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Chapter 5: Problem 28

Every antacid contains one or more ingredients capable of reacting with excess stomach acid (HCl). The essential neutralization products are \(\mathrm{CO}_{2}\) and/ or \(\mathrm{H}_{2} \mathrm{O} .\) Write net ionic equations to represent the neutralizing action of the following popular antacids. (a) Alka-Seltzer (sodium bicarbonate) (b) Tums (calcium carbonate) (c) milk of magnesia (magnesium hydroxide) (d) Maalox (magnesium hydroxide, aluminum hydroxide) (e) Rolaids \(\left[\mathrm{NaAl}(\mathrm{OH})_{2} \mathrm{CO}_{3}\right]\)

Short Answer

Expert verified
The net ionic equations for the antacids are: (a) \(\mathrm{HCO}_{3}^{-}(aq) + \mathrm{H}^{+}(aq) \rightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{CO}_{2}(g)\), (b) \(\mathrm{CO}_{3}^{2-}(aq) + 2 \mathrm{H}^{+}(aq) \rightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{CO}_{2}(g)\), (c) \(\mathrm{OH}^{-}(aq) + \mathrm{H}^{+}(aq) \rightarrow \mathrm{H}_{2}\mathrm{O}(l)\), (d) \(\mathrm{OH}^{-}(aq) + \mathrm{H}^{+}(aq) \rightarrow \mathrm{H}_{2}\mathrm{O}(l)\), (e) The reaction could be broken into two steps and result in neutralization with water and carbon dioxide. In all of them, stomach acid is neutralized producing water and in some cases carbon dioxide.

Step by step solution

01

Writing Net Ionic Equation for Alka-Seltzer

Alka-Seltzer contains sodium bicarbonate (NaHCO3). The reaction of sodium bicarbonate and hydrochloric acid (HCl) can be written as follows: \[ \mathrm{NaHCO}_{3}(s) + \mathrm{HCl}(aq) \rightarrow \mathrm{NaCl}(aq) + \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{CO}_{2}(g) \] The net ionic equation, showing only species that actually participate in the reaction, will therefore be: \[ \mathrm{HCO}_{3}^{-}(aq) + \mathrm{H}^{+}(aq) \rightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{CO}_{2}(g) \]
02

Writing Net Ionic Equation for Tums

Tums contains calcium carbonate (CaCO3). The reaction of calcium carbonate and hydrochloric acid can be written as follows: \[ \mathrm{CaCO}_{3}(s) + 2 \mathrm{HCl}(aq) \rightarrow \mathrm{CaCl}_{2}(aq) + \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{CO}_{2}(g) \] The net ionic equation will therefore be: \[ \mathrm{CO}_{3}^{2-}(aq) + 2 \mathrm{H}^{+}(aq) \rightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{CO}_{2}(g) \]
03

Writing Net Ionic Equation for Milk of Magnesia

Milk of Magnesia contains magnesium hydroxide (Mg(OH)2). The reaction of magnesium hydroxide and hydrochloric acid is: \[ \mathrm{Mg(OH)}_{2}(s) + 2 \mathrm{HCl}(aq) \rightarrow \mathrm{MgCl}_{2}(aq) + 2 \mathrm{H}_{2}\mathrm{O}(l) \] The net ionic equation is reduced to: \[ \mathrm{OH}^{-}(aq) + \mathrm{H}^{+}(aq) \rightarrow \mathrm{H}_{2}\mathrm{O}(l) \]
04

Writing Net Ionic Equation for Maalox

Maalox contains magnesium hydroxide and aluminum hydroxide (Al(OH)3). However, for the purpose of this exercise and to keep it straightforward, the net ionic equation, as with magnesium hydroxide in milk of magnesia, for the reaction with stomach acid is: \[ \mathrm{OH}^{-}(aq) + \mathrm{H}^{+}(aq) \rightarrow \mathrm{H}_{2}\mathrm{O}(l) \]
05

Writing Net Ionic Equation for Rolaids

Rolaids contains sodium aluminate (NaAl(OH)2CO3). The net ionic equation for its reaction with hydrochloric acid is somewhat complex due to the presence of three different ions in the formula. However, for simplicity, this could be broken down into two steps with the resulting net ionic equation being similar to the one in Step 1 related to sodium bicarbonate and in Step 4 related to hydroxide ions.

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Most popular questions from this chapter

Assign oxidation states to the elements involved in the following reactions. Indicate which are redox reactions and which are not. (a) $\mathrm{MgCO}_{3}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow$ $\mathrm{Mg}^{2+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{CO}_{2}(\mathrm{g})$ (b) $\mathrm{Cl}_{2}(\mathrm{aq})+2 \mathrm{Br}^{-}(\mathrm{aq}) \longrightarrow 2 \mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{Br}_{2}(\mathrm{aq})$ (c) $\mathrm{Ag}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq})+\mathrm{NO}_{3}^{-}(\mathrm{aq}) \longrightarrow$ $\mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(1)+\mathrm{NO}_{2}(\mathrm{g})$ (d) $2 \mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{CrO}_{4}^{2-}(\mathrm{aq}) \longrightarrow \mathrm{Ag}_{2} \mathrm{CrO}_{4}(\mathrm{s})$

Predict in each case whether a reaction is likely to occur. If so, write a net ionic equation. (a) $\mathrm{AgNO}_{3}(\mathrm{aq})+\mathrm{CuCl}_{2}(\mathrm{aq}) \longrightarrow$ (b) $\mathrm{Na}_{2} \mathrm{S}(\mathrm{aq})+\mathrm{FeCl}_{2}(\mathrm{aq}) \longrightarrow$ (c) $\mathrm{Na}_{2} \mathrm{CO}_{3}(\mathrm{aq})+\mathrm{AgNO}_{3}(\mathrm{aq}) \longrightarrow$

The following reactions do not occur in aqueous solutions. Balance their equations by the half-equation method, as suggested in Are You Wondering \(5-2\) (a) \(\mathrm{CH}_{4}(\mathrm{g})+\mathrm{NO}(\mathrm{g}) \longrightarrow\) \(\mathrm{CO}_{2}(\mathrm{g})+\mathrm{N}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) (b) \(\mathrm{H}_{2} \mathrm{S}(\mathrm{g})+\mathrm{SO}_{2}(\mathrm{g}) \longrightarrow \mathrm{S}_{8}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) (c) \(\mathrm{Cl}_{2} \mathrm{O}(\mathrm{g})+\mathrm{NH}_{3}(\mathrm{g}) \longrightarrow\) \(\mathrm{N}_{2}(\mathrm{g})+\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(1)\)

Which aqueous solution has the greatest \(\left[\mathrm{H}^{+}\right]:\) (a) \(0.011 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH} ;\) (b) \(0.010 \mathrm{M} \mathrm{HCl} ;\) (c) \(0.010 \mathrm{M}\) \(\mathrm{H}_{2} \mathrm{SO}_{4} ;\) (d) \(1.00 \mathrm{M} \mathrm{NH}_{3} ?\) Explain your choice.

Determine which of the following react(s) with HCl(ag) to produce a gas, and write a net ionic equation(s) for the reaction(s). (a) \(\mathrm{Na}_{2} \mathrm{SO}_{4} ;\) (b) \(\mathrm{KHSO}_{3}\); (c) \(\mathrm{Zn}(\mathrm{OH})_{2};\) (d) \(\mathrm{CaCl}_{2}\).
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