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Chapter 4: Problem 39

Complete and balance the following molecular equations, and then write the net ionic equation for each: (a) \(\mathrm{HBr}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow\) (b) \(\mathrm{Cu}(\mathrm{OH})_{2}(s)+\mathrm{HClO}_{4}(a q) \longrightarrow\) (c) \(\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{HNO}_{3}(a q) \longrightarrow\)

Short Answer

Expert verified
The net ionic equations for the given reactions are: (a) \(2\mathrm{H^{+}}(aq) + 2\mathrm{OH^{-}}(aq) \longrightarrow 2\mathrm{H_{2}O}(l)\) (b) \(\mathrm{Cu(OH)_{2}}(s) + 2\mathrm{H^{+}}(aq) \longrightarrow \mathrm{Cu^{2+}}(aq) + 2\mathrm{H_{2}O}(l)\) (c) \(\mathrm{Al(OH)_{3}}(s) + 3\mathrm{H^{+}}(aq) \longrightarrow \mathrm{Al^{3+}}(aq) + 3\mathrm{H_{2}O}(l)\)

Step by step solution

01

Reaction (a) - Write unbalanced molecular equation

The given unbalanced equation is: HBr(aq) + Ca(OH)2(aq) ->
02

Reaction (a) - Balance the equation

Let's balance the equation. We have \(2 \mathrm{HBr} (a q) + \mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow \mathrm{CaBr}_{2} (\mathrm{sq}) + 2\mathrm{H}_{2}\mathrm{O}(\ell)\)
03

Reaction (a) - Complete ionic equation

Now write the complete ionic equation: \(2\mathrm{H^{+}}(aq) + 2\mathrm{Br^{-}}(aq) + \mathrm{Ca^{2+}}(aq) + 2\mathrm{OH^{-}}(aq) \longrightarrow \mathrm{Ca^{2+}}(aq) + 2\mathrm{Br^{-}}(aq) + 2\mathrm{H_{2}O}(l)\)
04

Reaction (a) - Net ionic equation

Finally, the net ionic equation is: \(2\mathrm{H^{+}}(aq) + 2\mathrm{OH^{-}}(aq) \longrightarrow 2\mathrm{H_{2}O}(l)\) For Reaction (b):
05

Reaction (b) - Write unbalanced molecular equation

The given unbalanced equation is: Cu(OH)2(s) + HClO4(aq) ->
06

Reaction (b) - Balance the equation

Let's balance the equation. We have \( \mathrm{Cu}(\mathrm{OH})_{2}(s) + 2\mathrm{HClO}_4(\mathrm{aq}) \longrightarrow \mathrm{Cu}(\mathrm{ClO}_{4})_{2}(\mathrm{sq}) + 2\mathrm{H}_{2}\mathrm{O}(\ell)\)
07

Reaction (b) - Complete ionic equation

Now write the complete ionic equation: \(\mathrm{Cu(OH)_{2}}(s) + 2\mathrm{H^{+}}(aq) + 2\mathrm{ClO}_{4}^-(aq) \longrightarrow \mathrm{Cu^{2+}}(aq) + 2\mathrm{ClO}_{4}^-(aq) + 2\mathrm{H_{2}O}(l)\)
08

Reaction (b) - Net ionic equation

Finally, the net ionic equation is: \(\mathrm{Cu(OH)_{2}}(s) + 2\mathrm{H^{+}}(aq) \longrightarrow \mathrm{Cu^{2+}}(aq) + 2\mathrm{H_{2}O}(l)\) For Reaction (c):
09

Reaction (c) - Write unbalanced molecular equation

The given unbalanced equation is: Al(OH)3(s) + HNO3(aq) ->
10

Reaction (c) - Balance the equation

Let's balance the equation. We have \(\mathrm{Al}(\mathrm{OH})_{3}(s) + 3\mathrm{HNO}_3(\mathrm{aq}) \longrightarrow \mathrm{Al}(\mathrm{NO}_{3})_{3}(\mathrm{sq}) + 3\mathrm{H}_{2}\mathrm{O}(\ell)\)
11

Reaction (c) - Complete ionic equation

Now write the complete ionic equation: \(\mathrm{Al(OH)_{3}}(s) + 3\mathrm{H^{+}}(aq) + 3\mathrm{NO}_{3}^-(aq) \longrightarrow \mathrm{Al^{3+}}(aq) + 3\mathrm{NO}_{3}^-(aq) + 3\mathrm{H_{2}O}(l)\)
12

Reaction (c) - Net ionic equation

Finally, the net ionic equation is: \(\mathrm{Al(OH)_{3}}(s) + 3\mathrm{H^{+}}(aq) \longrightarrow \mathrm{Al^{3+}}(aq) + 3\mathrm{H_{2}O}(l)\)

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Most popular questions from this chapter

A solid sample of \(\mathrm{Zn}(\mathrm{OH})_{2}\) is added to \(0.350 \mathrm{~L}\) of \(0.500 \mathrm{M}\) aqueous HBr. The solution that remains is still acidic. It is then titrated with \(0.500 \mathrm{M} \mathrm{NaOH}\) solution, and it takes \(88.5 \mathrm{~mL}\) of the \(\mathrm{NaOH}\) solution to reach the equivalence point. What mass of \(\mathrm{Zn}(\mathrm{OH})_{2}\) was added to the HBr solution?

We have seen that ions in aqueous solution are stabilized by the attractions between the ions and the water molecules. Why then do some pairs of ions in solution form precipitates? \([\) Section 4.2\(]\)

You know that an unlabeled bottle contains a solution of one of the following: \(\mathrm{AgNO}_{3}, \mathrm{CaCl}_{2}\), or \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} .\) A friend suggests that you test a portion of the solution with \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\) and then with \(\mathrm{NaCl}\) solutions. Explain how these two tests together would be sufficient to determine which salt is present in the solution.

Specify what ions are present upon dissolving each of the following substances in water: (a) \(\mathrm{MgI}_{2}\), (b) \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3},\) (c) \(\mathrm{HClO}_{4}\), (d) \(\mathrm{NaCH}_{3} \mathrm{COO}\)

The distinctive odor of vinegar is due to acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH},\) which reacts with sodium hydroxide in the following fashion: $$\mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{NaOH}(a q) \longrightarrow$$ If \(3.45 \mathrm{~mL}\) of vinegar needs \(42.5 \mathrm{~mL}\) of \(0.115 \mathrm{M} \mathrm{NaOH}\) to reach the equivalence point in a titration, how many grams of acetic acid are in a \(1.00-\) qt sample of this vinegar?
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