Given The Chemical Reaction:${ 2 \text{NaOH} + \text{H}_2\text{SO}_4 \rightarrow 2 \text{H}_2\text{O} + \text{Na}_2\text{SO}_4 } 1. H O W M A N Y G R A M S O F S O D I U M S U L F A T E W I L L B E F O R M E D I F Y O U S T A R T W I T H 200 G R A M S O F S O D I U M H Y D R O X I D E ? − − − 1. How Many Grams Of Sodium Sulfate Will Be Formed If You Start With 200 Grams Of Sodium Hydroxide?--- 1. Ho W Man Y G R Am So F So D I U M S U L F A T E W I Ll B E F Or M E D I F Yo U S T A R Tw I T H 200 G R Am So F So D I U Mh Y D Ro X I D E ? − − − [ 2

Understanding the Chemical Reaction

The given chemical reaction is a classic example of a double displacement reaction between sodium hydroxide (NaOH) and sulfuric acid (H2SO4). The reaction produces sodium sulfate (Na2SO4) and water (H2O). The balanced chemical equation is:

${ 2 \text{NaOH} + \text{H}_2\text{SO}_4 \rightarrow 2 \text{H}_2\text{O} + \text{Na}_2\text{SO}_4 }$

Calculating the Molar Mass of Sodium Sulfate

To determine the number of grams of sodium sulfate formed, we need to calculate the molar mass of sodium sulfate. The molar mass of sodium sulfate (Na2SO4) is the sum of the atomic masses of its constituent elements:

• Sodium (Na): 22.99 g/mol
• Sulfur (S): 32.07 g/mol
• Oxygen (O): 16.00 g/mol

The molar mass of sodium sulfate is:

${ 2(22.99) + 32.07 + 4(16.00) = 142.04 \text{ g/mol} }$

Determining the Limiting Reactant

To determine the number of grams of sodium sulfate formed, we need to identify the limiting reactant. In this case, we are given 200 grams of sodium hydroxide. We need to calculate the number of moles of sodium hydroxide and sulfuric acid.

The molar mass of sodium hydroxide (NaOH) is:

${ 22.99 + 16.00 + 1.01 = 40.00 \text{ g/mol} }$

The number of moles of sodium hydroxide is:

${ \frac{200 \text{ g}}{40.00 \text{ g/mol}} = 5.00 \text{ mol} }$

The number of moles of sulfuric acid is:

${ \frac{100 \text{ g}}{98.08 \text{ g/mol}} = 1.02 \text{ mol} }$

Since the reaction requires a 2:1 ratio of sodium hydroxide to sulfuric acid, the number of moles of sulfuric acid required is:

${ 2(5.00) = 10.0 \text{ mol} }$

Since we only have 1.02 mol of sulfuric acid, it is the limiting reactant.

Calculating the Number of Moles of Sodium Sulfate Formed

Since sulfuric acid is the limiting reactant, we can calculate the number of moles of sodium sulfate formed using the stoichiometry of the reaction:

${ 1.02 \text{ mol} \text{ H}_2\text{SO}_4 \times \frac{1 \text{ mol} \text{ Na}_2\text{SO}_4}{1 \text{ mol} \text{ H}_2\text{SO}_4} = 1.02 \text{ mol} \text{ Na}_2\text{SO}_4 }$

Calculating the Mass of Sodium Sulfate Formed

The mass of sodium sulfate formed is:

${ 1.02 \text{ mol} \times 142.04 \text{ g/mol} = 144.41 \text{ g} }$

Therefore, approximately 144.41 grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide.

Conclusion

In conclusion, the given chemical reaction between sodium hydroxide and sulfuric acid produces sodium sulfate and water. By identifying the limiting reactant and using the stoichiometry of the reaction, we can calculate the number of moles and mass of sodium sulfate formed. In this case, approximately 144.41 grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide.

References

• "Chemical Equations and Reactions" by OpenStax
• "General Chemistry" by Linus Pauling

Additional Resources

• Khan Academy: Chemical Reactions and Equations
• Crash Course: Chemistry
• Chemistry LibreTexts: Chemical Reactions and Equations
  Frequently Asked Questions (FAQs) about Sodium Sulfate Formation ====================================================================

Q: What is the chemical equation for the reaction between sodium hydroxide and sulfuric acid?

A: The chemical equation for the reaction between sodium hydroxide and sulfuric acid is:

${ 2 \text{NaOH} + \text{H}_2\text{SO}_4 \rightarrow 2 \text{H}_2\text{O} + \text{Na}_2\text{SO}_4 }$

Q: What is the molar mass of sodium sulfate?

A: The molar mass of sodium sulfate (Na2SO4) is 142.04 g/mol.

Q: How do I determine the limiting reactant in a chemical reaction?

A: To determine the limiting reactant, you need to calculate the number of moles of each reactant and compare it to the stoichiometry of the reaction. In this case, we calculated the number of moles of sodium hydroxide and sulfuric acid and found that sulfuric acid is the limiting reactant.

Q: How do I calculate the number of moles of sodium sulfate formed?

A: To calculate the number of moles of sodium sulfate formed, you need to use the stoichiometry of the reaction. Since sulfuric acid is the limiting reactant, we can calculate the number of moles of sodium sulfate formed by multiplying the number of moles of sulfuric acid by the stoichiometric ratio.

Q: How do I calculate the mass of sodium sulfate formed?

A: To calculate the mass of sodium sulfate formed, you need to multiply the number of moles of sodium sulfate by its molar mass.

Q: What is the relationship between sodium hydroxide and sodium sulfate?

A: Sodium hydroxide (NaOH) and sodium sulfate (Na2SO4) are related through a double displacement reaction, where sodium hydroxide reacts with sulfuric acid to form sodium sulfate and water.

Q: Can I use this reaction to produce sodium sulfate on a large scale?

A: Yes, this reaction can be used to produce sodium sulfate on a large scale. However, you need to consider the stoichiometry of the reaction, the limiting reactant, and the molar masses of the reactants and products.

Q: What are some common applications of sodium sulfate?

A: Sodium sulfate has several common applications, including:

• Detergent manufacturing
• Textile manufacturing
• Paper manufacturing
• Food processing

Q: Is sodium sulfate safe to handle?

A: Sodium sulfate is generally safe to handle, but it can be irritating to the skin and eyes. You should wear protective gear, including gloves and goggles, when handling sodium sulfate.

Q: Can I dispose of sodium sulfate in the environment?

A: No, you should not dispose of sodium sulfate in the environment. Sodium sulfate can contaminate soil and water, and it can also harm aquatic life. You should dispose of sodium sulfate according to local regulations and guidelines.

Conclusion

In conclusion, the reaction between sodium hydroxide and sulfuric acid produces sodium sulfate and water. By understanding the chemical equation, stoichiometry, and molar masses of the reactants and products, you can calculate the number of moles and mass of sodium sulfate formed. We hope this FAQ article has provided you with a better understanding of this reaction and its applications.