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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 鈥� 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鈥檛 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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Key Concepts

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

Strong Base
A strong base is a substance that fully dissociates in water, releasing hydroxide ions ( OH^鈭拀) into the solution. Typically, strong bases are composed of the hydroxides of alkali metals or alkaline earth metals. Some examples include:
  • Lithium hydroxide (LiOH)
  • Sodium hydroxide (NaOH)
  • Potassium hydroxide (KOH)
These bases fully split into their positive ions and hydroxide ions when in water, making them highly effective at increasing pH.
Fully dissociating means that in a solution, there are basically no original base molecules left; they have all split into ions. Hence, strong bases have a significant influence in chemical reactions since they provide a substantial concentration of hydroxide ions.
Weak Base
A weak base is a chemical base that doesn't fully ionize in solution. Rather than completely dissociating, these bases exist in a state of equilibrium where only a fraction of the molecules split into ions. The equilibrium can be represented as:\[B + H_2O \rightleftharpoons BH^+ + OH^鈭抃] where "B" represents the base. Because of this equilibrium state, weak bases are not as effective in increasing pH levels as strong bases are.
Examples of weak bases include:
  • Cyanide ion (CN^鈭�)
  • Ammonia (NH_3)
  • Bicarbonate ion (HCO_3^鈭�)
In these cases, the reaction with water does not go to completion, leading to a lower production of hydroxide ions compared to strong bases.
Amphoteric Compound
An amphoteric compound is a substance that can act both as an acid and as a base. Water (H_2O) is one of the most well-known amphoteric compounds, readily donating or accepting a proton. When acting as a base, water can accept a hydrogen ion to form the hydronium ion:\[H_2O + H^+ \rightarrow H_3O^+\] Conversely, when acting as an acid, water can donate a hydrogen ion to form the hydroxide ion:\[H_2O \rightarrow OH^鈭� + H^+\] Amphoteric behavior isn't limited to water alone. Several other substances, particularly some oxides and hydroxides, also display this dual behavior:
  • Zinc oxide (ZnO) - reacts with both acids and bases
  • Aluminum hydroxide (Al(OH)_3) - can neutralize acids and bases
This versatility allows amphoteric compounds to be involved in a greater range of chemical reactions.

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Most popular questions from this chapter

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?

A certain salt, MX (containing the \(\mathrm{M}^{+}\) and \(\mathrm{X}^{-}\) ions), is dissolved in water, and the \(\mathrm{pH}\) of the resulting solution is 7.0. Can you say anything about the strengths of the acid and the base from which the salt is derived?

Predict the direction that predominates in this reaction: $$\mathrm{F}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HF}(a q)+\mathrm{OH}^{-}(a q)$$

Calculate the concentrations of \(\mathrm{H}^{+}, \mathrm{HCO}_{3}^{-},\) and \(\mathrm{CO}_{3}^{2-}\) in a \(0.025 \mathrm{M} \mathrm{H}_{2} \mathrm{CO}_{3}\) solution.

What are the strongest acid and strongest base that can exist in water?
See all solutions

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