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Chapter 4: Problem 95

Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the HCl(aq) in the stomach and each of the following substances used in various antacids: (a) \(\mathrm{Al}(\mathrm{OH})_{3}(s)\), (b) \(\mathrm{Mg}(\mathrm{OH})_{2}(s)\) (c) \(\mathrm{MgCO}_{3}(s)\) (d) \(\mathrm{NaAl}\left(\mathrm{CO}_{3}\right)(\mathrm{OH})_{2}(s),(\mathrm{e}) \mathrm{CaCO}_{3}(s)\)

Short Answer

Expert verified
The net ionic equations for the reaction of HCl(aq) with the given antacids are: (a) \(\mathrm{Al(OH)_{3}(s)} + 3\mathrm{H^+(aq)} \rightarrow \mathrm{Al^{3+}(aq)} + 3\mathrm{H_{2}O(l)}\) (b) \(\mathrm{Mg(OH)_{2}(s)} + 2\mathrm{H^+(aq)} \rightarrow \mathrm{Mg^{2+}(aq)} + 2\mathrm{H_{2}O(l)}\) (c) \(\mathrm{MgCO_{3}(s)} + 2\mathrm{H^+(aq)} \rightarrow \mathrm{Mg^{2+}(aq)} + \mathrm{H_{2}O(l)} + \mathrm{CO_{2}(g)}\) (d) \(2\mathrm{NaAl(CO_{3})(OH)_{2}(s)} + 6\mathrm{H^+(aq)} \rightarrow 2\mathrm{Na^+(aq)} + 2\mathrm{Al^{3+}(aq)} + 4\mathrm{H_{2}O(l)} + 2\mathrm{CO_{2}(g)}\) (e) \(\mathrm{CaCO_{3}(s)} + 2\mathrm{H^+(aq)} \rightarrow \mathrm{Ca^{2+}(aq)} + \mathrm{H_{2}O(l)} + \mathrm{CO_{2}(g)}\)

Step by step solution

01

1. Write the balanced chemical equation

Here are the balanced chemical equations for each reaction: (a) \(\mathrm{Al(OH)_{3}(s)} + 3\mathrm{HCl(aq)} \rightarrow \mathrm{AlCl_{3}(aq)} + 3\mathrm{H_{2}O(l)}\) (b) \(\mathrm{Mg(OH)_{2}(s)} + 2\mathrm{HCl(aq)} \rightarrow \mathrm{MgCl_{2}(aq)} + 2\mathrm{H_{2}O(l)}\) (c) \(\mathrm{MgCO_{3}(s)} + 2\mathrm{HCl(aq)} \rightarrow \mathrm{MgCl_{2}(aq)} + \mathrm{H_{2}O(l)} + \mathrm{CO_{2}(g)}\) (d) \(2\mathrm{NaAl(CO_{3})(OH)_{2}(s)} + 6\mathrm{HCl(aq)} \rightarrow 2\mathrm{NaCl(aq)} + 2\mathrm{AlCl_{3}(aq)} + 4\mathrm{H_{2}O(l)} + 2\mathrm{CO_{2}(g)}\) (e) \(\mathrm{CaCO_{3}(s)} + 2\mathrm{HCl(aq)} \rightarrow \mathrm{CaCl_{2}(aq)} + \mathrm{H_{2}O(l)} + \mathrm{CO_{2}(g)}\)
02

2. Separate aqueous ions

Now, we break down each aqueous solution into their respective ions: (a) \(\mathrm{Al(OH)_{3}(s)} + 3\mathrm{H^+(aq)} + 3\mathrm{Cl^-(aq)} \rightarrow \mathrm{Al^{3+}(aq)} + 3\mathrm{Cl^-(aq)} + 3\mathrm{H_{2}O(l)}\) (b) \(\mathrm{Mg(OH)_{2}(s)} + 2\mathrm{H^+(aq)} + 2\mathrm{Cl^-(aq)} \rightarrow \mathrm{Mg^{2+}(aq)} + 2\mathrm{Cl^-(aq)} + 2\mathrm{H_{2}O(l)}\) (c) \(\mathrm{MgCO_{3}(s)} + 2\mathrm{H^+(aq)} + 2\mathrm{Cl^-(aq)} \rightarrow \mathrm{Mg^{2+}(aq)} + 2\mathrm{Cl^-(aq)} + \mathrm{H_{2}O(l)} + \mathrm{CO_{2}(g)}\) (d) \(2\mathrm{NaAl(CO_{3})(OH)_{2}(s)} + 6\mathrm{H^+(aq)} + 6\mathrm{Cl^-(aq)} \rightarrow 2\mathrm{Na^+(aq)} + 2\mathrm{Cl^-(aq)} + 2\mathrm{Al^{3+}(aq)} + 6\mathrm{Cl^-(aq)} + 4\mathrm{H_{2}O(l)} + 2\mathrm{CO_{2}(g)}\) (e) \(\mathrm{CaCO_{3}(s)} + 2\mathrm{H^+(aq)} + 2\mathrm{Cl^-(aq)} \rightarrow \mathrm{Ca^{2+}(aq)} + 2\mathrm{Cl^-(aq)} + \mathrm{H_{2}O(l)} + \mathrm{CO_{2}(g)}\)
03

3. Cancel out spectator ions

We proceed to cancel out the spectator ions in each equation: (a) \(\cancel{3\mathrm{Cl^-(aq)}}\) (b) \(\cancel{2\mathrm{Cl^-(aq)}}\) (c) \(\cancel{2\mathrm{Cl^-(aq)}}\) (d) \(\cancel{2\mathrm{Cl^-(aq)}}\) and \(\cancel{6\mathrm{Cl^-(aq)}}\) (e) \(\cancel{2\mathrm{Cl^-(aq)}}\)
04

4. Write net ionic equations

Finally, we write the net ionic equations for each reaction: (a) \(\mathrm{Al(OH)_{3}(s)} + 3\mathrm{H^+(aq)} \rightarrow \mathrm{Al^{3+}(aq)} + 3\mathrm{H_{2}O(l)}\) (b) \(\mathrm{Mg(OH)_{2}(s)} + 2\mathrm{H^+(aq)} \rightarrow \mathrm{Mg^{2+}(aq)} + 2\mathrm{H_{2}O(l)}\) (c) \(\mathrm{MgCO_{3}(s)} + 2\mathrm{H^+(aq)} \rightarrow \mathrm{Mg^{2+}(aq)} + \mathrm{H_{2}O(l)} + \mathrm{CO_{2}(g)}\) (d) \(2\mathrm{NaAl(CO_{3})(OH)_{2}(s)} + 6\mathrm{H^+(aq)} \rightarrow 2\mathrm{Na^+(aq)} + 2\mathrm{Al^{3+}(aq)} + 4\mathrm{H_{2}O(l)} + 2\mathrm{CO_{2}(g)}\) (e) \(\mathrm{CaCO_{3}(s)} + 2\mathrm{H^+(aq)} \rightarrow \mathrm{Ca^{2+}(aq)} + \mathrm{H_{2}O(l)} + \mathrm{CO_{2}(g)}\)

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Most popular questions from this chapter

Three solutions are mixed together to form a single solution. One contains \(0.2 \mathrm{~mol} \mathrm{~Pb}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2},\) the second contains \(0.1 \mathrm{~mol} \mathrm{Na}_{2} \mathrm{~S},\) and the third contains \(0.1 \mathrm{~mol} \mathrm{CaCl}_{2}\). (a) Write the net ionic equations for the precipitation reaction or reactions that occur. (b) What are the spectator ions in the solution?

Glycerol, \(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}_{3},\) is a substance used extensively in the manufacture of cosmetics, foodstuffs, antifreeze, and plastics. Glycerol is a water-soluble liquid with a density of \(1.2656 \mathrm{~g} / \mathrm{mL}\) at \(15^{\circ} \mathrm{C}\). Calculate the molarity of a solution of glycerol made by dissolving \(50.000 \mathrm{~mL}\) glycerol at \(15^{\circ} \mathrm{C}\) in enough water to make \(250.00 \mathrm{~mL}\) of solution.

You choose to investigate some of the solubility guidelines for two ions not listed in Table \(4.1,\) the chromate ion \(\left(\mathrm{CrO}_{4}^{2-}\right)\) and the oxalate ion \(\left(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\right) .\) You are given \(0.01 \mathrm{M}\) solutions (A, B, C, D) of four water-soluble salts: $$ \begin{array}{lll} \hline \text { Solution } & \text { Solute } & \text { Color of Solution } \\ \hline \text { A } & \mathrm{Na}_{2} \mathrm{CrO}_{4} & \text { Yellow } \\ \mathrm{B} & \left(\mathrm{NH}_{4}\right)_{2} \mathrm{C}_{2} \mathrm{O}_{4} & \text { Colorless } \\ \mathrm{C} & \mathrm{AgNO}_{3} & \text { Colorless } \\ \mathrm{D} & \mathrm{CaCl}_{2} & \text { Colorless } \\ \hline \end{array} $$ When these solutions are mixed, the following observations are made: $$ \begin{array}{lll} \hline \text { Expt } & \text { Solutions } & \\ \text { Number } & \text { Mixed } & \text { Result } \\ \hline 1 & \mathrm{~A}+\mathrm{B} & \text { No precipitate, yellow solution } \\\ 2 & \mathrm{~A}+\mathrm{C} & \text { Red precipitate forms } \\ 3 & \mathrm{~A}+\mathrm{D} & \text { Yellow precipitate forms } \\ 4 & \mathrm{~B}+\mathrm{C} & \text { White precipitate forms } \\ 5 & \mathrm{~B}+\mathrm{D} & \text { White precipitate forms } \\ 6 & \mathrm{C}+\mathrm{D} & \text { White precipitate forms } \end{array} $$ (a) Write a net ionic equation for the reaction that occurs in each of the experiments. (b) Identify the precipitate formed, if any, in each of the experiments.

Define oxidation and reduction in terms of (a) electron transfer and (b) oxidation numbers.

Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (a) HF, (b) acetonitrile, \(\mathrm{CH}_{3} \mathrm{CN},\) (c) \(\mathrm{NaClO}_{4},\) (d) \(\mathrm{Ba}(\mathrm{OH})_{2}\).
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