Aluminium hydroxide has the chemical formula Al(OH)3. It is an inorganic compound consisting of one aluminum atom bonded to three hydroxide ions.
Aluminium hydroxide is commonly found as a white, gelatinous solid. It is insoluble in water but can dissolve in acids and bases. It is widely used in various applications, including as an antacid to neutralize stomach acid, as an ingredient in certain medications, and as a flame retardant in plastics and coatings. Aluminium hydroxide is also used in water treatment processes to remove impurities and as a filler in the production of ceramics, paper, and rubber.
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The structural formula of aluminium hydroxide is represented as Al(OH)3. It consists of an aluminum (Al) atom at the center, bonded to three hydroxide (OH) groups.
The hydroxide groups are composed of one oxygen (O) atom bonded to a hydrogen (H) atom. The structural formula shows the arrangement and bonding of atoms in the compound, providing a visual representation of its molecular structure.
In conclusion, aluminium hydroxide (Al(OH)3) is a compound with diverse applications and benefits. Its chemical formula reflects its composition, consisting of aluminium ions (Al3+) and hydroxide ions (OH-) held together by ionic bonds. Aluminium hydroxide is widely used as an antacid to relieve symptoms of heartburn and indigestion. It acts by neutralizing excess stomach acid and providing relief to the digestive system. Additionally, aluminium hydroxide is employed as a phosphate binder in patients with kidney disease to reduce the levels of phosphates in the blood. It also finds application as a vaccine adjuvant to enhance immune responses and as a fire retardant in various materials to delay the spread of flames. Furthermore, aluminium hydroxide serves as a filler and pigment in industries such as plastics, paints, and coatings, improving strength, stability, and coloration. Its properties make it a valuable compound in various sectors, showcasing its versatility and significance in different applications.
Example 1: What is the balanced chemical equation for the reaction between aluminium hydroxide and hydrochloric acid?
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Solution: The balanced chemical equation for this reaction can be written as:
2Al(OH)3 + 6HCl → 2AlCl3 + 6H2O
Example 2: When 50 grams of aluminium hydroxide reacts with excess sulfuric acid, how many grams of aluminium sulfate will be formed?
Solution: First, we need to calculate the molar mass of aluminium hydroxide:
Al(OH)3 = (1 × 26.98 g/mol) + (3 × 16.00 g/mol) + (3 × 1.01 g/mol) = 78.00 g/mol
Next, we calculate the number of moles of aluminium hydroxide:
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moles = mass / molar mass = 50 g / 78.00 g/mol = 0.641 moles
From the balanced chemical equation, we can see that the molar ratio between aluminium hydroxide and aluminium sulfate is 1:1. Therefore, the number of moles of aluminium sulfate formed will also be 0.641 moles.
Finally, we calculate the mass of aluminium sulfate:
mass = moles × molar mass
= 0.641 moles × (1 × 26.98 g/mol + 1 × 32.07 g/mol + 4 × 16.00 g/mol)
= 54.7 g
So, 50 grams of aluminium hydroxide will produce 54.7 grams of aluminium sulfate.
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This post was last modified on 28/03/2024 01:40
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