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Chapter 3: Problem 47

Identify each substance as a strong electrolyte, weak electrolyte, or nonelectrolyte. (a) \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) (b) \(\mathrm{H}_{2} \mathrm{CO}_{3}\) (c) \(\mathrm{HNO}_{3}\) (d) \(\mathrm{KOH}\)

Short Answer

Expert verified
(a) Strong electrolyte, (b) Weak electrolyte, (c) Strong electrolyte, (d) Strong electrolyte.

Step by step solution

01

Understand Electrolytes Types

An electrolyte is a compound that dissociates into ions when dissolved in water. Strong electrolytes completely dissociate into ions, while weak electrolytes partially dissociate. Nonelectrolytes do not dissociate into ions.
02

Analyze (a) \(\mathrm{Na}_{2} \mathrm{CO}_{3}\)

\(\mathrm{Na}_{2} \mathrm{CO}_{3}\) (sodium carbonate) is an ionic compound that dissociates completely in water to form \(\mathrm{Na}^{+}\) and \(\mathrm{CO}_{3}^{2-}\) ions. Hence, it is a strong electrolyte.
03

Analyze (b) \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

\(\mathrm{H}_{2} \mathrm{CO}_{3}\) (carbonic acid) is a weak acid that only partially dissociates into \(\mathrm{H}^{+}\) and \(\mathrm{HCO}_{3}^{-}\) ions in water. Therefore, it is a weak electrolyte.
04

Analyze (c) \(\mathrm{HNO}_{3}\)

\(\mathrm{HNO}_{3}\) (nitric acid) is a strong acid that completely dissociates into \(\mathrm{H}^{+}\) and \(\mathrm{NO}_{3}^{-}\) ions when dissolved in water. Thus, it is a strong electrolyte.
05

Analyze (d) \(\mathrm{KOH}\)

\(\mathrm{KOH}\) (potassium hydroxide) is a strong base and an ionic compound that completely dissociates into \(\mathrm{K}^{+}\) and \(\mathrm{OH}^{-}\) ions in water. Therefore, it is a strong electrolyte.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Strong Electrolytes
Strong electrolytes are substances that completely dissociate into ions when they dissolve in water. This full dissociation means that the compound breaks apart entirely, resulting in a solution that presents a high concentration of ions. These ions are excellent conductors of electricity, making the solution electrically conductive.

Several types of compounds are typically strong electrolytes:
  • Ionic Compounds: These include many salts, such as sodium chloride (NaCl) and sodium carbonate (Na鈧侰O鈧�). Upon dissolving, these compounds separate into cations and anions, their ionic components.
  • Strong Acids and Bases: Examples include hydrochloric acid (HCl) and potassium hydroxide (KOH). These substances also completely ionize in water, providing free ions.
Strong electrolytes are crucial in many chemical reactions and industrial processes because of their efficient conductivity and dissociation properties.
Weak Electrolytes
Weak electrolytes are compounds that only partially dissociate into ions in water. This partial dissociation means that in solution, only a small fraction of the solute exists as ions, while the remainder remains as undissociated molecules.

Characteristics and examples include:
  • Weak Acids: A classic example is carbonic acid (H鈧侰O鈧�). In water, it dissociates slightly to form a small amount of hydrogen ( H鈦� ) and bicarbonate ( HCO鈧冣伝 ) ions.
  • Weak Bases: Ammonia (NH鈧�) in water forms a limited number of ammonium (NH鈧勨伜) and hydroxide (OH鈦�) ions.
Weak electrolytes lead to solutions with lower electrical conductivity compared to strong electrolytes. These substances are vital when gradual pH changes or specific ion balances are required in a solution.
Nonelectrolytes
Nonelectrolytes are substances that do not dissociate into ions at all when dissolved in water. As a result, these compounds remain as intact molecules in the solution, meaning that they do not conduct electricity because no free ions are present.

Examples of nonelectrolytes include:
  • Common Organic Compounds: Many organic compounds, like glucose (C鈧咹鈧佲倐O鈧�) and ethanol (C鈧侶鈧匫H), dissolve in water but don't produce ions.
  • Covalent Compounds: Unlike ionic compounds, covalent compounds typically do not form ions when dissolved. Water itself is a covalent molecule and acts as a nonelectrolyte under standard conditions.
Nonelectrolytes are important in biological systems and various chemical applications where non-conductive solutions are needed. Understanding these compounds helps clarify why some solutions conduct electricity, while others do not.

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Most popular questions from this chapter

Classify each of these as an acid or a base. Which are strong and which are weak? What ions are produced when each is dissolved in water? (a) \(\mathrm{KOH}\) (b) \(\mathrm{Mg}(\mathrm{OH})_{2}\) (c) \(\mathrm{HClO}\) (d) \(\mathrm{HBr}\) (e) \(\mathrm{LiOH}\) (f) \(\mathrm{H}_{2} \mathrm{SO}_{3}\)

Iron reacts with oxygen to give iron(III) oxide, \(\mathrm{Fe}_{2} \mathrm{O}_{3}\). (a) Write a balanced equation for this reaction. (b) An ordinary iron nail (assumed to be pure iron) has a mass of \(5.58 \mathrm{~g} ;\) calculate the mass (in grams) of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) that is produced when the nail is converted completely to \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) (c) Calculate the mass of \(\mathrm{O}_{2}\) (in grams) required for the reaction.

Nitrogen monoxide is oxidized in air to give brown nitrogen dioxide. $$2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NO}_{2}(\mathrm{~g})$$ Starting with \(2.2 \mathrm{~mol} \mathrm{NO},\) calculate how many moles and how many grams of \(\mathrm{O}_{2}\) are required for complete reaction. Calculate what mass of \(\mathrm{NO}_{2}\), in grams, is produced.

You need \(1.00 \mathrm{~L}\) of \(0.125-\mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\). Which method is best to prepare this solution? Explain your choice. (a) Dilute \(36.0 \mathrm{~mL}\) of \(1.25-\mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) to a volume of \(1.00 \mathrm{~L}\). (b) Dilute \(20.8 \mathrm{~mL}\) of \(6.00-\mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) to a volume of \(1.00 \mathrm{~L}\). (c) Add \(50.0 \mathrm{~mL}\) of \(3.00-\mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) to \(950 . \mathrm{mL}\) water. (d) Add 500. mL of \(0.500-\mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) to \(500 . \mathrm{mL}\) water.

An unknown solution contains either lead ions or barium ions, but not both. Which one of these solutions could you use to tell whether the ions present are \(\mathrm{Pb}^{2+}\) or \(\mathrm{Ba}^{2+}\) ? Explain the reasoning behind your choice. $$\mathrm{HCl}(\mathrm{aq}), \mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}), \mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq})$$
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