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Chapter 4: Problem 40

Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (a) Aqueous acetic acid is neutralized by aqueous barium hydroxide. (b) Solid chromium(III) hydroxide reacts with nitrous acid. (c) Aqueous nitric acid and aqueous ammonia react.

Short Answer

Expert verified
(a) Balanced molecular equation: \(HC_{2}H_{3}O_{2}(aq) + Ba(OH)_{2}(aq) \rightarrow H_{2}O(l) + Ba(C_{2}H_{3}O_{2})_{2}(aq) \) Balanced net ionic equation: \(H^{+}(aq) + OH^{-}(aq) \rightarrow H_{2}O(l)\) (b) Balanced molecular equation: \(Cr(OH)_{3}(s) + 3HNO_{2}(aq) \rightarrow 3H_{2}O(l) + Cr(NO_{2})_{3}(aq) \) Balanced net ionic equation: \(Cr(OH)_{3}(s) + 3H^{+}(aq) \rightarrow 3H_{2}O(l) + Cr^{3+}(aq)\) (c) Balanced molecular equation: \(HNO_{3}(aq) + NH_{3}(aq) \rightarrow H_{2}O(l) + NH_{4}NO_{3}(aq) \) Balanced net ionic equation: \(H^{+}(aq) + NH_{3}(aq) \rightarrow H_{2}O(l) + NH_{4}^{+}(aq)\)

Step by step solution

01

Identify reactants and predict products

The reactants are aqueous acetic acid (HC鈧侶鈧僌鈧�) and aqueous barium hydroxide (Ba(OH)鈧�). Since it's a neutralization reaction, the products will be water (H鈧侽) and a salt, in this case, barium acetate (Ba(C鈧侶鈧僌鈧�)鈧�).
02

Write the balanced molecular equation

Balance the equation by making sure the number of atoms of each element is equal on both sides: \(HC_{2}H_{3}O_{2}(aq) + Ba(OH)_{2}(aq) \rightarrow H_{2}O(l) + Ba(C_{2}H_{3}O_{2})_{2}(aq) \)
03

Write the balanced net ionic equation

Remove the spectator ions in the balanced molecular equation to get the balanced net ionic equation: \(H^{+}(aq) + C_{2}H_{3}O_{2}^{-}(aq) + OH^{-}(aq) \rightarrow H_{2}O(l) + C_{2}H_{3}O_{2}^{-}(aq)\) (b):
04

Identify reactants and predict products

The reactants are solid chromium(III) hydroxide (Cr(OH)鈧�) and nitrous acid (HNO鈧�). The products will be water (H鈧侽) and a salt, which is chromium(III) nitrite (Cr(NO鈧�)鈧�).
05

Write the balanced molecular equation

Balance the equation by making sure the number of atoms of each element is equal on both sides: \(Cr(OH)_{3}(s) + 3HNO_{2}(aq) \rightarrow 3H_{2}O(l) + Cr(NO_{2})_{3}(aq) \)
06

Write the balanced net ionic equation

Remove the spectator ions in the balanced molecular equation to get the balanced net ionic equation: \(Cr(OH)_{3}(s) + 3H^{+}(aq) + 3NO_{2}^{-}(aq) \rightarrow 3H_{2}O(l) + Cr^{3+}(aq) + 3NO_{2}^{-}(aq)\) (c):
07

Identify reactants and predict products

The reactants are aqueous nitric acid (HNO鈧�) and aqueous ammonia (NH鈧�). The products will be water (H鈧侽) and a salt, which is ammonium nitrate (NH鈧凬O鈧�).
08

Write the balanced molecular equation

Balance the equation by making sure the number of atoms of each element is equal on both sides: \(HNO_{3}(aq) + NH_{3}(aq) \rightarrow H_{2}O(l) + NH_{4}NO_{3}(aq) \)
09

Write the balanced net ionic equation

Remove the spectator ions in the balanced molecular equation to get the balanced net ionic equation: \(H^{+}(aq) + NO_{3}^{-}(aq) + NH_{3}(aq) \rightarrow H_{2}O(l) + NH_{4}^{+}(aq) + NO_{3}^{-}(aq)\)

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Most popular questions from this chapter

Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (a) HF, (b) acetonitrile, \(\mathrm{CH}_{3} \mathrm{CN}\), (c) \(\mathrm{NaClO}_{4}\), (d) \(\mathrm{Ba}(\mathrm{OH})_{2}\).

Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. (a) \(\mathrm{NaCH}_{3} \mathrm{COO}\) and \(\mathrm{HCl}\), (b) \(\mathrm{KOH}\) and \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\), (c) \(\mathrm{Na}_{2} \mathrm{~S}\) and \(\mathrm{CdSO}_{4}\).

An 8.65-g sample of an unknown group \(2 \mathrm{~A}\) metal hydroxide is dissolved in \(85.0 \mathrm{~mL}\) of water. An acid-base indicator is added and the resulting solution is titrated with \(2.50 \mathrm{M}\) \(\mathrm{HCl}(a q)\) solution. The indicator changes color signaling that the equivalence point has been reached after \(56.9 \mathrm{~mL}\) of the hydrochloric acid solution has been added. (a) What is the molar mass of the metal hydroxide? (b) What is the identity of the metal cation: \(\mathrm{Ca}^{2+}, \mathrm{Sr}^{2+}, \mathrm{Ba}^{2+}\) ?

The commercial production of nitric acid involves the following chemical reactions: $$ \begin{aligned} 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) & \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) \\ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) & \longrightarrow 2 \mathrm{NO}_{2}(g) \\ 3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) & \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g) \end{aligned} $$ (a) Which of these reactions are redox reactions? (b) In each redox reaction identify the element undergoing oxidation and the element undergoing reduction. (c) How many grams of ammonia must you start with to make \(1000.0 \mathrm{~L}\) of a \(0.150 \mathrm{M}\) aqueous solution of nitric acid? Assume all the reactions give \(100 \%\) yield.

Formic acid, HCOOH, is a weak electrolyte. What solutes are present in an aqueous solution of this compound? Write the chemical equation for the ionization of HCOOH.
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