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Chapter 4: Problem 34

Balance the following equations and write the corresponding ionic and net ionic equations (if appropriate). (a) \(\mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{KOH}(a q) \longrightarrow\) (b) \(\mathrm{H}_{2} \mathrm{CO}_{3}(a q)+\mathrm{NaOH}(a q) \longrightarrow\) (c) \(\mathrm{HNO}_{3}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \longrightarrow\)

Short Answer

Expert verified
The balanced chemical equations are: (a) \(CH_{3}COOH_{(aq)} + KOH_{(aq)} \rightarrow KCH_{3}COO_{(aq)} + H_{2}O_{(l)}\) (b) \(H_{2}CO_{3}_{(aq)} + 2NaOH_{(aq)} \rightarrow Na_{2}CO_{3}_{(aq)} + 2H_{2}O_{(l)}\)(c) \(2HNO_{3}_{(aq)} + Ba(OH)_{2}_{(aq)} \rightarrow Ba(NO_{3})_{2}_{(aq)} + 2H_{2}O_{(l)}\). And the net ionic equations are: (a) \(CH_{3}COOH_{(aq)} + OH^-_{(aq)} \rightarrow CH_{3}COO^-_{(aq)} + H_{2}O_{(l)}\) (b) \(2H^{+}_{(aq)} + 2OH^-_{(aq)} \rightarrow 2H_{2}O_{(l)}\)(c) \(2H^{+}_{(aq)} + 2OH^-_{(aq)} \rightarrow 2H_{2}O_{(l)}\)

Step by step solution

01

Balance the equations and identify the products

First, identify the products of each reaction, which will always be water and a salt. Then balance the equations. (a) \(CH_{3}COOH_{(aq)} + KOH_{(aq)} \rightarrow KCH_{3}COO_{(aq)} + H_{2}O_{(l)}\) (b) \(H_{2}CO_{3}_{(aq)} + 2NaOH_{(aq)} \rightarrow Na_{2}CO_{3}_{(aq)} + 2H_{2}O_{(l)}\)(c) \(2HNO_{3}_{(aq)} + Ba(OH)_{2}_{(aq)} \rightarrow Ba(NO_{3})_{2}_{(aq)} + 2H_{2}O_{(l)}\)
02

Write the ionic equations

In an ionic equation, we break all the strong electrolytes into their individual ions.(a) \(CH_{3}COOH_{(aq)} + K^{+}_{(aq)} + OH^-_{(aq)} \rightarrow CH_{3}COO^-_{(aq)} + K^{+}_{(aq)} + H_{2}O_{(l)}\) (b) \(2H^{+}_{(aq)}+ CO_{3}^{2-}_{(aq)} + 2Na^{+}_{(aq)} + 2OH^-_{(aq)} \rightarrow 2Na^{+}_{(aq)}+ CO_{3}^{2-}_{(aq)} + 2H_{2}O_{(l)}\) (c) \(2H^{+}_{(aq)} + 2NO_{3}^-_{(aq)} + Ba^{2+}_{(aq)} + 2OH^-_{(aq)} \rightarrow Ba^{2+}_{(aq)} + 2NO_{3}^-_{(aq)} + 2H_{2}O_{(l)}\)
03

Write the net ionic equations

Finally, simplify to the net ionic equations by canceling out the species that appear on both sides of the equation (spectator ions)(a) \(CH_{3}COOH_{(aq)} + OH^-_{(aq)} \rightarrow CH_{3}COO^-_{(aq)} + H_{2}O_{(l)}\) (b) \(2H^{+}_{(aq)} + 2OH^-_{(aq)} \rightarrow 2H_{2}O_{(l)}\)(c) \(2H^{+}_{(aq)} + 2OH^-_{(aq)} \rightarrow 2H_{2}O_{(l)}\)

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Most popular questions from this chapter

Hydrogen halides (HF, HCl, HBr, HI) are highly reactive compounds that have many industrial and laboratory uses. (a) In the laboratory, HF and \(\mathrm{HCl}\) can be generated by reacting \(\mathrm{CaF}_{2}\) and \(\mathrm{NaCl}\) with concentrated sulfuric acid. Write appropriate equations for the reactions. (Hint: These are not redox reactions.) (b) Why is it that HBr and HI cannot be prepared similarly-that is, by reacting NaBr and NaI with concentrated sulfuric acid? (Hint: \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a stronger oxidizing agent than both \(\mathrm{Br}_{2}\) and \(\mathrm{I}_{2} .\) ) (c) HBr can be prepared by reacting phosphorus tribromide \(\left(\mathrm{PBr}_{3}\right)\) with water. Write an equation for this reaction.

You are given two colorless solutions, one containing \(\mathrm{NaCl}\) and the other sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right) .\) Suggest a chemical and a physical test that would allow you to distinguish between these two solutions.

A \(35.2-\mathrm{mL}, 1.66 M \mathrm{KMnO}_{4}\) solution is mixed with \(16.7 \mathrm{~mL}\) of \(0.892 \mathrm{M} \mathrm{KMnO}_{4}\) solution. Calculate the concentration of the final solution.

Oxygen \(\left(\mathrm{O}_{2}\right)\) and carbon dioxide \(\left(\mathrm{CO}_{2}\right)\) are colorless and odorless gases. Suggest two chemical tests that would enable you to distinguish between these two gases.

How many grams of \(\mathrm{KOH}\) are present in \(35.0 \mathrm{~mL}\) of a \(5.50 M\) solution?
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