cipitate and aqueous sodium iodide. (b) Aqueous solutions of nickel(II) sulfate and mercury(I) nitrate react to give a mercury(I) sulfate precipitate and aqueous nickel(II) nitrate. the llowing double-
cipitate and aqueous sodium iodide. (b) Aqueous solutions of nickel(II) sulfate and mercury(I) nitrate react to give a mercury(I) sulfate precipitate and aqueous nickel(II) nitrate. the llowing double-
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question 72 part B.
I answered the question but I am not sure if it’s correct. Thank you
![**Title: Understanding Reactions of Nickel(II) Sulfate and Mercury(I) Nitrate Solutions**
**Introduction**
In this lesson, we will explore the reaction between aqueous solutions of nickel(II) sulfate and mercury(I) nitrate. The main products of this reaction are mercury(I) sulfate as a precipitate and aqueous nickel(II) nitrate.
**Chemical Reaction**
The balanced chemical equation for the reaction is:
\[ \text{NiSO}_4 (aq) + \text{Hg}_2(\text{NO}_3)_2 (aq) \rightarrow \text{Hg}_2\text{SO}_4(s) + \text{Ni}(\text{NO}_3)_2 (aq) \]
**Balancing the Reaction**
- Each compound is assigned an oxidation state and the atoms are balanced accordingly.
- The equation above is already balanced, showing the conservation of mass.
**Solubility Information**
- \(\text{NiSO}_4\) is soluble in water.
- \(\text{Hg}_2(\text{NO}_3)_2\) is soluble in water.
- \(\text{Hg}_2\text{SO}_4\) is insoluble, leading to its formation as a precipitate.
- \(\text{Ni}(\text{NO}_3)_2\) is soluble in water.
**Conclusion**
From this reaction, it is important to note the solubility rules that dictate the formation of precipitates. Understanding these rules allows chemists to predict the outcomes of reactions and understand separation processes.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1db2cc66-1337-4fa7-be4a-e8027b848fd1%2F46092d3e-448d-4541-8fb6-f0eb2093e0ed%2F3pkxmnp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Understanding Reactions of Nickel(II) Sulfate and Mercury(I) Nitrate Solutions**
**Introduction**
In this lesson, we will explore the reaction between aqueous solutions of nickel(II) sulfate and mercury(I) nitrate. The main products of this reaction are mercury(I) sulfate as a precipitate and aqueous nickel(II) nitrate.
**Chemical Reaction**
The balanced chemical equation for the reaction is:
\[ \text{NiSO}_4 (aq) + \text{Hg}_2(\text{NO}_3)_2 (aq) \rightarrow \text{Hg}_2\text{SO}_4(s) + \text{Ni}(\text{NO}_3)_2 (aq) \]
**Balancing the Reaction**
- Each compound is assigned an oxidation state and the atoms are balanced accordingly.
- The equation above is already balanced, showing the conservation of mass.
**Solubility Information**
- \(\text{NiSO}_4\) is soluble in water.
- \(\text{Hg}_2(\text{NO}_3)_2\) is soluble in water.
- \(\text{Hg}_2\text{SO}_4\) is insoluble, leading to its formation as a precipitate.
- \(\text{Ni}(\text{NO}_3)_2\) is soluble in water.
**Conclusion**
From this reaction, it is important to note the solubility rules that dictate the formation of precipitates. Understanding these rules allows chemists to predict the outcomes of reactions and understand separation processes.
Transcribed Image Text:**Exercise 72: Write a balanced chemical equation for each of the following double-replacement reactions.**
(a) Aqueous solutions of chromium(III) iodide and sodium hydroxide react to give a chromium(III) hydroxide precipitate and aqueous sodium iodide.
(b) Aqueous solutions of nickel(II) sulfate and mercury(I) nitrate react to give mercury(I) sulfate precipitate and aqueous nickel(II) nitrate.
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