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Chapter 4: Problem 72

Write the balanced formula, complete ionic, and net ionic equations for each of the following acid–base reactions. a. \(\mathrm{HNO}_{3}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow\) b. $\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{KOH}(a q) \rightarrow$ c. \(\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{HCl}(a q) \rightarrow\)

Short Answer

Expert verified
a. Balanced formula equation: \[3\mathrm{HNO}_{3}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow \mathrm{Al(NO}_{3})_{3}(a q) + 3\mathrm{H}_{2}\mathrm{O}(l)\] Net ionic equation: \[3\mathrm{H^{+}}(a q) + 3\mathrm{OH}^{-}(a q) \rightarrow 3\mathrm{H}_{2}\mathrm{O}(l)\] b. Balanced formula equation: \[\mathrm{HC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}(a q)+\mathrm{KOH}(a q)\rightarrow\mathrm{KC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}(a q)+\mathrm{H}_{2}\mathrm{O}(l)\] Net ionic equation: \[\mathrm{H^{+}}(a q) + \mathrm{OH}^{-}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l)\] c. Balanced formula equation: \[\mathrm{Ca}(\mathrm{OH})_{2}(a q)+2\mathrm{HCl}(a q) \rightarrow \mathrm{CaCl}_{2}(a q) + 2\mathrm{H}_{2}\mathrm{O}(l)\] Net ionic equation: \[2\mathrm{H^{+}}(a q) + 2\mathrm{OH}^{-}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l)\]

Step by step solution

01

In this reaction, \(\mathrm{HNO}_{3}\) is the acid and \(\mathrm{Al(OH)}_{3}\) is the base. When they react, they will form a salt (aluminium nitrate) and water. #Step 2: Write the balanced formula equation#

The balanced formula equation for this reaction is: \[3\mathrm{HNO}_{3}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow \mathrm{Al(NO}_{3})_{3}(a q) + 3\mathrm{H}_{2}\mathrm{O}(l)\] #Step 3: Write the complete ionic equation#
02

The complete ionic equation for this reaction is: \[3\mathrm{H^{+}}(a q) + 3\mathrm{NO}_{3}^{-}(a q) + \mathrm{Al^{3+}}(a q) + 3\mathrm{OH}^{-}(a q) \rightarrow \mathrm{Al^{3+}}(a q) + 3\mathrm{NO}_{3}^{-}(a q) + 3\mathrm{H}_{2}\mathrm{O}(l)\] #Step 4: Write the net ionic equation#

The net ionic equation for this reaction is: \[3\mathrm{H^{+}}(a q) + 3\mathrm{OH}^{-}(a q) \rightarrow 3\mathrm{H}_{2}\mathrm{O}(l)\] # For Reaction (b) # #Step 1: Identify reactants and products#
03

In this reaction, \(\mathrm{HC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}\) (acetic acid) is the acid and \(\mathrm{KOH}\) is the base. When they react, they will form a salt (potassium acetate) and water. #Step 2: Write the balanced formula equation#

The balanced formula equation for this reaction is: \[\mathrm{HC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}(a q)+\mathrm{KOH}(a q)\rightarrow\mathrm{KC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}(a q)+\mathrm{H}_{2}\mathrm{O}(l)\] #Step 3: Write the complete ionic equation#
04

The complete ionic equation for this reaction is: \[\mathrm{H^{+}}(a q) + \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}(a q) + \mathrm{K}^{+}(a q) + \mathrm{OH}^{-}(a q) \rightarrow \mathrm{K}^{+}(a q) + \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-}(a q) + \mathrm{H}_{2}\mathrm{O}(l)\] #Step 4: Write the net ionic equation#

The net ionic equation for this reaction is: \[\mathrm{H^{+}}(a q) + \mathrm{OH}^{-}(a q) \rightarrow \mathrm{H}_{2}\mathrm{O}(l)\] # For Reaction (c) # #Step 1: Identify reactants and products#
05

In this reaction, \(\mathrm{Ca(OH)}_{2}\) is the base and \(\mathrm{HCl}\) is the acid. When they react, they will form a salt (calcium chloride) and water. #Step 2: Write the balanced formula equation#

The balanced formula equation for this reaction is: \[\mathrm{Ca}(\mathrm{OH})_{2}(a q)+2\mathrm{HCl}(a q) \rightarrow \mathrm{CaCl}_{2}(a q) + 2\mathrm{H}_{2}\mathrm{O}(l)\] #Step 3: Write the complete ionic equation#
06

The complete ionic equation for this reaction is: \[\mathrm{Ca^{2+}}(a q) + 2\mathrm{OH}^{-}(a q) + 2\mathrm{H^{+}}(a q) + 2\mathrm{Cl}^{-}(a q) \rightarrow \mathrm{Ca^{2+}}(a q) + 2\mathrm{Cl}^{-}(a q) + 2\mathrm{H}_{2}\mathrm{O}(l)\] #Step 4: Write the net ionic equation#

The net ionic equation for this reaction is: \[2\mathrm{H^{+}}(a q) + 2\mathrm{OH}^{-}(a q) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l)\]

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Most popular questions from this chapter

Chlorine gas was first prepared in 1774 by C. W. Scheele by oxidizing sodium chloride with manganese(IV) oxide. The reaction is $$\mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{MnO}_{2}(s) \longrightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{MnCl}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Cl}_{2}(g)$$ Balance this equation.

A 6.50-g sample of a diprotic acid requires 137.5 mL of a 0.750 M NaOH solution for complete neutralization. Determine the molar mass of the acid.

Calculate the concentration of all ions present when 0.160 \(\mathrm{g}\) of \(\mathrm{MgCl}_{2}\) is dissolved in 100.0 \(\mathrm{mL}\) of solution.

Assign oxidation numbers to all the atoms in each of the following. a. \(\mathrm{SrCr}_{2} \mathrm{O}_{7} \quad\) g. \(\mathrm{PbSO}_{3}\) b. \(\mathrm{CuCl}_{2} \quad \quad\) h. \(\mathrm{PbO}_{2}\) c. \(\mathrm{O}_{2} \quad\quad\quad\) i. $\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}$ d. \(\mathrm{H}_{2} \mathrm{O}_{2} \quad\quad \mathrm{j} . \mathrm{CO}_{2}\) e. \(\mathrm{MgCO}_{3} \quad\) k. $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Ce}\left(\mathrm{SO}_{4}\right)_{3}$ f. \(\mathrm{Ag} \quad\quad\quad \)l. \(\mathrm{Cr}_{2} \mathrm{O}_{3}\)

Assign oxidation states for all atoms in each of the following compounds a. \({KMnO}_{4} \quad\quad\quad f. {Fe}_{3} {O}_{4}\) b. \({NiO}_{2} \quad\quad\quad\quad g. {XeOF}_{4}\) c. \({Na}_{4} {Fe}({OH})_{6} \quad h. {SF}_{4}\) d. \({NH}_{4} {h}_{2} {HPO}_{4} \quad i. {CO}\) e. \({P}_{4} {O}_{6} \quad\quad\quad\quad\quad j. {C}_{6} {H}_{12} {O}_{6}\)
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