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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) How many milliliters of a stock solution of \(6.0 \mathrm{M} \mathrm{HNO}_{3}\) would you have to use to prepare \(110 \mathrm{~mL}\) of \(0.500 \mathrm{M} \mathrm{HNO}_{3} ?\) (b) If you dilute \(10.0 \mathrm{~mL}\) of the stock solution to a final volume of \(0.250 \mathrm{~L}\), what will be the concentration of the diluted solution?

Lanthanum metal forms cations with a charge of \(3+.\) Consider the following observations about the chemistry of lanthanum: When lanthanum metal is exposed to air, a white solid (compound \(\mathrm{A}\) ) is formed that contains lanthanum and one other element. When lanthanum metal is added to water, gas bubbles are observed and a different white solid (compound \(\mathrm{B}\) ) is formed. Both \(\mathrm{A}\) and \(\mathrm{B}\) dissolve in hydrochloric acid to give a clear solution. When either of these solutions is evaporated, a soluble white solid (compound C) remains. If compound \(\mathrm{C}\) is dissolved in water and sulfuric acid is added, a white precipitate (compound D) forms. (a) Propose identities for the substances \(\mathrm{A}, \mathrm{B}, \mathrm{C},\) and \(\mathrm{D} .(\mathbf{b})\) Write net ionic equations for all the reactions described. (c) Based on the preceding observations, what can be said about the position of lanthanum in the activity series (Table 4.5\() ?\)

(a) How many grams of solute are present in \(15.0 \mathrm{~mL}\) of \(0.736 \mathrm{M} \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7} ?\) (b) If \(14.00 \mathrm{~g}\) of \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) is dissolved in enough water to form \(250 \mathrm{~mL}\) of solution, what is the molarity of the solution? (c) How many milliliters of \(0.0455 \mathrm{M} \mathrm{CuSO}_{4}\) contain \(3.65 \mathrm{~g}\) of solute?

Suppose you have \(5.00 \mathrm{~g}\) of powdered magnesium metal, \(1.00 \mathrm{~L}\) of \(2.00 \mathrm{M}\) potassium nitrate solution, and \(1.00 \mathrm{~L}\) of \(2.00 \mathrm{M}\) silver nitrate solution. (a) Which one of the solutions will react with the magnesium powder? (b) What is the net ionic equation that describes this reaction? (c) What volume of solution is needed to completely react with the magnesium? (d) What is the molarity of the \(\mathrm{Mg}^{2+}\) ions in the resulting solution?

Classify each of the following aqueous solutions as a nonelectrolyte, weak electrolyte, or strong electrolyte: (a) \(\mathrm{LiClO}_{4}\), (b) \(\mathrm{HClO}\) (c) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}\) (propanol), (d) \(\mathrm{HClO}_{3}\), (e) \(\mathrm{CuSO}_{4}\), (f) \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) (sucrose).
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