method of preparation is typical of the way such problems are overcome. An intermediate is prepared which decomposes on heating to give the desired compound and a variety of volatile by-products. The sequence of reactions will also reveal that not all compounds containing the Ni2+ ion are green. Chemicals required Nickel(II) chloride hexahydrate 6.0 g Concentrated ammonium hydroxide 12 mL Ammonium tetrafluoroborate 5.0 g 6 mol/L ammonium hydroxide 12.5 mL Procedure A: Hexamminonickel(II)tetrafluoroborate Dissolve the nickel(II) chloride hexahydrate in 10 mL of warm deionized water in a 150 mL beaker. In a fumehood, add 12 mL of concentrated ammonium hydroxide to the Ni2+ solution, stirring well while solution and violet colored crystals of hexamminonickel(II) dichloride (these may not be visible). Slowly and carefully, add about 15 mL of water with stirring, to just redissolve these crystals at room temperature. If necessary, filter to remove any residue. Cover the beaker with a watch glass and return it to your bench for the next stage. Dissolve about 5 g of ammonium tetrafluoroborate in about 12.5 mL of 6 mol/L aqueous ammonia heating if necessary with a hot plate - stirrer in a fume hood to dissolve the solid, and add this solution to the nickel solution. A pale violet precipitate forms at once but because its refractive index is close to that of water; it is invisible until filtered. Collect the product by suction filtration with a Buchner funnel and wash it with small portions of 3 mol/L ammonia solution until the filtrate runs clear. Wash the violet product with acetone and remove as much liquid from it as possible using an aspirator. Store it in a labeled screw cap vial to prevent loss of ammonia. Determine the mass of product collected and report a percent yield. Place about 1.5 g of the hexamminonickel(II) tetrafluoroborate on a watch glass (record mass!), leave it in your desiccator until the next lab period.