Follow the directions for Question 9 for the following pairs of solutions.
(a) sodium phosphate and barium chloride
(b) zinc sulfate and potassium hydroxide
(c) ammonium sulfate and sodium chloride
(d) cobalt(III) nitrate and sodium phosphate
(a)
Interpretation:
The net ionic equation should be written when sodium phosphate and barium chloride are mixed.
Concept introduction:
Solubility of any compound is predicted by below solubility chart:
Group-1 cations and |
||||||
Group-2 cations | - | - | ||||
Transitions metal cations |
- | - | - |
Blank boxes indicate no precipitate formation occurs which means soluble in dilute solution.
Boxes with hyphen will form precipitate from dilute solutions and boxes where formula is written this is a cation-anion combination that will form precipitate.
Precipitation reactions: It is a type of chemical reactions where two soluble salts react with each other and formed different products, out of which one product must be insoluble in solution which is known as precipitate.
A chemical equation which shows only the species that are participated in the reaction is said to be net ionic equation.
Answer to Problem 10QAP
Precipitation occurs
The net ionic equation is:
Explanation of Solution
Sodium phosphate:
Barium chloride:
Reaction for the solution of sodium phosphate and barium chloride is written as:
Reactants:
Ions in solution:
Ions in solution:
Products:
Ions in solution:
Ions in solution:
Now,
So, the equation will be:
Now, cancelling out the ions which appear on both sides of the equation (
(b)
Interpretation:
The net ionic equation should be written when zinc sulfate and potassium hydroxide are mixed.
Concept introduction:
Solubility of any compound is predicted by above solubility chart.
Group-1 cations and |
||||||
Group-2 cations | - | - | ||||
Transitions metal cations |
- | - | - |
Blank boxes indicate no precipitate formation occurs which means soluble in dilute solution.
Boxes with hyphen will form precipitate from dilute solutions and boxes where formula is written this is a cation-anion combination that will form precipitate.
Precipitation reactions: It is a type of chemical reactions where two soluble salts react with each other and formed different products, out of which one product must be insoluble in solution which is known as precipitate.
A chemical equation which shows only the species that are participated in the reaction is said to be net ionic equation.
Answer to Problem 10QAP
Precipitation occurs
The net ionic equation is:
Explanation of Solution
Zinc sulfate:
Potassium hydroxide:
Reaction for the solution of zinc sulfate and potassium hydroxide is written as:
Reactants:
Ions in solution:
Ions in solution:
Products:
Ions in solution:
Ions in solution:
Now,
So, the equation will be:
Now, cancelling out the ions which appear on both sides of the equation (
(c)
Interpretation:
The net ionic equation should be written when ammonium sulfate and sodium chloride are mixed.
Concept introduction:
Solubility of any compound is predicted by below solubility chart:
Group-1 cations and |
||||||
Group-2 cations | - | - | ||||
Transitions metal cations |
- | - | - |
Blank boxes indicate no precipitate formation occurs which means soluble in dilute solution.
Boxes with hyphen will form precipitate from dilute solutions and boxes where formula is written this is a cation-anion combination that will form precipitate.
Precipitation reactions: It is a type of chemical reactions where two soluble salts react with each other and formed different products, out of which one product must be insoluble in solution which is known as precipitate.
A chemical equation which shows only the species that are participated in the reaction is said to be net ionic equation.
Answer to Problem 10QAP
No precipitation occurs.
Explanation of Solution
Ammonium sulfate:
Sodium chloride:
Reaction for the solution of silver nitrate and hydrochloric acid is written as:
Reactants:
Ions in solution:
Ions in solution:
Products:
Ions in solution:
Ions in solution:
Now,
(d)
Interpretation:
The net ionic equation should be written when cobalt(II) nitrate and sodium phosphate are mixed.
Concept introduction:
Solubility of any compound is predicted by below solubility chart:
Group-1 cations and
|
||||||
Group-2 cations | - | - | ||||
Transitions metal cations |
- | - | - |
Blank boxes indicate no precipitate formation occurs which means soluble in dilute solution.
Boxes with hyphen will form precipitate from dilute solutions and boxes where formula is written this is a cation-anion combination that will form precipitate.
Precipitation reactions: It is a type of chemical reactions where two soluble salts react with each other and formed different products, out of which one product must be insoluble in solution which is known as precipitate.
A chemical equation which shows only the species that are participated in the reaction is said to be net ionic equation.
Answer to Problem 10QAP
Precipitation occurs
The net ionic equation is:
Explanation of Solution
Cobalt(II) nitrate:
Sodium phosphate:
Reaction for the solution of silver nitrate and hydrochloric acid is written as:
Reactants:
Ions in solution:
Ions in solution:
Products:
Ions in solution:
Ions in solution:
Now,
So, the equation will be:
Now, cancelling out the ions which appear on both sides of the equation (
Want to see more full solutions like this?
Chapter 4 Solutions
Chemistry: Principles and Reactions
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY