Write a net ionic equation for any precipitation reaction that occurs when 1 M solutions of the following are mixed.
(a) copper(II) sulfate and sodium chloride
(b) manganese(II) nitrate and ammonium hydroxide
(c) silver nitrate and hydrochloric acid
(d) nickel(II) sulfate and potassium hydroxide
(e) ammonium carbonate and sodium nitrate
(a)
Interpretation:
The net ionic equation should be written when copper(II) sulfate and sodium chloride are mixed.
Concept introduction:
Solubility of any compound is predicted by above solubility chart.
Blank boxes indicate no precipitate formation occurs which means soluble in dilute solution.
Boxes with grey small box 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 9QAP
No precipitation occurs.
Explanation of Solution
Copper(II) sulfate:
Sodium chloride:
Reaction for the solution of copper(II) sulfate and sodium chloride is written as:
Reactants:
Ions in solution:
Ions in solution:
Products:
Ions in solution:
Ions in solution:
Now,
(b)
Interpretation:
The net ionic equation should be written when manganese(II) nitrate and ammonium hydroxide are mixed.
Concept introduction:
Solubility of any compound is predicted by above solubility chart.
Blank boxes indicate no precipitate formation occurs which means soluble in dilute solution.
Boxes with grey small box 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 9QAP
Precipitation occurs
The net ionic equation is:
Explanation of Solution
Manganese(II) nitrate:
Ammonium hydroxide:
Reaction for the solution of manganese(II) nitrate and ammonium 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 silver nitrate and hydrochloric acid are mixed.
Concept introduction:
Solubility of any compound is predicted by above solubility chart.
Blank boxes indicate no precipitate formation occurs which means soluble in dilute solution.
Boxes with grey small box 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 9QAP
Precipitation occurs
The net ionic equation is:
Explanation of Solution
Silver nitrate:
Hydrochloric acid:
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 (
(d)
Interpretation:
The net ionic equation should be written when nickel(II) sulfate and potassium hydroxide are mixed.
Concept introduction:
Solubility of any compound is predicted by above solubility chart.
Blank boxes indicate no precipitate formation occurs which means soluble in dilute solution.
Boxes with grey small box 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 9QAP
Precipitation occurs
The net ionic equation is:
Explanation of Solution
Nickel(II) sulfate:
Potassium hydroxide:
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 (
(e)
Interpretation:
The net ionic equation should be written when ammonium carbonate and sodium nitrate are mixed.
Concept introduction:
Solubility of any compound is predicted by above solubility chart.
Blank boxes indicate no precipitate formation occurs which means soluble in dilute solution.
Boxes with grey small box 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 9QAP
No precipitation occurs.
Explanation of Solution
Ammonium carbonate:
Sodium nitrate:
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,
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Chapter 4 Solutions
Chemistry: Principles and Reactions
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