How Many Moles Of Aluminum Ions \left( Al^{3+} \right ] Are Present In 0.46 Mol Of A L 2 ( S O 4 ) 3 Al_2\left( SO_4 \right)_3 A L 2 ( S O 4 ) 3 ?Express The Number Of Moles To Two Significant Figures. N A L 3 + = □ Mol N_{Al^{3+}} = \square \, \text{mol} N A L 3 + = □ Mol

Mar 9, 2025 by ADMIN 282 views

How Many Moles of Aluminum Ions are Present in 0.46 mol of $Al_2\left( SO_4 \right)_3$ ?

Understanding the Chemical Formula

The chemical formula $Al_2\left( SO_4 \right)_3$ represents a compound composed of aluminum, sulfur, and oxygen. To determine the number of moles of aluminum ions present in this compound, we need to understand the relationship between the number of moles of the compound and the number of moles of aluminum ions.

Calculating the Number of Moles of Aluminum Ions

The chemical formula $Al_2\left( SO_4 \right)_3$ indicates that one mole of the compound contains two moles of aluminum ions. This is because the subscript "2" in front of the aluminum symbol (Al) indicates that there are two aluminum atoms in each molecule of the compound.

To calculate the number of moles of aluminum ions present in 0.46 mol of $Al_2\left( SO_4 \right)_3$ , we can use the following equation:

$n_{Al^{3+}} = 2 \times n_{Al_2\left( SO_4 \right)_3}$

where $n_{Al^{3+}}$ is the number of moles of aluminum ions and $n_{Al_2\left( SO_4 \right)_3}$ is the number of moles of the compound.

Substituting the Given Value

We are given that $n_{Al_2\left( SO_4 \right)_3} = 0.46$ mol. Substituting this value into the equation above, we get:

$n_{Al^{3+}} = 2 \times 0.46$

Performing the Calculation

To calculate the number of moles of aluminum ions, we multiply the number of moles of the compound by 2:

$n_{Al^{3+}} = 2 \times 0.46 = 0.92$

Expressing the Answer to Two Significant Figures

The number of moles of aluminum ions is 0.92 mol. To express this answer to two significant figures, we round the value to 0.9 mol.

Conclusion

In conclusion, the number of moles of aluminum ions present in 0.46 mol of $Al_2\left( SO_4 \right)_3$ is 0.9 mol.

Key Takeaways

The chemical formula $Al_2\left( SO_4 \right)_3$ indicates that one mole of the compound contains two moles of aluminum ions.
To calculate the number of moles of aluminum ions present in a given amount of the compound, we multiply the number of moles of the compound by 2.
The number of moles of aluminum ions can be expressed to two significant figures by rounding the value to the nearest tenth.

Additional Information

The chemical formula $Al_2\left( SO_4 \right)_3$ is a compound composed of aluminum, sulfur, and oxygen.
The subscript "2" in front of the aluminum symbol (Al) indicates that there are two aluminum atoms in each molecule of the compound.
The number of moles of a substance can be calculated using the formula: $n = \frac{m}{M}$ , where $n$ is the number of moles, $m$ is the mass of the substance, and $M$ is the molar mass of the substance.
Frequently Asked Questions (FAQs) About Calculating Moles of Aluminum Ions

Q: What is the chemical formula for aluminum sulfate?

A: The chemical formula for aluminum sulfate is $Al_2\left( SO_4 \right)_3$ .

Q: How many moles of aluminum ions are present in one mole of aluminum sulfate?

A: One mole of aluminum sulfate contains two moles of aluminum ions.

Q: How do I calculate the number of moles of aluminum ions present in a given amount of aluminum sulfate?

A: To calculate the number of moles of aluminum ions, multiply the number of moles of aluminum sulfate by 2.

Q: What is the relationship between the number of moles of aluminum sulfate and the number of moles of aluminum ions?

A: The number of moles of aluminum ions is twice the number of moles of aluminum sulfate.

Q: Can I express the number of moles of aluminum ions to two significant figures?

A: Yes, you can express the number of moles of aluminum ions to two significant figures by rounding the value to the nearest tenth.

Q: What is the molar mass of aluminum sulfate?

A: The molar mass of aluminum sulfate is 342.14 g/mol.

Q: How do I calculate the number of moles of aluminum sulfate using the molar mass?

A: To calculate the number of moles of aluminum sulfate, use the formula: $n = \frac{m}{M}$ , where $n$ is the number of moles, $m$ is the mass of the substance, and $M$ is the molar mass of the substance.

Q: What is the significance of the subscript "2" in front of the aluminum symbol (Al) in the chemical formula $Al_2\left( SO_4 \right)_3$ ?

A: The subscript "2" indicates that there are two aluminum atoms in each molecule of aluminum sulfate.

Q: Can I use the same calculation to determine the number of moles of aluminum ions in a different compound?

A: No, the calculation is specific to aluminum sulfate and cannot be used for other compounds.

Q: What are some common applications of aluminum sulfate?

A: Aluminum sulfate is commonly used as a coagulant in water treatment, as a mordant in dyeing and printing, and as a fire retardant.

Q: Is aluminum sulfate a strong acid or a weak acid?

A: Aluminum sulfate is a weak acid.

Q: Can I store aluminum sulfate in a household setting?

A: Yes, aluminum sulfate can be stored in a household setting, but it should be kept in a cool, dry place and away from children and pets.

Q: What are some safety precautions I should take when handling aluminum sulfate?

A: When handling aluminum sulfate, wear protective gloves and eyewear, and avoid inhaling the dust.