Answered

Explore Westonci.ca, the leading Q&A site where experts provide accurate and helpful answers to all your questions. Find reliable answers to your questions from a wide community of knowledgeable experts on our user-friendly Q&A platform. Get precise and detailed answers to your questions from a knowledgeable community of experts on our Q&A platform.

What else is produced during the replacement reaction of silver nitrate and potassium sulfate?

[tex]\[ 2 \text{AgNO}_3 + \text{K}_2\text{SO}_4 \rightarrow \text{Ag}_2\text{SO}_4 + \][/tex]
A. [tex]\(\text{KNO}_3\)[/tex]
B. [tex]\(2 \text{KNO}_3\)[/tex]
C. [tex]\(\text{K}_2\)[/tex]
D. [tex]\(2 \text{AgNO}_3\)[/tex]

Sagot :

GinnyAnswer
Certainly! Let's consider the given chemical equation:

[tex]\[ 2 \, \text{AgNO}_3 + \text{K}_2\text{SO}_4 \rightarrow \text{Ag}_2\text{SO}_4 + \text{ ? } \][/tex]

This is a double displacement reaction where the ions of the reacting compounds exchange their partners to form new compounds.

### Step-by-Step Solution:

1. Identify Reactants and Products:
- Reactants:
- Silver nitrate ([tex]\(\text{AgNO}_3\)[/tex])
- Potassium sulfate ([tex]\(\text{K}_2\text{SO}_4\)[/tex])
- Products:
- Silver sulfate ([tex]\(\text{Ag}_2\text{SO}_4\)[/tex])
- The other product needs to be determined.

2. Determine the Ionic Forms:
- Silver nitrate ([tex]\(\text{AgNO}_3\)[/tex]) dissociates into [tex]\(\text{Ag}^+\)[/tex] and [tex]\(\text{NO}_3^-\)[/tex].
- Potassium sulfate ([tex]\(\text{K}_2\text{SO}_4\)[/tex]) dissociates into [tex]\(\text{K}^+\)[/tex] and [tex]\(\text{SO}_4^{2-}\)[/tex].

3. Recombine the Ions:
- [tex]\(\text{Ag}^+\)[/tex] will combine with [tex]\(\text{SO}_4^{2-}\)[/tex] to form silver sulfate ([tex]\(\text{Ag}_2\text{SO}_4\)[/tex]).
- [tex]\(\text{K}^+\)[/tex] will combine with [tex]\(\text{NO}_3^-\)[/tex] to form potassium nitrate ([tex]\(\text{KNO}_3\)[/tex]).

4. Balance the Chemical Equation:
- Start by writing the unbalanced equation:
[tex]\[ \text{AgNO}_3 + \text{K}_2\text{SO}_4 \rightarrow \text{Ag}_2\text{SO}_4 + \text{KNO}_3 \][/tex]
- Balance the silver (Ag) atoms:
[tex]\[ 2 \, \text{AgNO}_3 + \text{K}_2\text{SO}_4 \rightarrow \text{Ag}_2\text{SO}_4 + \text{KNO}_3 \][/tex]
- Now balance the potassium (K) atoms by ensuring that the potassium atoms on both sides are equal:
[tex]\[ 2 \, \text{AgNO}_3 + \text{K}_2\text{SO}_4 \rightarrow \text{Ag}_2\text{SO}_4 + 2 \, \text{KNO}_3 \][/tex]

### Final Equation:
[tex]\[ 2 \, \text{AgNO}_3 + \text{K}_2\text{SO}_4 \rightarrow \text{Ag}_2\text{SO}_4 + 2 \, \text{KNO}_3 \][/tex]

Thus, the other product formed during the reaction of silver nitrate ([tex]\(\text{AgNO}_3\)[/tex]) and potassium sulfate ([tex]\(\text{K}_2\text{SO}_4\)[/tex]) is:

[tex]\[ \boxed{2 \, \text{KNO}_3} \][/tex]

So, the correct choice is [tex]\(2 \, \text{KNO}_3\)[/tex], which corresponds to option 2.
We appreciate your visit. Our platform is always here to offer accurate and reliable answers. Return anytime. Thank you for your visit. We're committed to providing you with the best information available. Return anytime for more. Stay curious and keep coming back to Westonci.ca for answers to all your burning questions.