(a)
Interpretation:
Net ionic equation has to be written for the formation of precipitate and the spectator ions has to be identified in the reaction between
(a)
Explanation of Solution
The reaction given is between aqueous solutions of
Aqueous solution of
The balanced chemical equation for the reaction is given as follows:
Complete ionic equation is written by showing the ions present in aqueous solution. This is given as follows:
In the complete ionic equation, the common ions that are present on both sides of the equation is known as spectator ions. Thus in this case, the spectator ions are
Thus net ionic equation can be written as follows:
(b)
Interpretation:
Net ionic equation has to be written for the formation of precipitate and the spectator ions has to be identified in the reaction between
(b)
Explanation of Solution
The reaction given is between aqueous solutions of
Aqueous solution of
The balanced chemical equation for the reaction is given as follows:
Complete ionic equation is written by showing the ions present in aqueous solution. This is given as follows:
In the complete ionic equation, the common ions that are present on both sides of the equation is known as spectator ions. Thus in this case, the spectator ions are
Thus net ionic equation can be written as follows:
(c)
Interpretation:
Net ionic equation has to be written for the formation of precipitate and the spectator ions has to be identified in the reaction between
(c)
Explanation of Solution
The reaction given is between aqueous solutions of
Aqueous solution of
The balanced chemical equation for the reaction is given as follows:
Complete ionic equation is written by showing the ions present in aqueous solution. This is given as follows:
In the complete ionic equation, the common ions that are present on both sides of the equation is known as spectator ions. Thus in this case, the spectator ions are
Thus net ionic equation can be written as follows:
(d)
Interpretation:
Net ionic equation has to be written for the formation of precipitate and the spectator ions has to be identified in the reaction between
(d)
Explanation of Solution
The reaction given is between aqueous solutions of
Aqueous solution of
The balanced chemical equation for the reaction is given as follows:
Complete ionic equation is written by showing the ions present in aqueous solution. This is given as follows:
In the complete ionic equation, the common ions that are present on both sides of the equation is known as spectator ions. Thus in this case, the spectator ions are
Thus net ionic equation can be written as follows:
(e)
Interpretation:
Net ionic equation has to be written for the formation of precipitate and the spectator ions has to be identified in the reaction between
(e)
Explanation of Solution
The reaction given is between aqueous solutions of
Aqueous solution of
The balanced chemical equation for the reaction is given as follows:
Complete ionic equation is written by showing the ions present in aqueous solution. This is given as follows:
In the complete ionic equation, the common ions that are present on both sides of the equation is known as spectator ions. Thus in this case, the spectator ions are
Thus net ionic equation can be written as follows:
Want to see more full solutions like this?
Chapter F Solutions
Chemical Principles: The Quest for Insight
- If aqueous solutions of potassium carbonate and copper(II) nitrate are mixed, a precipitate is formed. Write the complete and net ionic equations for this reaction, and name the precipitate.arrow_forwardAn aqueous sample is known to contain either Mg2+ or Ba2+ ions. Treatment of the sample with Na2CO3 produces a precipitate, but treatment with ammonium sulfate does not. Use the solubility rules (see Table 4.1) to determine which cation is present.arrow_forwardWrite the net ionic equation for the reaction, if any, that occurs on mixing (a) solutions of sodium hydroxide and magnesium chloride. (b) solutions of sodium nitrate and magnesium bromide. (c) magnesium metal and a solution of hydrochloric acid to produce magnesium chloride and hydrogen. Magnesium metal reacting with HCl.arrow_forward
- If aqueous solutions of potassium sulfide and iron(III) chloride are mixed, a precipitate is formed. Write the complete and net ionic equations for this reaction, and name the precipitate.arrow_forwardA student weighs out a 4.80-g sample of aluminum bromide, transfers it to a 100-mL volumetric flask, adds enough water to dissolve it, and then adds water to the 100-mL mark. What is the molarity of aluminum bromide in the resulting solution?arrow_forwardummarize the simple solubility rules for ionic compounds. How do we use these rules in determining the identity of the solid formed in a precipitation reaction? Give examples including balanced complete and net ionic equations.arrow_forward
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningLiving By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHERChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning