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Chapter 16: Problem 32

Classify each of these species as a weak or strong base: (a) LiOH, (b) \(\mathrm{CN}^{-}\) (c) \(\mathrm{H}_{2} \mathrm{O}\) (d) \(\mathrm{ClO}_{4}^{-},(\mathrm{e}) \mathrm{NH}_{2}^{-}\)

Short Answer

Expert verified
(a) \(LiOH\) is a strong base, (b) \(\mathrm{CN}^{-}\) is a weak base, (c) \(\mathrm{H}_{2} \mathrm{O}\) is a weak base, (d) \(\mathrm{ClO}_{4}^{-}\) is not a base, (e) \(\mathrm{NH}_{2}^{-}\) is a strong base.

Step by step solution

01

Identify \(LiOH\)

Lithium hydroxide (\(LiOH\)) is a Group 1 hydroxide. These species are classified as strong bases because they are completely ionized in solution.
02

Identify \(\mathrm{CN}^{-}\)

Cyanide ion (\(\mathrm{CN}^{-}\)) is classified as a weak base. This is due to its ability to accept a proton from water, forming hydrocyanic acid and hydroxide ion. However, this reaction does not proceed to completion – the majority of the cyanide ions remain unreacted in this reaction. Hence, it is termed as a weak base.
03

Identify \(\mathrm{H}_{2} \mathrm{O}\)

Water (\(\mathrm{H}_{2} \mathrm{O}\)) can both donate and accept a proton, which makes it an amphoteric compound. However, it is weak in both its acid and base characteristics- hence, it is a weak base.
04

Identify \(\mathrm{ClO}_{4}^{-}\)

The perchlorate ion (\(\mathrm{ClO}_{4}^{-}\)) isn't considered a base because it does not carry any unshared pair of electrons to accept an H+. Therefore, it doesn’t act as a base.
05

Identify \(\mathrm{NH}_{2}^{-}\)

The amide ion (\(\mathrm{NH}_{2}^{-}\)) is a strong base as it has an unbonded pair of electrons that can easily accept a proton. It is formed from the dissociation of ammonia (\(NH_3\)), which is a weak base- but the ion itself is a strong base.

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Most popular questions from this chapter

Classify these following oxides as acidic, basic, amphoteric, or neutral: (a) \(\mathrm{CO}_{2},\) (b) \(\mathrm{K}_{2} \mathrm{O},\) (c) \(\mathrm{CaO}\) (d) \(\mathrm{N}_{2} \mathrm{O}_{5},(\mathrm{e}) \mathrm{CO},(\mathrm{f}) \mathrm{NO}\) \((\mathrm{g}) \mathrm{SnO}_{2},(\mathrm{~h}) \mathrm{SO}_{3},(\mathrm{i}) \mathrm{Al}_{2} \mathrm{O}_{3}\) (j) \(\mathrm{BaO}\).

Classify each of these species as a Bronsted acid or base, or both: (a) \(\mathrm{H}_{2} \mathrm{O},\) (b) \(\mathrm{OH}^{-},\) (c) \(\mathrm{H}_{3} \mathrm{O}^{+}\), (d) \(\mathrm{NH}_{3}\) (e) \(\mathrm{NH}_{4}^{+},\) (f) \(\mathrm{NH}_{2}^{-},(\mathrm{g}) \mathrm{NO}_{3}^{-},\) (h) \(\mathrm{CO}_{3}^{2-}\) (i) HBr, (j) HCN.

You are given two beakers containing separately an aqueous solution of strong acid (HA) and an aqueous solution of weak acid (HB) of the same concentration. Describe how you would compare the strengths of these two acids by (a) measuring the \(\mathrm{pH},\) (b) measuring electrical conductance, (c) studying the rate of hydrogen gas evolution when these solutions are reacted with an active metal such as \(\mathrm{Mg}\) or \(\mathrm{Zn}\).

HA and \(\mathrm{HB}\) are both weak acids although \(\mathrm{HB}\) is the stronger of the two. Will it take more volume of a \(0.10 M \mathrm{NaOH}\) solution to neutralize \(50.0 \mathrm{~mL}\) of \(0.10 \mathrm{M}\) HB than \(50.0 \mathrm{~mL}\) of \(0.10 \mathrm{M}\) HA?

Write all the species (except water) that are present in a phosphoric acid solution. Indicate which species can act as a Bronsted acid, which as a Bronsted base, and which as both a Bronsted acid and a Bronsted base.
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