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Chapter 4: Problem 34

Write a balanced net ionic equation for each of the following acid-base reactions in water. (a) acetic acid \(\left(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)\) with strontium hydroxide (b) diethylamine, \(\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{NH}\), with sulfuric acid (c) aqueous hydrogen cyanide (HCN) with sodium hydroxide

Short Answer

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Question: Write the balanced net ionic equations for the following reactions: (a) Acetic acid (HC2H3O2) with strontium hydroxide (b) Diethylamine (C2H5)2NH with sulfuric acid (c) Aqueous hydrogen cyanide (HCN) with sodium hydroxide Answer: (a) HC2H3O2 (aq) + 2 OH- (aq) -> 2 CH3COO- (aq) + 2 H2O (l) (b) (C2H5)2NH (aq) + H2SO4 (aq) -> (C2H5)2NH2+ (aq) + HSO4- (aq) (c) HCN (aq) + OH- (aq) -> CN- (aq) + H2O (l)

Step by step solution

01

Write the balanced complete ionic equation

For the reaction between acetic acid and strontium hydroxide, first write the reactants and products. Acetic acid is a weak acid that will donate a proton to the hydroxide ion from the strong base strontium hydroxide, forming aqueous acetate ions and water. The complete balanced equation is: HC2H3O2 (aq) + Sr(OH)2 (aq) -> 2 CH3COO- (aq) + Sr2+ (aq) + 2 H2O (l)
02

Identify and remove spectator ions

The spectator ion in this reaction is the strontium cation, Sr2+. So, we remove this ion from both sides of the equation.
03

Write the balanced net ionic equation

After removing the spectator ion, the net ionic equation is: HC2H3O2 (aq) + 2 OH- (aq) -> 2 CH3COO- (aq) + 2 H2O (l) (b) Diethylamine (C2H5)2NH with sulfuric acid
04

Write the balanced complete ionic equation

Diethylamine, a weak base, will accept a proton from the strong acid sulfuric acid. This will form aqueous diethylammonium ions and hydrogen sulfate ions. The complete balanced equation is: (C2H5)2NH (aq) + H2SO4 (aq) -> (C2H5)2NH2+ (aq) + HSO4- (aq)
05

Identify and remove spectator ions

There are no spectator ions in this reaction since all components are involved in the reaction.
06

Write the balanced net ionic equation

The net ionic equation is the same as the complete ionic equation in this case: (C2H5)2NH (aq) + H2SO4 (aq) -> (C2H5)2NH2+ (aq) + HSO4- (aq) (c) Aqueous hydrogen cyanide (HCN) with sodium hydroxide
07

Write the balanced complete ionic equation

Aqueous hydrogen cyanide, a weak acid, will donate a proton to the hydroxide ion from the strong base sodium hydroxide, forming water and aqueous cyanide ions. The complete balanced equation is: HCN (aq) + NaOH (aq) -> NaCN (aq) + H2O (l)
08

Identify and remove spectator ions

The spectator ion in this reaction is the sodium cation, Na+. So, we remove this ion from both sides of the equation.
09

Write the balanced net ionic equation

After removing the spectator ion, the net ionic equation is: HCN (aq) + OH- (aq) -> CN- (aq) + H2O (l)

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Most popular questions from this chapter

Consider the following generic equation: $$ \mathrm{H}^{+}(a q)+\mathrm{B}^{-}(a q) \longrightarrow \mathrm{HB}(a q) $$ For which of the following pairs would this be the correct prototype equation for the acid-base reaction in solution? If it is not correct, write the proper equation for the acid-base reaction between the pair. (a) nitric acid and calcium hydroxide (b) hydrochloric acid and \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) (c) hydrobromic acid and aqueous ammonia (d) perchloric acid and barium hydroxide (e) sodium hydroxide and nitrous acid

Solid iron(III) hydroxide is added to \(625 \mathrm{~mL}\) of \(0.280 \mathrm{M} \mathrm{HCl}\). The resulting solution is acidic and titrated with \(238.2 \mathrm{~mL}\) of \(0.113 \mathrm{M} \mathrm{NaOH}\). What mass of iron(III) hydroxide was added to the HCl?

Itwenty-five \(\mathrm{mL}\) of a \(0.388 \mathrm{M}\) solution of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) is mixed with \(35.3 \mathrm{~mL}\) of \(0.229 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}\). What is the molarity of the resulting solution? Assume that the volumes are additive.

Write net ionic equations to explain the formation of (a) a white precipitate when solutions of calcium sulfate and sodium carbonate are mixed. (b) two different precipitates formed when solutions of iron(III) sulfate and barium hydroxide are mixed.

When solutions of aluminum sulfate and sodium hydroxide are mixed, a white gelatinous precipitate forms. (a) Write a balanced net ionic equation for the reaction. (b) What is the mass of the precipitate when \(2.76 \mathrm{~g}\) of aluminum sulfate in \(125 \mathrm{~mL}\) of solution is combined with \(85.0 \mathrm{~mL}\) of \(0.2500 \mathrm{M} \mathrm{NaOH}\) ? (c) What is the molarity of the ion in excess? (Ignore spectator ions and assume that volumes are additive.)
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