Chapter 11, Problem 56A

(a)

Interpretation Introduction

Interpretation:

The balanced net ionic equation needs to be determined for reaction ${\text{H}}_{\text{2}}{\text{C}}_{\text{2}}{\text{O}}_{\text{4}}+\text{KOH}\to \left[{\text{H}}_{\text{2}}\text{O}\right]$ and the product that is not ionized is given.

Concept Introduction:

A net ionic equation is an equation in which the ions that are participating directly in the reaction are included. Those ions which are not participating directly are called spectator ions and they are removed from the complete ionic equation to write net ionic equation.

Answer to Problem 56A

The balanced net ionic equation is ${\text{H}}^{\text{+}}\left(\text{aq}\right){\text{+ OH}}^{\text{-}}\left(\text{aq}\right)\to {\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$ .

Explanation of Solution

Chemical symbols and formulas are used for representing a chemical reaction where reactants are written on left side and chemical products are written on right side.

The chemical equation is balanced by making the number and types of atoms on left and right sides of the equation as same.

It is given that there is a reaction ${\text{H}}_{\text{2}}{\text{C}}_{\text{2}}{\text{O}}_{\text{4}}+\text{KOH}\to \left[{\text{H}}_{\text{2}}\text{O}\right]$ so, the balanced ionic equation becomes:

  ${\text{2H}}^{\text{+}}{\text{+C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}{\text{+2K}}^{\text{+}}{\text{+2OH}}^{\text{-}}\to {\text{2K}}^{\text{+}}{\text{+C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}{\text{+2H}}_{\text{2}}\text{O}$

The balanced net ionic equation shows the particles involved in the reaction with respect to mass and charge, so it is as:

  ${\text{H}}^{\text{+}}\left(\text{aq}\right){\text{+ OH}}^{\text{-}}\left(\text{aq}\right)\to {\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

(b)

Interpretation Introduction

Interpretation:

The balanced net ionic equation needs to be determined for reaction ${\text{Na}}_{\text{2}}\text{S}+\text{HCl}\to \left[{\text{H}}_{\text{2}}\text{S}\right]$ and the product that is not ionized is given.

Concept Introduction:

A balanced equation is a net ionic equation which shows the particles involved in the reaction with respect to mass and charge.

Answer to Problem 56A

The balanced net ionic equation is ${\text{ S}}^{2-}(aq)+2{\text{H}}^{+}(aq)\to {\text{H}}_{\text{2}}\text{S(g)}$ .

Explanation of Solution

Chemical symbols and formulas are used for representing a chemical reaction where reactants are written on left side and chemical products are written on right side.

The chemical equation is balanced by making the number and types of atoms on left and right sides of the equation as same.

It is given that there is a reaction ${\text{Na}}_{\text{2}}\text{S}+\text{HCl}\to \left[{\text{H}}_{\text{2}}\text{S}\right]$ so, the balanced ionic equation becomes :

  ${\text{2Na}}^{+}{\text{+ S}}^{2-}+2{\text{H}}^{+}{\text{+ 2Cl}}^{-}\to {\text{H}}_{\text{2}}\text{S}+2{\text{Na}}^{+}{\text{+2Cl}}^{-}$

The balanced net ionic equation shows the particles involved in the reaction with respect to mass and charge and the product that is ionized is sodium chloride so equation is as:

  ${\text{ S}}^{2-}(aq)+2{\text{H}}^{+}(aq)\to {\text{H}}_{\text{2}}\text{S(g)}$

(c)

Interpretation Introduction

Interpretation:

The balanced net ionic equation needs to be determined for reaction $\text{NaOH}+\text{Fe}{\left({\text{NO}}_{\text{3}}\right)}_3\to \left[\text{Fe}\left({\text{OH}}_3\right)\right]$ and the product that is not ionized is given.

Concept Introduction:

A balanced equation is a net ionic equation which shows the particles involved in the reaction with respect to mass and charge.

Answer to Problem 56A

The balanced net ionic equation is ${\text{Fe}}^{3+}+{\text{3OH}}^{-}\to \left[\text{Fe}\left({\text{OH}}_3\right)\right]$ .

Explanation of Solution

Chemical symbols and formulas are used for representing a chemical reaction where reactants are written on left side and chemical products are written on right side.

The chemical equation is balanced by making the number and types of atoms on left and right sides of the equation as same.

It is given that there is a reaction $\text{NaOH}+\text{Fe}{\left({\text{NO}}_{\text{3}}\right)}_3\to \left[\text{Fe}\left({\text{OH}}_3\right)\right]$ so, the balanced ionic equation becomes as:

  ${\text{3Na}}^{+}{\text{+ 3OH}}^{-}+{\text{Fe}}^{3+}+3{\text{NO}}_3{}^{-}\to \left[\text{Fe}\left({\text{OH}}_3\right)\right]+3{\text{Na}}^{+}+3{\text{NO}}_3{}^{-}$

The balanced net ionic equation shows the particles involved in the reaction with respect to mass and charge and the product that is ionized is sodium nitrate so equation is as:

  ${\text{Fe}}^{3+}+{\text{3OH}}^{-}\to \left[\text{Fe}\left({\text{OH}}_3\right)\right]$