Chapter 9, Problem 9.60E

Interpretation Introduction

(a)

Interpretation:

The molecular, total ionic and net ionic equations to represent the neutralization reaction between $\text{KOH}$ and ${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}$ are to be stated.

Concept introduction:

In acid-base reaction, an acid reacts with a base to from a salt and water. Acid-base reaction is also known as neutralization reaction. A general acid-base reaction is represented as,

$\begin{array}{ccccccc}\text{HA}& +& \text{BOH}& \rightleftharpoons & \text{BA}& +& {\text{H}}_{\text{2}}\text{O}\\ \text{Acid}& & \text{Base}& & \text{Salt}& & \text{Water}\end{array}$

Answer to Problem 9.60E

The molecular, total ionic and net ionic equations to represent the neutralization reaction between $\text{KOH}$ and ${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}$ respectively are,

$\begin{array}{c}2\text{KOH}\left(\text{aq}\right)+{\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}\left(\text{aq}\right)\to {\text{K}}_{\text{2}}{\text{HPO}}_4\left(\text{aq}\right)+2{\text{H}}_{\text{2}}\text{O}\left(l\right)\\ 2{\text{K}}^{+}\left(\text{aq}\right)+2{\text{OH}}^{-}\left(\text{aq}\right)+2{\text{H}}^{+}\left(\text{aq}\right)+{\text{HPO}}_4{}^{2-}\left(\text{aq}\right)\to 2{\text{K}}^{+}\left(\text{aq}\right)+{\text{HPO}}_{\text{4}}{}^{2-}\left(\text{aq}\right)+2{\text{H}}_{\text{2}}\text{O}\left(l\right)\\ 2{\text{OH}}^{-}\left(\text{aq}\right)+2{\text{H}}^{+}\left(\text{aq}\right)\to 2{\text{H}}_{\text{2}}\text{O}\left(l\right)\end{array}$

Explanation of Solution

In acid-base reaction, an acid reacts with a base to from a salt and water. Acid-base reaction is also known as neutralization reaction.

The balanced molecular ionic equation reaction between $\text{KOH}$ and ${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}$ is,

$2\text{KOH}\left(\text{aq}\right)+{\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}\left(\text{aq}\right)\to {\text{K}}_{\text{2}}{\text{HPO}}_4\left(\text{aq}\right)+2{\text{H}}_{\text{2}}\text{O}\left(l\right)$

The balanced total ionic equation reaction between $\text{KOH}$ and ${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}$ is,

$2{\text{K}}^{+}\left(\text{aq}\right)+2{\text{OH}}^{-}\left(\text{aq}\right)+2{\text{H}}^{+}\left(\text{aq}\right)+{\text{HPO}}_4{}^{2-}\left(\text{aq}\right)\to 2{\text{K}}^{+}\left(\text{aq}\right)+{\text{HPO}}_{\text{4}}{}^{2-}\left(\text{aq}\right)+2{\text{H}}_{\text{2}}\text{O}\left(l\right)$ ${\text{K}}^{+}$ and ${\text{HPO}}_4{}^{2-}$ ion is common on the both sides of the complete ionic reaction therefore, to write net ionic reaction these ions must be eliminated from the reaction.

The balanced net ionic equation reaction between $\text{KOH}$ and ${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}$ is,

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

Conclusion

The molecular, total ionic and net ionic equations to represent the neutralization reaction between $\text{KOH}$ and ${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}$ are,

$\begin{array}{c}2\text{KOH}\left(\text{aq}\right)+{\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}\left(\text{aq}\right)\to {\text{K}}_{\text{2}}{\text{HPO}}_4\left(\text{aq}\right)+2{\text{H}}_{\text{2}}\text{O}\left(l\right)\\ 2{\text{K}}^{+}\left(\text{aq}\right)+2{\text{OH}}^{-}\left(\text{aq}\right)+2{\text{H}}^{+}\left(\text{aq}\right)+{\text{HPO}}_4{}^{2-}\left(\text{aq}\right)\to 2{\text{K}}^{+}\left(\text{aq}\right)+{\text{HPO}}_{\text{4}}{}^{2-}\left(\text{aq}\right)+2{\text{H}}_{\text{2}}\text{O}\left(l\right)\\ 2{\text{OH}}^{-}\left(\text{aq}\right)+2{\text{H}}^{+}\left(\text{aq}\right)\to 2{\text{H}}_{\text{2}}\text{O}\left(l\right)\end{array}$

Interpretation Introduction

(b)

Interpretation:

The molecular, total ionic and net ionic equations to represent the neutralization reaction between $\text{KOH}$ and ${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}$ are to be stated.

Concept introduction:

In acid-base reaction, an acid reacts with a base to from a salt and water. Acid-base reaction is also known as neutralization reaction. A general acid-base reaction is represented as,

$\begin{array}{ccccccc}\text{HA}& +& \text{BOH}& \rightleftharpoons & \text{BA}& +& {\text{H}}_{\text{2}}\text{O}\\ \text{Acid}& & \text{Base}& & \text{Salt}& & \text{Water}\end{array}$

Answer to Problem 9.60E

The molecular, total ionic and net ionic equations to represent the neutralization reaction between $\text{KOH}$ and ${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}$ are,

$\begin{array}{c}3\text{KOH}\left(\text{aq}\right)+{\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}\left(\text{aq}\right)\to {\text{K}}_{\text{3}}{\text{PO}}_4\left(\text{aq}\right)+3{\text{H}}_{\text{2}}\text{O}\left(l\right)\\ 3{\text{K}}^{+}\left(\text{aq}\right)+3{\text{OH}}^{-}\left(\text{aq}\right)+3{\text{H}}^{+}\left(\text{aq}\right)+{\text{PO}}_4{}^{3-}\left(\text{aq}\right)\to 3{\text{K}}^{+}\left(\text{aq}\right)+{\text{PO}}_{\text{4}}{}^{3-}\left(\text{aq}\right)+3{\text{H}}_{\text{2}}\text{O}\left(l\right)\\ 3{\text{OH}}^{-}\left(\text{aq}\right)+3{\text{H}}^{+}\left(\text{aq}\right)\to 3{\text{H}}_{\text{2}}\text{O}\left(l\right)\end{array}$

Explanation of Solution

In acid-base reaction, an acid reacts with a base to from a salt and water. Acid-base reaction is also known as neutralization reaction.

The balanced molecular ionic equation reaction between $\text{KOH}$ and ${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}$ is,

$3\text{KOH}\left(\text{aq}\right)+{\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}\left(\text{aq}\right)\to {\text{K}}_{\text{3}}{\text{PO}}_4\left(\text{aq}\right)+3{\text{H}}_{\text{2}}\text{O}\left(l\right)$

The balanced total ionic equation reaction between $\text{KOH}$ and ${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}$ is,

$3{\text{K}}^{+}\left(\text{aq}\right)+3{\text{OH}}^{-}\left(\text{aq}\right)+3{\text{H}}^{+}\left(\text{aq}\right)+{\text{PO}}_4{}^{3-}\left(\text{aq}\right)\to 3{\text{K}}^{+}\left(\text{aq}\right)+{\text{PO}}_{\text{4}}{}^{3-}\left(\text{aq}\right)+3{\text{H}}_{\text{2}}\text{O}\left(l\right)$

The ${\text{K}}^{+}$ and ${\text{PO}}_4{}^{3-}$ ion is common on the both sides of the complete ionic reaction therefore, to write net ionic reaction these ions must be eliminated from the reaction.

The balanced net ionic equation reaction between $\text{KOH}$ and ${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}$ is,

$3{\text{OH}}^{-}\left(\text{aq}\right)+3{\text{H}}^{+}\left(\text{aq}\right)\to 3{\text{H}}_{\text{2}}\text{O}\left(l\right)$

Conclusion

The molecular, total ionic and net ionic equations to represent the neutralization reaction between $\text{KOH}$ and ${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}$ are,

$\begin{array}{c}3\text{KOH}\left(\text{aq}\right)+{\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}\left(\text{aq}\right)\to {\text{K}}_{\text{3}}{\text{PO}}_4\left(\text{aq}\right)+3{\text{H}}_{\text{2}}\text{O}\left(l\right)\\ 3{\text{K}}^{+}\left(\text{aq}\right)+3{\text{OH}}^{-}\left(\text{aq}\right)+3{\text{H}}^{+}\left(\text{aq}\right)+{\text{PO}}_4{}^{3-}\left(\text{aq}\right)\to 3{\text{K}}^{+}\left(\text{aq}\right)+{\text{PO}}_{\text{4}}{}^{3-}\left(\text{aq}\right)+3{\text{H}}_{\text{2}}\text{O}\left(l\right)\\ 3{\text{OH}}^{-}\left(\text{aq}\right)+3{\text{H}}^{+}\left(\text{aq}\right)\to 3{\text{H}}_{\text{2}}\text{O}\left(l\right)\end{array}$

Interpretation Introduction

(c)

Interpretation:

The molecular, total ionic and net ionic equations to represent the neutralization reaction between $\text{KOH}$ and ${\text{H}}_{\text{2}}{\text{C}}_2{\text{O}}_{\text{4}}$ are to be stated.

Concept introduction:

In acid-base reaction, an acid reacts with a base to from a salt and water. Acid-base reaction is also known as neutralization reaction. A general acid-base reaction is represented as,

$\begin{array}{ccccccc}\text{HA}& +& \text{BOH}& \rightleftharpoons & \text{BA}& +& {\text{H}}_{\text{2}}\text{O}\\ \text{Acid}& & \text{Base}& & \text{Salt}& & \text{Water}\end{array}$

Answer to Problem 9.60E

The molecular, total ionic and net ionic equations to represent the neutralization reaction between $\text{KOH}$ and ${\text{H}}_{\text{2}}{\text{C}}_2{\text{O}}_{\text{4}}$ are,

$\begin{array}{c}\text{KOH}\left(\text{aq}\right)+{\text{H}}_{\text{2}}{\text{C}}_2{\text{O}}_{\text{4}}\left(\text{aq}\right)\to {\text{KHC}}_2{\text{O}}_4\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(l\right)\\ {\text{K}}^{+}\left(\text{aq}\right)+{\text{OH}}^{-}\left(\text{aq}\right)+{\text{H}}^{+}\left(\text{aq}\right)+{\text{HC}}_2{\text{O}}_4{}^{-}\left(\text{aq}\right)\to {\text{K}}^{+}\left(\text{aq}\right)+{\text{HC}}_2{\text{O}}_4{}^{-}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(l\right)\\ {\text{OH}}^{-}\left(\text{aq}\right)+{\text{H}}^{+}\left(\text{aq}\right)\to {\text{H}}_{\text{2}}\text{O}\left(l\right)\end{array}$

Explanation of Solution

In acid-base reaction, an acid reacts with a base to from a salt and water. Acid-base reaction is also known as neutralization reaction.

The balanced molecular ionic equation reaction between $\text{KOH}$ and ${\text{H}}_{\text{2}}{\text{C}}_2{\text{O}}_{\text{4}}$ is,

$\text{KOH}\left(\text{aq}\right)+{\text{H}}_{\text{2}}{\text{C}}_2{\text{O}}_{\text{4}}\left(\text{aq}\right)\to {\text{KHC}}_2{\text{O}}_4\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(l\right)$

The balanced total ionic equation reaction between $\text{KOH}$ and ${\text{H}}_{\text{2}}{\text{C}}_2{\text{O}}_{\text{4}}$ is,

${\text{K}}^{+}\left(\text{aq}\right)+{\text{OH}}^{-}\left(\text{aq}\right)+{\text{H}}^{+}\left(\text{aq}\right)+{\text{HC}}_2{\text{O}}_4{}^{-}\left(\text{aq}\right)\to {\text{K}}^{+}\left(\text{aq}\right)+{\text{HC}}_2{\text{O}}_4{}^{-}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(l\right)$

The ${\text{K}}^{+}$ and ${\text{HC}}_2{\text{O}}_4{}^{-}$ ion is common on the both sides of the complete ionic reaction therefore, to write net ionic reaction these ions must be eliminated from the reaction.

The balanced net ionic equation reaction between $\text{KOH}$ and ${\text{H}}_{\text{2}}{\text{C}}_2{\text{O}}_{\text{4}}$ is,

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

Conclusion

The molecular, total ionic and net ionic equations to represent the neutralization reaction between $\text{KOH}$ and ${\text{H}}_{\text{2}}{\text{C}}_2{\text{O}}_{\text{4}}$ are,

$\begin{array}{c}\text{KOH}\left(\text{aq}\right)+{\text{H}}_{\text{2}}{\text{C}}_2{\text{O}}_{\text{4}}\left(\text{aq}\right)\to {\text{KHC}}_2{\text{O}}_4\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(l\right)\\ {\text{K}}^{+}\left(\text{aq}\right)+{\text{OH}}^{-}\left(\text{aq}\right)+{\text{H}}^{+}\left(\text{aq}\right)+{\text{HC}}_2{\text{O}}_4{}^{-}\left(\text{aq}\right)\to {\text{K}}^{+}\left(\text{aq}\right)+{\text{HC}}_2{\text{O}}_4{}^{-}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(l\right)\\ {\text{OH}}^{-}\left(\text{aq}\right)+{\text{H}}^{+}\left(\text{aq}\right)\to {\text{H}}_{\text{2}}\text{O}\left(l\right)\end{array}$