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Chapter 4: Problem 65

Write the balanced formula, complete ionic, and net ionic equations for each of the following acid-base reactions. a. \(\mathrm{HClO}_{4}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(s) \rightarrow\) b. \(\mathrm{HCN}(a q)+\mathrm{NaOH}(a q) \rightarrow\) c. \(\mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \rightarrow\)

Short Answer

Expert verified
a. Balanced Formula Equation: \(2\mathrm{HClO}_{4}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(s) \rightarrow \mathrm{Mg(ClO}_{4})_{2}(a q)+2\mathrm{H}_{2}\mathrm{O}(l)\) Complete Ionic Equation: \(2\mathrm{H^+}(a q)+2\mathrm{ClO}_{4}^-(a q)+\mathrm{Mg^{2+}}(a q)+2\mathrm{OH^-}(a q) \rightarrow \mathrm{Mg^{2+}}(a q)+2\mathrm{ClO}_{4}^-(a q)+2\mathrm{H}_{2}\mathrm{O}(l)\) Net Ionic Equation: \(2\mathrm{H^+}(a q)+2\mathrm{OH^-}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l)\) b. Balanced Formula Equation: \(\mathrm{HCN}(a q)+\mathrm{NaOH}(a q) \rightarrow \mathrm{NaCN}(a q)+\mathrm{H}_{2}\mathrm{O}(l)\) Complete Ionic Equation: \(\mathrm{HCN}(a q)+\mathrm{Na^+}(a q)+\mathrm{OH^-}(a q) \rightarrow \mathrm{Na^+}(a q)+\mathrm{CN^-}(a q)+\mathrm{H}_{2}\mathrm{O}(l)\) Net Ionic Equation: \(\mathrm{HCN}(a q)+\mathrm{OH^-}(a q) \rightarrow \mathrm{CN^-}(a q)+\mathrm{H}_{2}\mathrm{O}(l)\) c. Balanced Formula Equation: \(\mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \rightarrow \mathrm{NaCl}(a q)+\mathrm{H}_{2}\mathrm{O}(l)\) Complete Ionic Equation: \(\mathrm{H^+}(a q)+\mathrm{Cl^-}(a q)+\mathrm{Na^+}(a q)+\mathrm{OH^-}(a q) \rightarrow \mathrm{Na^+}(a q)+\mathrm{Cl^-}(a q)+\mathrm{H}_{2}\mathrm{O}(l)\) Net Ionic Equation: \(\mathrm{H^+}(a q)+\mathrm{OH^-}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l)\)

Step by step solution

01

Write the balanced formula equation

Combine the given reactants to form a salt and water. The salt formed will be \(\mathrm{Mg(ClO}_{4})_{2}\) and the product will be water. Balance the equation: \[2\mathrm{HClO}_{4}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(s) \rightarrow \mathrm{Mg(ClO}_{4})_{2}(a q)+2\mathrm{H}_{2}\mathrm{O}(l)\]
02

Write the complete ionic equation

Break strong electrolytes: \[2\mathrm{H^+}(a q)+2\mathrm{ClO}_{4}^-(a q)+\mathrm{Mg^{2+}}(a q)+2\mathrm{OH^-}(a q) \rightarrow \mathrm{Mg^{2+}}(a q)+2\mathrm{ClO}_{4}^-(a q)+2\mathrm{H}_{2}\mathrm{O}(l)\]
03

Write the net ionic equation

Cancel spectator ions and simplify: \[2\mathrm{H^+}(a q)+2\mathrm{OH^-}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l)\] b. \(\mathrm{HCN}(a q)+\mathrm{NaOH}(a q) \rightarrow\)
04

Write the balanced formula equation

Combine the given reactants to form a salt and water. The salt formed will be \(\mathrm{NaCN}\) and the product will be water. Balance the equation: \[\mathrm{HCN}(a q)+\mathrm{NaOH}(a q) \rightarrow \mathrm{NaCN}(a q)+\mathrm{H}_{2}\mathrm{O}(l)\]
05

Write the complete ionic equation

HCN is a weak acid and does not dissociate completely. So, we won't break it down into ions. Break down NaOH because it is a strong electrolyte: \[\mathrm{HCN}(a q)+\mathrm{Na^+}(a q)+\mathrm{OH^-}(a q) \rightarrow \mathrm{Na^+}(a q)+\mathrm{CN^-}(a q)+\mathrm{H}_{2}\mathrm{O}(l)\]
06

Write the net ionic equation

Cancel spectator ions and simplify: \[\mathrm{HCN}(a q)+\mathrm{OH^-}(a q) \rightarrow \mathrm{CN^-}(a q)+\mathrm{H}_{2}\mathrm{O}(l)\] c. \(\mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \rightarrow\)
07

Write the balanced formula equation

Combine the given reactants to form a salt and water. The salt formed will be \(\mathrm{NaCl}\) and the product will be water. Balance the equation: \[\mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \rightarrow \mathrm{NaCl}(a q)+\mathrm{H}_{2}\mathrm{O}(l)\]
08

Write the complete ionic equation

Break down HCl and NaOH into their ions because they are both strong electrolytes: \[\mathrm{H^+}(a q)+\mathrm{Cl^-}(a q)+\mathrm{Na^+}(a q)+\mathrm{OH^-}(a q) \rightarrow \mathrm{Na^+}(a q)+\mathrm{Cl^-}(a q)+\mathrm{H}_{2}\mathrm{O}(l)\]
09

Write the net ionic equation

Cancel spectator ions and simplify: \[\mathrm{H^+}(a q)+\mathrm{OH^-}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l)\]

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Most popular questions from this chapter

Specify which of the following are oxidation-reduction reactions, and identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. a. \(\mathrm{Cu}(s)+2 \mathrm{Ag}^{+}(a q) \rightarrow 2 \mathrm{Ag}(s)+\mathrm{Cu}^{2+}(a q)\) b. \(\mathrm{HCl}(g)+\mathrm{NH}_{3}(\mathrm{~g}) \rightarrow \mathrm{NH}_{4} \mathrm{Cl}(s)\) c. \(\mathrm{SiCl}_{4}(l)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow 4 \mathrm{HCl}(a q)+\mathrm{SiO}_{2}(s)\) d. \(\mathrm{SiCl}_{4}(l)+2 \mathrm{Mg}(s) \rightarrow 2 \mathrm{MgCl}_{2}(s)+\operatorname{Si}(s)\) e. \(\mathrm{Al}(\mathrm{OH})_{4}^{-}(a q) \rightarrow \mathrm{AlO}_{2}^{-}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)\)

A 230.-mL sample of a \(0.275 \mathrm{M} \mathrm{CaCl}_{2}\) solution is left on a hot plate overnight; the following morning, the solution is \(1.10 \mathrm{M}\). What volume of water evaporated from the \(0.275 \mathrm{M} \mathrm{CaCl}_{2}\) solution?

Zinc and magnesium metal each react with hydrochloric acid according to the following equations: $$ \begin{array}{l} \mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g) \\ \mathrm{Mg}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{H}_{2}(g) \end{array} $$ A \(10.00-\mathrm{g}\) mixture of zinc and magnesium is reacted with the stoichiometric amount of hydrochloric acid. The reaction mixture is then reacted with \(156 \mathrm{~mL}\) of \(3.00 M\) silver nitrate to produce the maximum possible amount of silver chloride. a. Determine the percent magnesium by mass in the original mixture. b. If \(78.0 \mathrm{~mL}\) of \(\mathrm{HCl}\) was added, what was the concentration of the \(\mathrm{HCl}\) ?

Calculate the molarity of each of these solutions. a. A \(5.623-\mathrm{g}\) sample of \(\mathrm{NaHCO}_{3}\) is dissolved in enough water to make \(250.0 \mathrm{~mL}\) of solution. b. A \(184.6-\mathrm{mg}\) sample of \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) is dissolved in enough water to make \(500.0 \mathrm{~mL}\) of solution. c. A 0.1025-g sample of copper metal is dissolved in \(35 \mathrm{~mL}\) of concentrated \(\mathrm{HNO}_{3}\) to form \(\mathrm{Cu}^{2+}\) ions and then water is added to make a total volume of \(200.0 \mathrm{~mL}\). (Calculate the molarity of \(\mathrm{Cu}^{2+} .\) )

Show how each of the following strong electrolytes "breaks up" into its component ions upon dissolving in water by drawing molecular-level pictures. a. \(\mathrm{NaBr}\) f. \(\mathrm{FeSO}_{4}\) b. \(\mathrm{MgCl}_{2}\) g. \(\mathrm{KMnO}_{4}\) c. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) h. \(\mathrm{HClO}_{4}\) d. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) i. \(\mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) (ammonium acetate) e. \(\mathrm{NaOH}\)
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