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Chapter 18: Problem 21

Write balanced net ionic equations for the following reactions, and label the conjugate acid-base pairs: (a) \(\mathrm{HNO}_{3}(a q)+\mathrm{Li}_{2} \mathrm{CO}_{3}(a q) \rightleftharpoons \mathrm{LiNO}_{3}(a q)+\mathrm{LiHCO}_{3}(a q)\) (b) \(2 \mathrm{NH}_{4} \mathrm{Cl}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \rightleftharpoons 2 \mathrm{H}_{2} \mathrm{O}(I)+\mathrm{BaCl}_{2}(a q)+2 \mathrm{NH}_{3}(a q)\)

Short Answer

Expert verified
The net ionic equations are \(\mathrm{H}^{+}(aq) + \mathrm{CO}_{3}^{2-}(aq) \rightleftharpoons \mathrm{HCO}_{3}^{-}(aq)\) and \(2\mathrm{NH}_{4}^{+}(aq) + 2\mathrm{OH}^{-}(aq) \rightleftharpoons 2\mathrm{H}_{2} \mathrm{O}(l) + 2\mathrm{NH}_{3}(aq)\). The conjugate acid-base pairs are \(\mathrm{H}^{+}\)/\(\mathrm{HCO}_{3}^{-}\), \(\mathrm{CO}_{3}^{2-}\)/\(\mathrm{HCO}_{3}^{-}\), \(\mathrm{NH}_{4}^{+}\)/\(\mathrm{NH}_{3}\), and \(\mathrm{OH}^{-}\)/\(\mathrm{H}_{2} \mathrm{O}\).

Step by step solution

01

Identify the Reactants and Products

Begin by identifying all the reactants and products in each given reaction. For (a), the reactants are \(\mathrm{HNO}_{3}(aq)\) and \(\mathrm{Li}_{2}\mathrm{CO}_{3}(aq)\), and the products are \(\mathrm{LiNO}_{3}(aq)\) and \(\mathrm{LiHCO}_{3}(aq)\). For (b), the reactants are \(2\mathrm{NH}_{4} \mathrm{Cl}(aq)\) and \(\mathrm{Ba}(\mathrm{OH})_{2}(aq)\), and the products are \(2\ \mathrm{H}_{2} \mathrm{O}(l)\), \(\mathrm{BaCl}_{2}(aq)\), and \(2\ \mathrm{NH}_{3}(aq)\).
02

Write Complete Ionic Equations

Break each compound into its respective ions. For reaction (a), \(\mathrm{HNO}_{3}(aq) + \mathrm{Li}_{2}\mathrm{CO}_{3}(aq) \rightleftharpoons \mathrm{LiNO}_{3}(aq) + \mathrm{LiHCO}_{3}(aq)\): \[ \mathrm{H}^{+}(aq) + \mathrm{NO}_{3}^{-}(aq) + 2\mathrm{Li}^{+}(aq) + \mathrm{CO}_{3}^{2-}(aq) \rightleftharpoons 2\mathrm{Li}^{+}(aq) + \mathrm{NO}_{3}^{-}(aq) + \mathrm{Li}^{+}(aq) + \mathrm{HCO}_{3}^{-}(aq)\] For reaction (b), \(2\mathrm{NH}_{4} \mathrm{Cl}(aq) + \mathrm{Ba}(\mathrm{OH})_{2}(aq) \rightleftharpoons 2\mathrm{H}_{2} \mathrm{O}(l) + \mathrm{BaCl}_{2}(aq) + 2\mathrm{NH}_{3}(aq)\): \[2\mathrm{NH}_{4}^{+}(aq) + 2\mathrm{Cl}^{-}(aq) + \mathrm{Ba}^{2+}(aq) + 2\mathrm{OH}^{-}(aq) \rightleftharpoons 2\mathrm{H}_{2} \mathrm{O}(l) + \mathrm{Ba}^{2+}(aq) + 2\mathrm{Cl}^{-}(aq) + 2\mathrm{NH}_{3}(aq)\]
03

Cancel the Spectator Ions

Identify and cancel the spectator ions present on both sides of the equations.For reaction (a), cancel \(\mathrm{NO}_{3}^{-}\) and \(2\mathrm{Li}^{+}\). The net ionic equation becomes: \[\mathrm{H}^{+}(aq) + \mathrm{CO}_{3}^{2-}(aq) \rightleftharpoons \mathrm{HCO}_{3}^{-}(aq) \]
04

Write the Net Ionic Equation for (b)

In reaction (b), cancel \(\mathrm{Cl}^{-}\) and \(\mathrm{Ba}^{2+}\). The net ionic equation becomes: \[2\mathrm{NH}_{4}^{+}(aq) + 2\mathrm{OH}^{-}(aq) \rightleftharpoons 2\mathrm{H}_{2} \mathrm{O}(l) + 2\mathrm{NH}_{3}(aq)\]
05

Identify the Conjugate Acid-Base Pairs

In reaction (a), the conjugate acid-base pairs are \(\mathrm{H}^{+}\) (acid) and \(\mathrm{HCO}_{3}^{-}\) (conjugate base), and \(\mathrm{CO}_{3}^{2-}\) (base) and \(\mathrm{HCO}_{3}^{-}\) (conjugate acid). For reaction (b), the pairs are \(\mathrm{NH}_{4}^{+}\) (acid) and \(\mathrm{NH}_{3}\) (conjugate base), and \(\mathrm{OH}^{-}\) (base) and \(\mathrm{H}_{2} \mathrm{O}\) (conjugate acid).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Acid-Base Reactions
Understanding acid-base reactions is crucial for writing balanced ionic equations. In these reactions, acids donate protons (H鈦� ions) while bases accept protons. For example, in reaction (a), nitric acid (HNO鈧�) acts as an acid, and lithium carbonate (Li鈧侰O鈧�) acts as a base. During the reaction, the acid and base exchange ions to form new products. This exchange is key to predicting the outcome of many chemical reactions.
Conjugate Acid-Base Pairs
Conjugate acid-base pairs are fundamental to understanding the dynamics of acid-base reactions. When an acid donates a proton, it forms its conjugate base, and when a base accepts a proton, it forms its conjugate acid. For example, in reaction (a), H鈦� (the conjugate acid) and HCO鈧冣伝 (the conjugate base) are one pair, while CO鈧兟测伝 (the base) and HCO鈧冣伝 (the conjugate acid) are another. Identifying these pairs helps us understand how acids and bases transform during reactions.
Ionic Equations
Ionic equations break down compounds into their respective ions. This helps in clearly seeing which ions participate in reaction and which do not (spectator ions). For instance, in reaction (b), the complete ionic equation is:

2NH鈧勨伜(aq) + 2Cl鈦�(aq) + Ba虏鈦�(aq) + 2OH鈦�(aq) 鈬� 2H鈧侽(l) + Ba虏鈦�(aq) + 2Cl鈦�(aq) + 2NH鈧�(aq)

By canceling the spectator ions (Cl鈦� and Ba虏鈦�), we get the net ionic equation:
2NH鈧勨伜(aq) + 2OH鈦�(aq) 鈬� 2H鈧侽(l) + 2NH鈧�(aq).

This simplification helps in focusing on the actual chemical change occurring in the reaction.

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Most popular questions from this chapter

Identify the Lewis acid and Lewis base in each reaction: (a) \(\mathrm{Na}^{+}+6 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{Na}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{+}\) (b) \(\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}\) (c) \(\mathrm{F}^{-}+\mathrm{BF}_{3} \rightleftharpoons \mathrm{BF}_{4}^{-}\)

(a) What is the \(K_{\mathrm{b}}\) of the benzoate ion, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COO}^{-} ?\) (b) What is the \(K_{a}\) of the 2 -hydroxycthylammonium ion, \(\mathrm{HOCH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{3}^{+}\left(\mathrm{p} K_{\mathrm{b}}\right.\) of \(\left.\mathrm{HOCH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}=4.49\right) ?\)

What is an amphiprotic species? Name one and write balanced equations that show why it is amphiprotic.

Putrescine \(\left[\mathrm{NH}_{2}\left(\mathrm{CH}_{2}\right)_{4} \mathrm{NH}_{2}\right],\) found in rotting animal tissue, is now known to be in all cells and essential for normal and abnormal (cancerous) growth. It also plays a key role in the formation of GABA, a neurotransmitter. A \(0.10 M\) aqueous solution of putrescine has \(\left[\mathrm{OH}^{-}\right]=2.1 \times 10^{-3}\). What is the \(\bar{K}_{\mathrm{b}} ?\)

(a) What are \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right],\left[\mathrm{OH}^{-}\right],\) and \(\mathrm{pOH}\) in a solution with a \(\mathrm{pH}\) of \(4.77 ?\) (b) What are \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right],[\mathrm{OH}],\) and \(\mathrm{pH}\) in a solution with a pOH of \(5.65 ?\)
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