NiCl2 + NaOH = Ni(OH)2 + NaCl | Nickel Chloride + Sodium Hydroxide Reaction

Nickel chloride (NiCl2) and sodium hydroxide (NaOH) reacts and gives green colour nickel hydroxide (Ni(OH)2) precipitate and sodium chloride (NaCl). Nickel chloride is a green colour solution and sodium chloride is colourless aqueous solution. However, nickel hydroxide is not soluble in excess NaOH.

NiCl2 + NaOH reaction

NiCl2(aq) + NaOH(aq) = Ni(OH)2(s) + NaCl(aq)

Aqueous nickel chloride is a green colour solution and aqueous sodium hydroxide is a colourless solution. When they react with each other, green colour precipitate, nickel hydroxide and colourless sodium chloride solution is given.

Balanced equation of nickel chloride and sodium hydroxide

NiCl2(aq) + 2NaOH(aq) = Ni(OH)2(s) + 2NaCl(aq)

1 mol of NiCl2 reacts with 2 mol of NaOH and produce 1 mol of Ni(OH)2 and 2 mol of NaCl. Except Ni(OH)2, all other compounds exist as aqueous state. Ni(OH)2 exists in solid state.

Observations during the reaction

When you are slowly adding one chemical to other chemical drop by drop, at one time, you will see a green colour precipitate is formed in the solution. If you suddenly add one chemical to another, green precipitate is also formed immediately.

In the presence of excess NaOH, what will happen to the green precipitate?

We know some metal hydroxides are soluble in the presence of excess NaOH. Those soluble metal hydroxides have amphoteric characteristics.

Nickel hydroxide is not soluble in excess sodium hydroxide because nickel hydroxide is not a amphoteric hydroxide. Therefore, nickel hydroxide precipitate will remain as the green precipitate when NaOH is added more and more.

What will happen to pH value of NaOH solution when NiCl2 is added?

We know, aqueous NaOH has high pH values because NaOH is a strong base. When NiCl2 is added, OH- ions are reduced in the aqueous solution because OH- ions are combined with Ni2+ and get deposited as a precipitated. Due to reduction of OH- ion concentration, pH value is decreased.

Questions asked by students

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Can I identify aqueous NiCl2 and aqueous FeCl2 by NaOH?

Both aqueous NiCl2 and queous FeCl2 are green colour solutions. Both these compounds react with NaOH and give green colour precipitates (respective metal hydroxides) and they are insoluble in excess NaOH. Therefore we cannot identify NiCl2 and FeCl2 by NaOH.

If solid NiCl2 is added to aqueous NaOH, can I see the green precipitate?

Yes. you see. Because solid NiCl2 dissociates to nickel +2 ions and chloride ions in water. Then, nickel +2 ion and hydroxyl ions form nickel hydroxide precipitate.

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