Zinc Hydroxide Formula

What is the Formula of Zinc Hydroxide?

On earth, Zinc Hydroxide exists as a rare natural mineral. It is also an amphoteric white solid compound, which has the ability to dissolve in a solution of strong acid or strong base. It takes place as three rare earth minerals Ashoverite, Wulfingite, and Sweetite. The formula for zinc hydroxide is Zn(OH)\[_{2}\].


Properties of Zinc Hydroxide


Physical Properties


Chemical formula of zinc hydroxide

Zn(OH)\[_{2}\]

Molecular weight

99.394 g/mol

Melting point

125 degree Celsius

Density

3.053 g/cm\[^{3}\]

Odour

Odourless

Appearance

Dull white flocculent precipitate

Valency of Zn

2

Oxidation State

+2

Solubility

Slightly soluble in water, insoluble in alcohol


Chemical Properties

Aluminium reacting with the zinc hydroxide solution gives a white precipitate that is soluble in excess of the reagent to produce complex Al(OH)\[_{4}\] indicates the aluminium presence. The respective zinc hydroxide to zinc oxide equation is given below:

2Al\[_{3}\]+(aq) + 3Zn(OH)\[_{2}\](aq) → 2Al(OH)\[_{3}\](s) + 3Zn

Zinc cations react with the hydrogen sulphide in the presence of ammonium chloride and ammonia produces a white precipitate of zinc sulphide, which is soluble in acids.

Zn\[^{2+}\](aq) + S\[^{2-}\] → ZnS(s)


Zinc Hydroxide Structural Formula

The zinc hydroxide chemical formula or chemical formula for zinc hydroxide is Zn(OH)\[_{2}\]. Let us look at the typical structural representation of Zinc Hydroxide is given below:

[Image will be Uploaded Soon]

It exists in the tetragonal or orthorhombic forms.

In regular conditions, zinc dissociates to produce zinc ions along with the 2 hydroxide ions from the sodium hydroxide solution to produce zinc hydroxide.

Zn\[^{2+}\] + 2OH\[^{-}\] → Zn(OH)\[_{2}\]

When Zinc hydroxide reacts with an excess amount of sodium hydroxide, it precipitates to produce Zn (OH)\[_{2}\] and later dissolves into zincate ion.

Zn (OH)\[_{2}\] + 2OH\[^{-}\] → Zn(OH)\[_{4}^{2-}\]


Uses of Zinc Hydroxide – Zn(OH)\[_{2}\]

The primary uses of Zinc Hydroxide are listed below:

  • It can be used as an adsorbing agent in medicine.

  • They are utilized for the careful dressings where it works as a retentive. Huge bandages, which are utilized post-medical procedure, can be covered with the zinc compound for engrossing the blood from any injuries.

  • It is also used as an intermediate for the commercial production of pigments and pesticides.

FAQs (Frequently Asked Questions)

1. Give the Production of Sodium Hydroxide?

Answer: The synthesis starts from the electrolysis process of ultra-pure Sodium Chloride (which is a highly purified table salt). Chlorine and Sodium are separated immediately; while chlorine may be employed for many various reactions (largely based on market prices and demand), sodium reacts with water to produce Sodium Hydroxide, NaOH, that comes out from the reactor in an aqueous solution of 50%. The solid form (prills, pellets, or flakes) need heat treatment to dry the solution.


The most expensive part of the production is given as the energy required for the electrolysis. The means to separate sodium and chlorine used to be a mercurium cell reaction; nowadays, a specific membrane can be used in all modern reactors.

2. Which Bond Does Sodium Hydroxide Belong To?

Answer: It depends upon which bond (in NaOH) that we are dealing with. The bond between hydrogen and oxygen is covalent and between the hydroxide part and sodium is ionic. We can decide it on our own by calculating the electronegativity difference between its constituent elements. If the result is 1.7 or above, the bond is ionic and if it is below 1.7, the bond is covalent.


There exist 2 types of bonds in a NaOH molecule. The first one is an ionic bond, which bonds the Na+ ion and OH- ion. The positive Na+ ion is attracted to the OH- ion in this bond. (Because the opposite charges attract)


The second one is the covalent bond between the O and H atoms. The electrons present in this bond are shared between the atoms, which means that both atoms share the electrons in order to fill the valence electron shells.