onsider the mixing of aqueous solutions of lead(II) nitrate and sodium iodide to form a solid.
. Name the possible products, and determine the formulas of these possible products.
. What is the precipitate? How do you know?
. Must the subscript for an ion in a reactant stay the same as the subscript of that ion in a product? Explain your answer.
(a)
Interpretation:
To write the name of product and formula of product when lead nitrate,
Concept Introduction:
A balanced chemical equation is an equation that contains same number of atoms as well as of each element of reactants and products of reaction.
For example, the reaction between lead sulphide and oxygen is as follows:
In balanced chemical equation the numbers of atoms of each element on each side means product as well reactants of reaction are always equal. Calculate the number of atoms of reactants and products as follows:
In the given reaction, the number of all atoms, on the both sides are equal hence this is a balance reaction.
The most common driving forces which create product in chemical reactions are as follows:
- Formation of a solid.
- Formation of water.
- Transfer of electrons.
- Formation of gas.
Answer to Problem 1ALQ
Lead iodide
Explanation of Solution
Precipitation reaction means formation of solids or formation of any Precipitate; when solutions of two ionic substances are mixed and any solid will forms in the solution mixture, the reaction is known as Precipitation reaction.
The name of product and formula of product when lead nitrate,
(b)
Interpretation:
The precipitate formed on mixing of lead nitrate,
Concept Introduction:
There are following solubility rules:
- The salts formed from sodium, potassium and ammonium ions are soluble in nature.
All sulfate salts are soluble except
All nitrate salts are soluble. The formula of nitrate polyatomic ion is
All the salts formed from chloride, bromide and iodide are soluble except those with
All sulfate salts are insoluble except
All sulfides are insoluble except
All oxides and hydroxides are insoluble except
All carbonates are insoluble except
Answer to Problem 1ALQ
Explanation of Solution
According to rule, all the salts formed from chloride, bromide and iodide are soluble except those with
When lead nitrate,
Therefore, precipitate formed is
(c)
Interpretation:
When lead nitrate,
Concept Introduction:
Molecular equation:
The equation which shows all of reactants and products in molecular or un-dissociated form is known as Molecular equation. For example, the Molecular equation of solutions of potassium bromide and silver nitrate is as follows:
Complete ionic equation:
In the complete ionic equation, the strong electrolytes indicate by as ions. For example, the complete ionic equation of solutions of potassium bromide and silver nitrate is following
Net ionic equation:
In the net ionic equation there is no any spectator ion, only those species or ions which undergoes change is present called net ionic equation. For example, the net ionic equation of solutions of potassium bromide and silver nitrate is following:
Answer to Problem 1ALQ
To balance the number of atoms and charge.
Explanation of Solution
When lead nitrate,
For the above reaction, the complete ionic equation can be written as follows:
Here, subscript of each ions on left side are equal to the subscript of the same ion on right side to balance the number of atoms and charge on both side of the reaction arrow.
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Chapter 7 Solutions
Introductory Chemistry: A Foundation
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- Which of the following statements is/are true regarding solutions? l type='a'> If a solute is dissolved in water, then the resulting solution is considered aqueous. i>If two solutions are mixed and no chemical reaction occurs, then a net ionic equation cannot be written. i>If two clear solutions are mixed and then cloudiness results, this indicates that a precipitate formed.arrow_forwardThe traditional method of analysis for the amount of chloride ion present in a sample is to dissolve the sample in water and then slowly to add a solution of silver nitrate. Silver chloride ¡s very insoluble in water, and by adding a slight excess of silver nitrate, it is possible to effectively remove all chloride ion from the sample. :math>Ag+(aq)+Cl+(aq)AgCl(s) ppose a 1.054-g sample is known to contain 10.3% chloride ion by mass. What mass of silver nitrate must be used to completely precipitate the chloride ion from the sample? What mass of silver chloride will be obtained?arrow_forwardOn the basis of the general solubility rules given in Table 4.1, predict the identity of the precipitate that forms when the following aqueous solutions are mixed. If no precipitate forms, indicate which rules apply.arrow_forward
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