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Chapter 4: Problem 35

Classify each of the following as a strong or weak acid or base. a. HF b. \(\mathrm{KOH}\) c. \(\mathrm{HClO}_{4}\) d. HIO

Short Answer

Expert verified
a) HF: weak acid, b) KOH: strong base, c) HClO4: strong acid, d) HIO: weak acid.

Step by step solution

01

Understanding Acid and Base Strength

To classify acids and bases as strong or weak, we need to know their dissociation in water. Strong acids and bases dissociate completely, whereas weak acids and bases only partially dissociate.
02

Classifying HF

HF is hydrofluoric acid, which is known to only partially dissociate in water, making it a weak acid.
03

Classifying KOH

KOH is potassium hydroxide, which is a metal hydroxide and dissociates completely in water, therefore, it is a strong base.
04

Classifying  ext{HClO}_{4}

ext{HClO}_{4} is perchloric acid, well known for its complete dissociation in water, classifying it as a strong acid.
05

Classifying HIO

HIO, hypoiodous acid, is similar to HF in that it only partially dissociates in water, making it a weak acid.

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Key Concepts

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

Dissociation in Water
Dissociation in water is a crucial concept in understanding the strength of acids and bases. It refers to the process by which an acid or base separates into ions when dissolved in water. This separation is what allows the substance to conduct electricity and participate in chemical reactions.
For acids, the dissociation process involves the release of hydrogen ions (H鈦�) into solution. For bases, the dissociation typically results in the release of hydroxide ions (OH鈦�).
  • Complete Dissociation: If an acid or base dissociates fully into its ions in water, it is termed 'strong'.
  • Partial Dissociation: If an acid or base only partially dissociates in water, it is labeled as 'weak'.
Understanding dissociation helps predict an acid or base's behavior and its impact on the pH of a solution.
Strong Acid
Strong acids are a class of acids that dissociate completely in water, releasing all their hydrogen ions into the solution. This complete dissociation is what leads to their high characteristic of strong acids, making them highly effective at lowering the pH of solutions.
Here are some key points about strong acids:
  • Examples include \( ext{HClO}_{4}\) (perchloric acid), \( ext{HCl}\) (hydrochloric acid), \( ext{HNO}_{3}\) (nitric acid), and \( ext{H}_{2} ext{SO}_{4}\) (sulfuric acid).
  • They completely ionize in solution, meaning they have no undissociated molecules left.
  • They are great conductors of electricity due to the high concentration of ions.
The full dissociation results in a strong acid's ability to participate actively in chemical reactions and effectively acidify solutions.
Weak Acid
Weak acids differ from strong acids due to their incomplete dissociation in water. This means they only release some of their hydrogen ions into the solution, leaving a significant proportion of undissociated molecules.
Here are some aspects of weak acids:
  • Examples include HF (hydrofluoric acid) and HIO (hypoiodous acid).
  • They create an equilibrium between the dissociated ions and the undissociated acid, which means not all the acid contributes to the acidity of the solution.
  • They result in a relatively lesser change in the pH of the solution compared to strong acids.
Weak acids have a less pronounced effect on the pH, making them useful in scenarios requiring subtle acidity, like buffer solutions.
Strong Base
A strong base is an ionic compound that fully dissociates into its constituent ions in water. Strong bases release a large number of hydroxide ions (OH鈦�) into the solution, which significantly increases the pH, making the solution very basic.
Several important points about strong bases include:
  • Common examples are metal hydroxides like KOH (potassium hydroxide) and NaOH (sodium hydroxide).
  • They completely dissociate in water, contributing significantly to the solution's conductivity and basic nature.
  • They are highly effective at neutralizing acids due to their full ionic dissociation.
Due to their high reactivity, strong bases are used in applications where a significant shift in alkalinity is required, such as in chemical manufacturing and cleaning agents.
Weak Base
Weak bases do not dissociate fully in water; instead, they only partially release their hydroxide ions. This partial dissociation means that weak bases are less effective at increasing the pH of a solution compared to strong bases.
Look at the characteristics of weak bases:
  • Examples include ammonia (\( ext{NH}_{3}\)) and methylamine
  • They establish an equilibrium between the ionized and unionized base in the solution.
  • The concentration of hydroxide ions in the solution is lower than that of strong bases.
Weak bases are useful for maintaining controlled basicity, often employed in processes where gradual changes in pH are required, leveraging their mild alkalinity.

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Most popular questions from this chapter

Silver nitrate reacts with strontium chloride in an aqueous precipitation reaction. What are the formulas of silver nitrate and strontium chloride? Write the molecular equation and net ionic equation for the reaction. What are the names of the products? Give the molecular equation for another reaction that produces the same precipitate.

In the following reactions, label the oxidizing agent and the reducing agent. a. \(\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g)\) b. \(\mathrm{PbS}(s)+4 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{PbSO}_{4}(s)+4 \mathrm{H}_{2} \mathrm{O}(l)\)

A sample of \(\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}\) was heated to \(100^{\circ} \mathrm{C}\), where it lost water and gave another hydrate of copper(II) ion that contained 29.76\% Cu. An \(85.42-\mathrm{mg}\) sample of this new hydrate gave \(93.33 \mathrm{mg}\) of barium sulfate precipitate when treated with a barium nitrate solution. What is the formula of the new hydrate?

A sample of oxalic acid, \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\), weighing \(1.192 \mathrm{~g}\) is placed in a \(100.0-\mathrm{mL}\) volumetric flask, which is then filled to the mark with water. What is the molarity of the solution?

An aqueous solution contains \(4.00 \% \mathrm{NH}_{3}\) (ammonia) by mass. The density of the aqueous ammonia is \(0.979 \mathrm{~g} / \mathrm{mL}\). What is the molarity of \(\mathrm{NH}_{3}\) in the solution?
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