Q. 10.14 - An Introduction to General, Organic, and Biological Chemistry

Question

Identify the Bronsted-Lowry acid-base pairs in each of the following equations:

a. ${\mathrm{H}}_3{\mathrm{PO}}_4\left(aq\right)+{\mathrm{H}}_2\mathrm{O}\left(l\right)\rightleftarrows {\mathrm{H}}_2{\mathrm{PO}}_4^{-}\left(aq\right)+{\mathrm{H}}_3{\mathrm{O}}^{+}\left(aq\right)$

b. ${\mathrm{CO}}_3{}^{2-}(aq)+{\mathrm{H}}_2\mathrm{O}(l)\rightleftarrows {\mathrm{HCO}}_3^{-}(aq)+{\mathrm{OH}}^{-}(aq)$

c. ${\mathrm{H}}_3{\mathrm{PO}}_4\left(aq\right)+{\mathrm{NH}}_3\left(aq\right)\rightleftarrows {\mathrm{H}}_2{\mathrm{PO}}_4^{-}\left(aq\right)+{\mathrm{NH}}_4^{+}\left(aq\right)$

Step-by-Step Solution

Answer

Part a. the conjugate acid-base pair ${\mathrm{H}}_3{\mathrm{PO}}_4$ and ${\mathrm{H}}_2{{\mathrm{PO}}_4}^{-}$ along with ${\mathrm{H}}_{2}O$ and${\mathrm{H}}_3{O}^{+}$

Part b. the conjugate acid-base pair ${\mathrm{H}}_{2}O$ and $O{H}^{-}$ along with $C{O}_3^{2-}$ and $HC{O}_3^{-}$

Part c. the conjugate acid-base pair ${\mathrm{H}}_3{\mathrm{PO}}_4$ and ${\mathrm{H}}_2{{\mathrm{PO}}_4}^{-}$ along with $N{H}_3$ and $N{H}_4^{+}$

Step 1: Given information part(a)

The objective is to solve the following equation for the Bronsted-Lowry acid-base pairs.

Step 2: Explanation part(a)

a)$H_{3}P{O}_4$ contributes $H^{+} to H_{2}O$ in the statement. The conjugate base was $H_{2}P{O}_4^{-}$, and the conjugate acid was $H_3{O}^{+}$. The conjugation acid-base pair includes ${\mathrm{H}}_3{\mathrm{PO}}_4$ and ${\mathrm{H}}_2{{\mathrm{PO}}_4}^{-}$moreover ${\mathrm{H}}_{2}O$ and ${\mathrm{H}}_3{O}^{+}$.

Step 3: Given information part(b)

The task is to solve the following equation for the Bronsted-Lowry acid-base pairs.

Step 4: Explanation part(b)

b) $H_{2}O$ donates $H^{+} to C{O}_3^{2-}$ throughout the reaction. The conjugate base is obtained, and the conjugate acid is obtained as $HC{O}_3^{-}$. ${\mathrm{H}}_{2}O$ and $O{H}^{-}$moreover $C{O}_3^{2-}$ and $HC{O}_3^{-}$ Consider the acid-base pair in conjugation.

Step 5: Given information part(c)

The task is to solve the given equation for the Bronsted-Lowry acid-base pairs.

Step 6: Explanation part(c)

c) In the process Phosphoric acid (${\mathrm{H}}_3{\mathrm{PO}}_4$)releases ${\mathrm{H}}^{+}$ and ${\mathrm{NH}}_3$ receives it . The conjugate base of  phosphoric acid is${\mathrm{H}}_2{\mathrm{PO}}_4^{-}$, and the conjugate acid of Ammonia is${\mathrm{NH}}_4^{+}$. In this instance, the conjugate acid-base pairs are  ⁣${\mathrm{H}}_3{\mathrm{PO}}_4$ and ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}$ along with ${\mathrm{NH}}_3$ and${\mathrm{NH}}_4^{+}$