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Chapter 4: Problem 10

Identify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte: (a) \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\) (b) Ne, (c) \(\mathrm{NH}_{3}\) (d) \(\mathrm{NaOH}\).

Short Answer

Expert verified
(a) Barium nitrate is a strong electrolyte.\n(b) Neon is a nonelectrolyte.\n(c) Ammonia is a weak electrolyte.\n(d) Sodium hydroxide is a strong electrolyte.

Step by step solution

01

Analysis of Barium Nitrate (\(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\))

Barium nitrate is a salt which ionizes completely in water to give \( \mathrm{Ba^{2+}} \) and \( \mathrm{NO_{3}^-} \) ions. Therefore, it is a strong electrolyte.
02

Analysis of Neon (Ne)

Neon is a noble gas and it does not ionize or dissociate into ions in water. Therefore, it is a nonelectrolyte.
03

Analysis of Ammonia (\(\mathrm{NH}_{3}\))

Ammonia is a weak base which only partially ionizes in water to give \( \mathrm{NH_{4}^{+}} \) and \( \mathrm{OH^{-}} \) ions. Therefore, it is a weak electrolyte.
04

Analysis of Sodium Hydroxide (\(\mathrm{NaOH}\))

Sodium Hydroxide is a strong base which ionizes completely in water to give \( \mathrm{Na^{+}} \) and \( \mathrm{OH^{-}} \) ions. Therefore, it is a strong electrolyte.

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Most popular questions from this chapter

Ammonium nitrate \(\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)\) is one of the most important nitrogen-containing fertilizers. Its purity can be analyzed by titrating a solution of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) with a standard \(\mathrm{NaOH}\) solution. In one experiment a \(0.2041-\mathrm{g}\) sample of industrially prepared \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) required \(24.42 \mathrm{~mL}\) of \(0.1023 \mathrm{M} \mathrm{NaOH}\) for neutralization. (a) Write a net ionic equation for the reaction. (b) What is the percent purity of the sample?

Before aluminum was obtained by electrolytic reduction from its ore \(\left(\mathrm{Al}_{2} \mathrm{O}_{3}\right)\), the metal was produced by chemical reduction of \(\mathrm{AlCl}_{3}\). Which metals would you use to reduce \(\mathrm{Al}^{3+}\) to \(\mathrm{Al} ?\)

What is the difference between an ionic equation and a molecular equation?

Identify each of the following species as a Bronsted acid, base, or both: (a) HI, (b) \(\mathrm{CH}_{3} \mathrm{COO}^{-}\), (c) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) (d) \(\mathrm{HSO}_{4}^{-}\)

The concentration of \(\mathrm{Cu}^{2+}\) ions in the water (which also contains sulfate ions) discharged from a certain industrial plant is determined by adding excess sodium sulfide \(\left(\mathrm{Na}_{2} \mathrm{~S}\right)\) solution to \(0.800 \mathrm{~L}\) of the water. The molecular equation is $$ \mathrm{Na}_{2} \mathrm{~S}(a q)+\mathrm{CuSO}_{4}(a q) \longrightarrow_{\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\operatorname{CuS}(s)} $$ Write the net ionic equation and calculate the molar concentration of \(\mathrm{Cu}^{2+}\) in the water sample if \(0.0177 \mathrm{~g}\) of solid \(\mathrm{CuS}\) is formed.
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