Aqueous Sodium Phosphate And Aqueous Iron (III) Chloride React To Produce Aqueous Sodium Chloride And Solid Iron (III) Phosphate. What Is The Balanced Net Ionic Equation For The Reaction?$[ \text{Fe}^{3+}_{(aq)} + \text{PO} 4^{3-} {(aq)}

by ADMIN 238 views

Aqueous Sodium Phosphate and Aqueous Iron (III) Chloride Reaction: Balanced Net Ionic Equation

In this article, we will explore the reaction between aqueous sodium phosphate and aqueous iron (III) chloride to produce aqueous sodium chloride and solid iron (III) phosphate. The balanced net ionic equation for this reaction will be determined, providing a deeper understanding of the chemical process involved.

The chemical reaction between aqueous sodium phosphate and aqueous iron (III) chloride can be represented by the following equation:

Na3PO4(aq)+FeCl3(aq)→NaCl(aq)+FePO4(s){ \text{Na}_3\text{PO}_4(aq) + \text{FeCl}_3(aq) \rightarrow \text{NaCl}(aq) + \text{FePO}_4(s) }

Step 1: Write the Unbalanced Equation

The first step in writing the balanced net ionic equation is to write the unbalanced equation. In this case, the unbalanced equation is already provided:

Na3PO4(aq)+FeCl3(aq)→NaCl(aq)+FePO4(s){ \text{Na}_3\text{PO}_4(aq) + \text{FeCl}_3(aq) \rightarrow \text{NaCl}(aq) + \text{FePO}_4(s) }

Step 2: Break Down the Compounds into Ions

The next step is to break down the compounds into their respective ions. This will help us identify the ions that are involved in the reaction.

  • Aqueous sodium phosphate (Na3PO4) breaks down into:
    • 3Na+ (sodium ions)
    • PO43- (phosphate ions)
  • Aqueous iron (III) chloride (FeCl3) breaks down into:
    • Fe3+ (iron (III) ions)
    • 3Cl- (chloride ions)
  • Aqueous sodium chloride (NaCl) breaks down into:
    • Na+ (sodium ions)
    • Cl- (chloride ions)
  • Solid iron (III) phosphate (FePO4) breaks down into:
    • Fe3+ (iron (III) ions)
    • PO43- (phosphate ions)

Step 3: Write the Net Ionic Equation

The net ionic equation is written by removing the spectator ions, which are ions that appear on both sides of the equation and do not participate in the reaction.

In this case, the spectator ions are the sodium ions (Na+) and the chloride ions (Cl-). The net ionic equation is:

{ \text{Fe}^{3+}_{(aq)} + \text{PO}_4^{3-}_{(aq)} \rightarrow \text{FePO}_4(s) }

Step 4: Balance the Net Ionic Equation

The final step is to balance the net ionic equation. In this case, the equation is already balanced.

In conclusion, the balanced net ionic equation for the reaction between aqueous sodium phosphate and aqueous iron (III) chloride to produce aqueous sodium chloride and solid iron (III) phosphate is:

{ \text{Fe}^{3+}_{(aq)} + \text{PO}_4^{3-}_{(aq)} \rightarrow \text{FePO}_4(s) }

This equation provides a clear understanding of the chemical process involved in the reaction and can be used to predict the products of the reaction.

  • The balanced net ionic equation is a crucial concept in chemistry that helps us understand the chemical process involved in a reaction.
  • The net ionic equation is written by removing the spectator ions, which are ions that appear on both sides of the equation and do not participate in the reaction.
  • The balanced net ionic equation can be used to predict the products of a reaction.
  • What is the balanced net ionic equation for the reaction between aqueous sodium phosphate and aqueous iron (III) chloride?
    • The balanced net ionic equation is: { \text{Fe}^{3+}_{(aq)} + \text{PO}_4^{3-}_{(aq)} \rightarrow \text{FePO}_4(s) }
  • What are the spectator ions in the reaction between aqueous sodium phosphate and aqueous iron (III) chloride?
    • The spectator ions are the sodium ions (Na+) and the chloride ions (Cl-).
  • Petrucci, R. H., Harwood, W. S., Herring, F. G., & Madura, J. D. (2007). General chemistry: Principles and modern applications. Pearson Prentice Hall.
  • Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.
    Aqueous Sodium Phosphate and Aqueous Iron (III) Chloride Reaction: Q&A

In our previous article, we explored the reaction between aqueous sodium phosphate and aqueous iron (III) chloride to produce aqueous sodium chloride and solid iron (III) phosphate. We also determined the balanced net ionic equation for this reaction. In this article, we will answer some frequently asked questions related to this reaction.

Q1: What is the balanced net ionic equation for the reaction between aqueous sodium phosphate and aqueous iron (III) chloride?

A1: The balanced net ionic equation is: { \text{Fe}^{3+}_{(aq)} + \text{PO}_4^{3-}_{(aq)} \rightarrow \text{FePO}_4(s) }

Q2: What are the spectator ions in the reaction between aqueous sodium phosphate and aqueous iron (III) chloride?

A2: The spectator ions are the sodium ions (Na+) and the chloride ions (Cl-).

Q3: What is the role of the iron (III) ions in the reaction?

A3: The iron (III) ions (Fe3+) act as the reactant in the reaction, combining with the phosphate ions (PO43-) to form solid iron (III) phosphate (FePO4).

Q4: What is the role of the phosphate ions in the reaction?

A4: The phosphate ions (PO43-) act as the reactant in the reaction, combining with the iron (III) ions (Fe3+) to form solid iron (III) phosphate (FePO4).

Q5: What is the product of the reaction between aqueous sodium phosphate and aqueous iron (III) chloride?

A5: The product of the reaction is solid iron (III) phosphate (FePO4) and aqueous sodium chloride (NaCl).

Q6: What is the significance of the balanced net ionic equation in chemistry?

A6: The balanced net ionic equation is a crucial concept in chemistry that helps us understand the chemical process involved in a reaction. It provides a clear understanding of the reactants, products, and the chemical process involved in the reaction.

Q7: How can the balanced net ionic equation be used to predict the products of a reaction?

A7: The balanced net ionic equation can be used to predict the products of a reaction by identifying the reactants and the chemical process involved in the reaction.

Q8: What are some common mistakes to avoid when writing the balanced net ionic equation?

A8: Some common mistakes to avoid when writing the balanced net ionic equation include:

  • Not breaking down the compounds into their respective ions
  • Not removing the spectator ions
  • Not balancing the equation

Q9: How can the balanced net ionic equation be used in real-world applications?

A9: The balanced net ionic equation can be used in real-world applications such as:

  • Predicting the products of a reaction
  • Understanding the chemical process involved in a reaction
  • Designing new chemical reactions

Q10: What are some resources available for learning more about the balanced net ionic equation?

A10: Some resources available for learning more about the balanced net ionic equation include:

  • Textbooks on general chemistry
  • Online resources such as Khan Academy and Crash Course
  • Scientific journals and articles

In conclusion, the balanced net ionic equation is a crucial concept in chemistry that helps us understand the chemical process involved in a reaction. By answering some frequently asked questions related to this reaction, we have provided a deeper understanding of the balanced net ionic equation and its significance in chemistry.

  • The balanced net ionic equation is a crucial concept in chemistry that helps us understand the chemical process involved in a reaction.
  • The balanced net ionic equation can be used to predict the products of a reaction.
  • The balanced net ionic equation can be used in real-world applications such as predicting the products of a reaction and understanding the chemical process involved in a reaction.
  • What is the balanced net ionic equation for the reaction between aqueous sodium phosphate and aqueous iron (III) chloride?
    • The balanced net ionic equation is: { \text{Fe}^{3+}_{(aq)} + \text{PO}_4^{3-}_{(aq)} \rightarrow \text{FePO}_4(s) }
  • What are the spectator ions in the reaction between aqueous sodium phosphate and aqueous iron (III) chloride?
    • The spectator ions are the sodium ions (Na+) and the chloride ions (Cl-).
  • Petrucci, R. H., Harwood, W. S., Herring, F. G., & Madura, J. D. (2007). General chemistry: Principles and modern applications. Pearson Prentice Hall.
  • Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.