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Chapter 4: Problem 26

Commercial cold packs and hot packs are available for treating athletic injuries. Both types contain a pouch of water and a dry chemical. When the pack is struck, the pouch of water breaks, dissolving the chemical, and the solution becomes either hot or cold. Many hot packs use magnesium sulfate, and many cold packs use ammonium nitrate. Write reactions to show how these strong electrolytes break apart when they dissolve in water.

Short Answer

Expert verified
Magnesium sulfate (\(MgSO_4\)) dissociates in water as follows: \(MgSO_4 (aq) \rightarrow Mg^{2+} (aq) + SO_4^{2-} (aq)\). Ammonium nitrate (\(NH_4NO_3\)) dissociates in water as follows: \(NH_4NO_3 (aq) \rightarrow NH_4^{+} (aq) + NO_3^{-} (aq)\).

Step by step solution

01

Identify the magnesium sulfate formula

Magnesium sulfate is an ionic compound with the chemical formula \( MgSO_4 \). Step 2: Dissociation of magnesium sulfate in water
02

Dissociation of magnesium sulfate in water

When magnesium sulfate dissolves in water, it dissociates into magnesium ions and sulfate ions: \[ MgSO_4 (aq) \rightarrow Mg^{2+} (aq) + SO_4^{2-} (aq) \] For ammonium nitrate: Step 1: Identify the ammonium nitrate formula
03

Identify the ammonium nitrate formula

Ammonium nitrate is an ionic compound with the chemical formula \( NH_4NO_3 \). Step 2: Dissociation of ammonium nitrate in water
04

Dissociation of ammonium nitrate in water

When ammonium nitrate dissolves in water, it dissociates into ammonium ions and nitrate ions: \[ NH_4NO_3 (aq) \rightarrow NH_4^{+} (aq) + NO_3^{-} (aq) \] Thus, we have shown the reactions for strong electrolytes, magnesium sulfate and ammonium nitrate, breaking apart when they dissolve in water.

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Most popular questions from this chapter

A 0.500-L sample of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution was analyzed by taking a \(100.0-\mathrm{mL}\) aliquot and adding \(50.0 \mathrm{~mL}\) of \(0.213 M \mathrm{NaOH}\). After the reaction occurred, an excess of \(\mathrm{OH}^{-}\) ions remained in the solution. The excess base required \(13.21 \mathrm{~mL}\) of \(0.103 \mathrm{M} \mathrm{HCl}\) for neutralization. Calculate the molarity of the original sample of \(\mathrm{H}_{2} \mathrm{SO}_{4}\). Sulfuric acid has two acidic hydrogens.

A solution is prepared by dissolving \(0.5842 \mathrm{~g}\) oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) in enough water to make \(100.0 \mathrm{~mL}\) of solution. A \(10.00-\mathrm{mL}\) aliquot (portion) of this solution is then diluted to a final volume of \(250.0\) \(\mathrm{mL}\). What is the final molarity of the oxalic acid solution?

The vanadium in a sample of ore is converted to \(\mathrm{VO}^{2+}\). The VO \(^{2+}\) ion is subsequently titrated with \(\mathrm{MnO}_{4}^{-}\) in acidic solution to form \(\mathrm{V}(\mathrm{OH})_{4}{ }^{+}\) and manganese(II) ion. The unbalanced titration reaction is \(\mathrm{MnO}_{4}^{-}(a q)+\mathrm{VO}^{2+}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) $$ \mathrm{V}(\mathrm{OH})_{4}^{+}(a q)+\mathrm{Mn}^{2+}(a q)+\mathrm{H}^{+}(a q) $$ To titrate the solution, \(26.45 \mathrm{~mL}\) of \(0.02250 \mathrm{M} \mathrm{MnO}_{4}^{-}\) was required. If the mass percent of vanadium in the ore was \(58.1 \%\), what was the mass of the ore sample? Hint: Balance the titration reaction by the oxidation states method.

Polychlorinated biphenyls (PCBs) have been used extensively as dielectric materials in electrical transformers. Because PCBs have been shown to be potentially harmful, analysis for their presence in the environment has become very important. PCBs are manufactured according to the following generic reaction: $$ \mathrm{C}_{12} \mathrm{H}_{10}+n \mathrm{Cl}_{2} \rightarrow \mathrm{C}_{12} \mathrm{H}_{10-n} \mathrm{Cl}_{n}+n \mathrm{HCl} $$ This reaction results in a mixture of \(\mathrm{PCB}\) products. The mixture is analyzed by decomposing the PCBs and then precipitating the resulting \(\mathrm{Cl}^{-}\) as \(\mathrm{AgCl}\) a. Develop a general equation that relates the average value of \(n\) to the mass of a given mixture of \(\mathrm{PCBs}\) and the mass of AgCl produced b. A \(0.1947-\mathrm{g}\) sample of a commercial \(\mathrm{PCB}\) yielded \(0.4791 \mathrm{~g}\) of \(\mathrm{AgCl}\). What is the average value of \(n\) for this sample?

A solution of ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) in water is prepared by dissolving \(75.0 \mathrm{~mL}\) of ethanol (density \(=0.79 \mathrm{~g} / \mathrm{cm}^{3}\) ) in enough water to make \(250.0 \mathrm{~mL}\) of solution. What is the molarity of the ethanol in this solution?
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