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Chapter 15: Problem 2

Indicate whether each compound is an electrolyte or a nonelectrolyte in water: (a) \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) (b) \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{O}\) (c) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) (d) \(\mathrm{CH}_{3} \mathrm{OH}\) (e) \(\mathrm{CuSO}_{4}\) (f) \(\mathrm{KBr}\) (g) \(\mathrm{HBr}\)

Short Answer

Expert verified
(a) Al(NO3)3 is an electrolyte. (b) (CH3)2O is a nonelectrolyte. (c) (NH4)2SO4 is an electrolyte. (d) CH3OH is a nonelectrolyte. (e) CuSO4 is an electrolyte. (f) KBr is an electrolyte. (g) HBr is an electrolyte.

Step by step solution

01

(a) Al(NO3)3

Aluminium nitrate is a soluble ionic compound in water. When it dissolves in water, it dissociates into ions: \(\mathrm{Al}^{3+}\) and \(\mathrm{NO}_{3}^{-}\). Since it produces ions in solution, it is an electrolyte.
02

(b) (CH3)2O

Dimethyl ether is a covalent compound, and it does not dissociate into ions when dissolved in water. Since it does not produce ions in solution, it is a nonelectrolyte.
03

(c) (NH4)2SO4

Ammonium sulfate is a soluble ionic compound in water. When it dissolves in water, it dissociates into ions: \(\mathrm{NH}_{4}^{+}\) and \(\mathrm{SO}_{4}^{2-}\). Since it produces ions in solution, it is an electrolyte.
04

(d) CH3OH

Methanol is a covalent compound, and it does not dissociate into ions when dissolved in water. Since it does not produce ions in solution, it is a nonelectrolyte.
05

(e) CuSO4

Copper sulfate is a soluble ionic compound in water. When it dissolves in water, it dissociates into ions: \(\mathrm{Cu}^{2+}\) and \(\mathrm{SO}_{4}^{2-}\). Since it produces ions in solution, it is an electrolyte.
06

(f) KBr

Potassium bromide is a soluble ionic compound in water. When it dissolves in water, it dissociates into ions: \(\mathrm{K}^{+}\) and \(\mathrm{Br}^{-}\). Since it produces ions in solution, it is an electrolyte.
07

(g) HBr

Hydrogen bromide is a strong acid, which means it dissociates completely into ions when dissolved in water: \(\mathrm{H}^{+}\) and \(\mathrm{Br}^{-}\). Since it produces ions in solution, it is an electrolyte.

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Most popular questions from this chapter

Sulfuric acid, \(\mathrm{H}_{2} \mathrm{SO}_{4}\), is a diprotic acid with dissociation equilibrium constants of \(K_{\mathrm{eq}}>1.0 \times 10^{3}\) and \(K_{\mathrm{eq}}=1.2 \times 10^{-2} .\) Write the two dissociation equilibrium equations, and match the proper \(K_{\text {eq }}\) to each. Which species is the weak acid?

How would the Bronsted-Lowry theory explain that ammonia is a weak base?

A solution has an \(\mathrm{OH}\) concentration of \(10^{-11} \mathrm{M}\). (a) Is this solution basic or acidic? Explain how you know. (b) Without using a calculator, explain how you could quickly determine the \(\mathrm{H}_{3} \mathrm{O}\) concentration of this solution. What is that concentration?

The base- 10 logarithm of 60 is a number: (a) Between \(-2\) and \(-1\) (b) Between \(-1\) and 0 (c) Between 0 and 1 (d) Between 1 and 2 (e) Between 2 and 3

Based solely on concentrations, when is an aqueous solution judged to be basic? Give two answers to this question.
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