Determine The Mass Of Sodium Nitrate Produced When 0.73 Grams Of Nickel (II) Nitrate Reacts With Sodium Hydroxide According To The Following Unbalanced Chemical Equation:$[ \text{Ni(NO}_3\text{)}_2(aq) + \text{NaOH}(aq) \rightarrow

Introduction

In this article, we will determine the mass of sodium nitrate produced when 0.73 grams of nickel (II) nitrate reacts with sodium hydroxide according to the given unbalanced chemical equation. To solve this problem, we need to first balance the chemical equation, then calculate the number of moles of nickel (II) nitrate and sodium hydroxide, and finally use the mole ratio to find the mass of sodium nitrate produced.

Balancing the Chemical Equation

The given unbalanced chemical equation is:

${ \text{Ni(NO}_3\text{)}_2(aq) + \text{NaOH}(aq) \rightarrow \text{Ni(OH)}_2(s) + \text{NaNO}_3(aq) }$

To balance the equation, we need to make sure that the number of atoms of each element is the same on both the reactant and product sides. The balanced equation is:

${ \text{Ni(NO}_3\text{)}_2(aq) + 2\text{NaOH}(aq) \rightarrow \text{Ni(OH)}_2(s) + 2\text{NaNO}_3(aq) }$

Calculating the Number of Moles of Nickel (II) Nitrate

To calculate the number of moles of nickel (II) nitrate, we need to know its molar mass. The molar mass of nickel (II) nitrate is 182.7 g/mol. We can calculate the number of moles of nickel (II) nitrate using the formula:

${ \text{moles} = \frac{\text{mass}}{\text{molar mass}} }$

Substituting the values, we get:

${ \text{moles of Ni(NO}_3\text{)}_2 = \frac{0.73 \text{ g}}{182.7 \text{ g/mol}} = 0.004 \text{ mol} }$

Calculating the Number of Moles of Sodium Hydroxide

To calculate the number of moles of sodium hydroxide, we need to know its molar mass. The molar mass of sodium hydroxide is 40 g/mol. Since the balanced equation shows that 2 moles of sodium hydroxide react with 1 mole of nickel (II) nitrate, we can calculate the number of moles of sodium hydroxide as follows:

${ \text{moles of NaOH} = 2 \times \text{moles of Ni(NO}_3\text{)}_2 = 2 \times 0.004 \text{ mol} = 0.008 \text{ mol} }$

Calculating the Mass of Sodium Nitrate Produced

To calculate the mass of sodium nitrate produced, we need to know its molar mass. The molar mass of sodium nitrate is 84 g/mol. Since the balanced equation shows that 2 moles of sodium nitrate are produced for every 1 mole of nickel (II) nitrate, we can calculate the mass of sodium nitrate produced as follows:

${ \text{mass of NaNO}_3 = 2 \times \text{moles of Ni(NO}_3\text{)}_2 \times \text{molar mass of NaNO}_3 }$ ${ \text{mass of NaNO}_3 = 2 \times 0.004 \text{ mol} \times 84 \text{ g/mol} = 0.672 \text{ g} }$

Conclusion

In this article, we determined the mass of sodium nitrate produced when 0.73 grams of nickel (II) nitrate reacts with sodium hydroxide according to the given unbalanced chemical equation. We first balanced the chemical equation, then calculated the number of moles of nickel (II) nitrate and sodium hydroxide, and finally used the mole ratio to find the mass of sodium nitrate produced. The mass of sodium nitrate produced is 0.672 grams.

Limitations of the Calculation

The calculation assumes that the reaction is 100% efficient and that no side reactions occur. In reality, the reaction may not be 100% efficient, and side reactions may occur, which can affect the actual mass of sodium nitrate produced.

Future Work

To improve the accuracy of the calculation, we can consider the following:

• Measure the actual mass of sodium nitrate produced using a balance or other analytical technique.
• Account for any side reactions that may occur during the reaction.
• Use a more accurate value for the molar mass of sodium nitrate.

References

• [1] "Chemical Equations" by OpenStax. CC BY 4.0.
• [2] "Molar Mass" by Wikipedia. CC BY-SA 3.0.

Glossary

• Molar mass: The mass of one mole of a substance.
• Mole ratio: The ratio of the number of moles of one substance to the number of moles of another substance.
• Balanced equation: A chemical equation in which the number of atoms of each element is the same on both the reactant and product sides.
  Frequently Asked Questions (FAQs) =====================================

Q: What is the purpose of balancing a chemical equation?

A: Balancing a chemical equation is essential to ensure that the number of atoms of each element is the same on both the reactant and product sides. This is crucial for predicting the amount of product formed and the amount of reactant consumed.

Q: How do I determine the number of moles of a substance?

A: To determine the number of moles of a substance, you need to know its molar mass and its mass. You can use the formula: moles = mass / molar mass.

Q: What is the mole ratio in a chemical reaction?

A: The mole ratio is the ratio of the number of moles of one substance to the number of moles of another substance. It is essential to determine the mole ratio to predict the amount of product formed and the amount of reactant consumed.

Q: How do I calculate the mass of a product formed in a chemical reaction?

A: To calculate the mass of a product formed in a chemical reaction, you need to know its molar mass and the number of moles of the product. You can use the formula: mass = moles x molar mass.

Q: What are some common sources of error in calculating the mass of a product formed in a chemical reaction?

A: Some common sources of error in calculating the mass of a product formed in a chemical reaction include:

• Inaccurate values for the molar mass of the product
• Inaccurate values for the number of moles of the product
• Failure to account for side reactions or other factors that may affect the amount of product formed

Q: How can I improve the accuracy of my calculations?

A: To improve the accuracy of your calculations, you can:

• Use more accurate values for the molar mass of the product
• Use more accurate values for the number of moles of the product
• Account for side reactions or other factors that may affect the amount of product formed
• Use a more precise analytical technique to measure the mass of the product

Q: What are some real-world applications of calculating the mass of a product formed in a chemical reaction?

A: Some real-world applications of calculating the mass of a product formed in a chemical reaction include:

• Predicting the yield of a chemical reaction in a manufacturing process
• Determining the amount of product formed in a chemical reaction in a laboratory setting
• Calculating the amount of reactant consumed in a chemical reaction
• Predicting the amount of waste produced in a chemical reaction

Glossary

• Molar mass: The mass of one mole of a substance.
• Mole ratio: The ratio of the number of moles of one substance to the number of moles of another substance.
• Balanced equation: A chemical equation in which the number of atoms of each element is the same on both the reactant and product sides.
• Side reaction: A reaction that occurs in addition to the main reaction, often resulting in the formation of unwanted products.

References

• [] "Chemical Equations" by OpenStax. CC BY 4.0.
• [2] "Molar Mass" by Wikipedia. CC BY-SA 3.0.
• [3] "Chemical Reactions" by Khan Academy. CC BY-NC-SA 4.0.

Further Reading

• "Chemical Equations" by OpenStax
• "Molar Mass" by Wikipedia
• "Chemical Reactions" by Khan Academy