Aluminum sulfate, also known as alum, is a chemical compound with the formula Al2(SO4)3. It is a white, crystalline solid that is highly soluble in water and is commonly used in various industrial and commercial applications, including water treatment, paper manufacturing, and pharmaceuticals. One of the key properties of aluminum sulfate is its molar mass, which is a measure of the total mass of a mole of the substance.
Calculating the Molar Mass of Aluminum Sulfate
To calculate the molar mass of aluminum sulfate, we need to know the atomic masses of its constituent elements, which are aluminum (Al), sulfur (S), and oxygen (O). The atomic masses of these elements are approximately 26.98 g/mol for aluminum, 32.06 g/mol for sulfur, and 16.00 g/mol for oxygen. The formula for aluminum sulfate is Al2(SO4)3, which means that one mole of the compound contains 2 moles of aluminum, 3 moles of sulfur, and 12 moles of oxygen.
Step-by-Step Calculation
The molar mass of aluminum sulfate can be calculated as follows:
- 2 moles of aluminum: 2 x 26.98 g/mol = 53.96 g/mol
- 3 moles of sulfur: 3 x 32.06 g/mol = 96.18 g/mol
- 12 moles of oxygen: 12 x 16.00 g/mol = 192.00 g/mol
The total molar mass of aluminum sulfate is the sum of the molar masses of its constituent elements: 53.96 g/mol + 96.18 g/mol + 192.00 g/mol = 342.14 g/mol.
| Element | Atomic Mass (g/mol) | Number of Moles | Molar Mass Contribution (g/mol) |
|---|---|---|---|
| Aluminum (Al) | 26.98 | 2 | 53.96 |
| Sulfur (S) | 32.06 | 3 | 96.18 |
| Oxygen (O) | 16.00 | 12 | 192.00 |
| Total | 342.14 |
Key Points
- The molar mass of aluminum sulfate is 342.14 g/mol.
- The calculation of the molar mass involves summing the atomic masses of the constituent elements, taking into account the number of moles of each element in the compound.
- Aluminum sulfate is a widely used chemical compound with applications in water treatment, paper manufacturing, and pharmaceuticals.
- The molar mass of aluminum sulfate is an important property in many of its applications, including the calculation of dosages and the optimization of reaction conditions.
- Understanding the molar mass of aluminum sulfate requires knowledge of the atomic masses of its constituent elements and the ability to calculate the total molar mass of the compound.
Applications of Aluminum Sulfate
Aluminum sulfate has a wide range of applications due to its unique properties, including its high solubility in water and its ability to form a gel-like substance when mixed with water. Some of the most common applications of aluminum sulfate include:
- Water treatment: Aluminum sulfate is used as a coagulant to remove impurities and contaminants from water.
- Paper manufacturing: Aluminum sulfate is used to size paper, improving its strength and water resistance.
- Pharmaceuticals: Aluminum sulfate is used as an excipient in some pharmaceutical products, helping to stabilize and enhance the delivery of active ingredients.
Technical Specifications
Aluminum sulfate is available in various forms, including anhydrous and hydrated forms. The anhydrous form of aluminum sulfate has a molar mass of 342.14 g/mol, while the hydrated form has a molar mass that depends on the number of water molecules present in the compound.
The hydrated form of aluminum sulfate is commonly used in water treatment applications, where it is used to remove impurities and contaminants from water.What is the molar mass of aluminum sulfate?
+The molar mass of aluminum sulfate is 342.14 g/mol.
What are the common applications of aluminum sulfate?
+Aluminum sulfate is commonly used in water treatment, paper manufacturing, and pharmaceuticals.
How is the molar mass of aluminum sulfate calculated?
+The molar mass of aluminum sulfate is calculated by summing the atomic masses of its constituent elements, taking into account the number of moles of each element in the compound.
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