Chapter 17, Problem 2CR

Interpretation Introduction

Interpretation:

The relationship between the conjugate acid-base pair in a Bronsted-Lowry model is to be described. The balanced chemical equations for the given molecules/ions behaving as Bronsted-Lowry acids in water are to be stated and the balanced chemical equations for the given molecules/ions behaving as Bronsted-Lowry bases in water are to be stated.

Concept Introduction:

In a Bronsted-Lowry acid-base model, the conjugate acid is formed by accepting the proton by a base from acid and a conjugate base is formed by the donation of proton by an acid to a base.

Answer to Problem 2CR

The relationship between the conjugate acid-base pair in a Bronsted-Lowry model is rightfully stated.

The chemical equation for $\text{HCl}$ in water is shown below.

$\text{HCl}+{\text{H}}_2\text{O}\to {\text{H}}_3{\text{O}}^{+}+{\text{Cl}}^{-}$

The chemical equation for ${\text{H}}_2{\text{SO}}_4$ in water is shown below.

${\text{H}}_2{\text{SO}}_4+2{\text{H}}_2\text{O}\to 2{\text{H}}_3{\text{O}}^{+}+{\text{SO}}_4^{2-}$

The chemical equation for ${\text{H}}_3{\text{PO}}_4$ in water is shown below.

${\text{H}}_3{\text{PO}}_4+3{\text{H}}_2\text{O}\to 3{\text{H}}_3{\text{O}}^{+}+{\text{PO}}_4^{3-}$

The chemical equation for ${\text{NH}}_4^{+}$ in water is shown below.

${\text{NH}}_4^{+}+{\text{H}}_2\text{O}\to {\text{H}}_3{\text{O}}^{+}+{\text{NH}}_3$

The chemical equation for ${\text{NH}}_3$ in water is shown below.

${\text{NH}}_3+{\text{H}}_2\text{O}\to {\text{NH}}_4^{+}+{\text{OH}}^{-}$

The chemical equation for ${\text{HCO}}_3^{-}$ in water is shown below.

${\text{HCO}}_3^{-}+{\text{H}}_2\text{O}\to {\text{H}}_2{\text{CO}}_3+{\text{OH}}^{-}$

The chemical equation for ${\text{NH}}_2^{-}$ in water is shown below.

${\text{NH}}_2^{-}+{\text{H}}_2\text{O}\to {\text{NH}}_3+{\text{OH}}^{-}$

The chemical equation for ${\text{H}}_2{\text{PO}}_4^{-}$ in water is shown below.

${\text{H}}_2{\text{PO}}_4^{-}+{\text{H}}_2\text{O}\to {\text{H}}_3{\text{PO}}_4+{\text{OH}}^{-}$.

Explanation of Solution

The chemical equation for $\text{HCl}$ in water is shown below.

$\text{HCl}+{\text{H}}_2\text{O}\to {\text{H}}_3{\text{O}}^{+}+{\text{Cl}}^{-}$

The $\text{HCl}$ acts a Bronsted-Lowry acid and donates its proton to water. Chloride ion is the conjugate base.

The chemical equation for ${\text{H}}_2{\text{SO}}_4$ in water is shown below.

${\text{H}}_2{\text{SO}}_4+2{\text{H}}_2\text{O}\to 2{\text{H}}_3{\text{O}}^{+}+{\text{SO}}_4^{2-}$

The ${\text{H}}_2{\text{SO}}_4$ acts a Bronsted-Lowry acid and donates its proton to water. Sulfate ion is the conjugate base.

The chemical equation for ${\text{H}}_3{\text{PO}}_4$ in water is shown below.

${\text{H}}_3{\text{PO}}_4+3{\text{H}}_2\text{O}\to 3{\text{H}}_3{\text{O}}^{+}+{\text{PO}}_4^{3-}$

The ${\text{H}}_3{\text{PO}}_4$ acts a Bronsted-Lowry acid and donates its proton to water. Phosphate ion is the conjugate base.

The chemical equation for ${\text{NH}}_4^{+}$ in water is shown below.

${\text{NH}}_4^{+}+{\text{H}}_2\text{O}\to {\text{H}}_3{\text{O}}^{+}+{\text{NH}}_3$

The ${\text{H}}_2{\text{SO}}_4$ acts a Bronsted-Lowry acid and donates its proton to water. Ammonia is the conjugate base.

The chemical equation for ${\text{NH}}_3$ in water is shown below.

${\text{NH}}_3+{\text{H}}_2\text{O}\to {\text{NH}}_4^{+}+{\text{OH}}^{-}$

The ${\text{NH}}_3$ acts a Bronsted-Lowry base and accepts proton from water. Ammonium ion is the conjugate acid.

The chemical equation for ${\text{HCO}}_3^{-}$ in water is shown below.

${\text{HCO}}_3^{-}+{\text{H}}_2\text{O}\to {\text{H}}_2{\text{CO}}_3+{\text{OH}}^{-}$

The ${\text{HCO}}_3^{-}$ acts a Bronsted-Lowry base and accepts proton from water. Carbonic acid is the conjugate acid.

The chemical equation for ${\text{NH}}_2^{-}$ in water is shown below.

${\text{NH}}_2^{-}+{\text{H}}_2\text{O}\to {\text{NH}}_3+{\text{OH}}^{-}$

The ${\text{NH}}_2^{-}$ acts a Bronsted-Lowry base and accepts proton from water. Ammonia is the conjugate acid.

The chemical equation for ${\text{H}}_2{\text{PO}}_4^{-}$ in water is shown below.

${\text{H}}_2{\text{PO}}_4^{-}+{\text{H}}_2\text{O}\to {\text{H}}_3{\text{PO}}_4+{\text{OH}}^{-}$

The ${\text{H}}_2{\text{PO}}_4^{-}$ acts a Bronsted-Lowry base and accepts proton from water. Phosphoric acid is the conjugate acid.

Conclusion

The relationship between the conjugate acid-base pair in a Bronsted-Lowry model is rightfully stated.

The chemical equation for $\text{HCl}$ in water is shown below.

$\text{HCl}+{\text{H}}_2\text{O}\to {\text{H}}_3{\text{O}}^{+}+{\text{Cl}}^{-}$

The chemical equation for ${\text{H}}_2{\text{SO}}_4$ in water is shown below.

${\text{H}}_2{\text{SO}}_4+2{\text{H}}_2\text{O}\to 2{\text{H}}_3{\text{O}}^{+}+{\text{SO}}_4^{2-}$

The chemical equation for ${\text{H}}_3{\text{PO}}_4$ in water is shown below.

${\text{H}}_3{\text{PO}}_4+3{\text{H}}_2\text{O}\to 3{\text{H}}_3{\text{O}}^{+}+{\text{PO}}_4^{3-}$

The chemical equation for ${\text{NH}}_4^{+}$ in water is shown below.

${\text{NH}}_4^{+}+{\text{H}}_2\text{O}\to {\text{H}}_3{\text{O}}^{+}+{\text{NH}}_3$

The chemical equation for ${\text{NH}}_3$ in water is shown below.

${\text{NH}}_3+{\text{H}}_2\text{O}\to {\text{NH}}_4^{+}+{\text{OH}}^{-}$

The chemical equation for ${\text{HCO}}_3^{-}$ in water is shown below.

${\text{HCO}}_3^{-}+{\text{H}}_2\text{O}\to {\text{H}}_2{\text{CO}}_3+{\text{OH}}^{-}$

The chemical equation for ${\text{NH}}_2^{-}$ in water is shown below.

${\text{NH}}_2^{-}+{\text{H}}_2\text{O}\to {\text{NH}}_3+{\text{OH}}^{-}$

The chemical equation for ${\text{H}}_2{\text{PO}}_4^{-}$ in water is shown below.

${\text{H}}_2{\text{PO}}_4^{-}+{\text{H}}_2\text{O}\to {\text{H}}_3{\text{PO}}_4+{\text{OH}}^{-}$.