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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
When magnesium sulfate (MgSO₄) and ammonium nitrate (NH₄NO₃) dissolve in water, they dissociate into their constituent ions acting as strong electrolytes. The dissociation reactions are as follows: \[MgSO_4(s) \rightarrow Mg^{2+}(aq) + SO_4^{2-}(aq)\] \[NH_4NO_3(s) \rightarrow NH_4^{+}(aq) + NO_3^{-}(aq)\]

Step by step solution

01

Understanding strong electrolytes

A strong electrolyte is a substance that completely dissociates into its ions when dissolved in water. This means that when the substance is dissolved, it breaks apart into its constituent ions, which can carry electric current. In this exercise, we need to understand how strong electrolytes magnesium sulfate (a hot pack component) and ammonium nitrate (a cold pack component) break apart when they dissolve in water. Step 2: Writing the chemical formula for magnesium sulfate
02

Writing the chemical formula for magnesium sulfate

Magnesium sulfate is a chemical compound made up of magnesium (Mg), sulfur (S), and oxygen (O). The formula for magnesium sulfate is MgSO_4. Step 3: Writing the dissociation reaction for magnesium sulfate in water
03

Writing the dissociation reaction for magnesium sulfate in water

When magnesium sulfate dissolves in water, it dissociates into its constituent ions: magnesium cation (Mg^2+) and sulfate anion (SO_4^2-). The balanced chemical equation for the dissociation of magnesium sulfate in water is as follows: \[MgSO_4(s) \rightarrow Mg^{2+}(aq) + SO_4^{2-}(aq)\] Step 4: Writing the chemical formula for ammonium nitrate
04

Writing the chemical formula for ammonium nitrate

Ammonium nitrate is a chemical compound made up of ammonium (NH_4) and nitrate (NO_3). The formula for ammonium nitrate is NH_4NO_3. Step 5: Writing the dissociation reaction for ammonium nitrate in water
05

Writing the dissociation reaction for ammonium nitrate in water

When ammonium nitrate dissolves in water, it dissociates into its constituent ions: ammonium cation (NH_4^+) and nitrate anion (NO_3^-). The balanced chemical equation for the dissociation of ammonium nitrate in water is as follows: \[NH_4NO_3(s) \rightarrow NH_4^{+}(aq) + NO_3^{-}(aq)\] In conclusion, when magnesium sulfate and ammonium nitrate dissolve in water, they act as strong electrolytes, breaking apart into their constituent ions. The dissociation reactions for magnesium sulfate and ammonium nitrate in water are as follows: \[MgSO_4(s) \rightarrow Mg^{2+}(aq) + SO_4^{2-}(aq)\] \[NH_4NO_3(s) \rightarrow NH_4^{+}(aq) + NO_3^{-}(aq)\]

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Most popular questions from this chapter

In most of its ionic compounds, cobalt is either \(\mathrm{Co}(\mathrm{II})\) or \(\mathrm{Co}(\mathrm{III})\). One such compound, containing chloride ion and waters of hydration, was analyzed, and the following results were obtained. A \(0.256-\mathrm{g}\) sample of the compound was dissolved in water, and excess silver nitrate was added. The silver chloride was filtered, dried, and weighed, and it had a mass of \(0.308 \mathrm{~g}\). A second sample of \(0.416 \mathrm{~g}\) of the compound was dissolved in water, and an excess of sodium hydroxide was added. The hydroxide salt was filtered and heated in a flame, forming cobalt(III) oxide. The mass of cobalt(III) oxide formed was \(0.145 \mathrm{~g}\). a. What is the percent composition, by mass, of the compound? b. Assuming the compound contains one cobalt ion per formula unit, what is the formula? c. Write balanced equations for the three reactions described.

Some of the substances commonly used in stomach antacids are \(\mathrm{MgO}, \mathrm{Mg}(\mathrm{OH})_{2}\), and \(\mathrm{Al}(\mathrm{OH})_{3} .\) a. Write a balanced equation for the neutralization of hydrochloric acid by each of these substances. b. Which of these substances will neutralize the greatest amount of \(0.10 M \mathrm{HCl}\) per gram?

A solution was prepared by mixing \(50.00 \mathrm{~mL}\) of \(0.100 \mathrm{M}\) \(\mathrm{HNO}_{3}\) and \(100.00 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{HNO}_{3} .\) Calculate the molarity of the final solution of nitric acid.

What volume of each of the following acids will react completely with \(50.00 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{NaOH}\) ? a. \(0.100 \mathrm{M} \mathrm{HCl}\) b. \(0.150 \mathrm{M} \mathrm{HNO}_{3}\) c. \(0.200 \mathrm{M} \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) ( 1 acidic hydrogen)

Assign oxidation states for all atoms in each of the following compounds. a. \(\mathrm{KMnO}_{4}\) b. \(\mathrm{NiO}_{2}\) c. \(\mathrm{Na}_{4} \mathrm{Fe}(\mathrm{OH})_{6}\) d. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4}\) e. \(\mathrm{P}_{4} \mathrm{O}_{6}\) f. \(\mathrm{Fe}_{3} \mathrm{O}_{4}\) g. \(\mathrm{XeOF}_{4}\) h. \(\mathrm{SF}_{4}\) i. CO j. \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)
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