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Chapter 7: Problem 10

Hydrochloric acid is a stronger acid than acetic acid because (1) It can neutralize large quantity of alkali. (2) It can corrode anything it comes in contact. (3) It ionizes completely into ions in an aqueous solution. (4) It ionizes partially into ions in aqueous solution.

Short Answer

Expert verified
Option (3) - It ionizes completely into ions in an aqueous solution.

Step by step solution

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01

- Understand the Question

Read the question thoroughly to understand what is being asked. The question is asking why Hydrochloric acid is a stronger acid than acetic acid.
02

- Recall the Definition of Acid Strength

Recall that the strength of an acid is determined by its ability to completely ionize in an aqueous solution. A stronger acid ionizes more completely.
03

- Evaluate Each Option

Evaluate each answer option to determine which one aligns with the definition of a strong acid: 1. Neutralizing a large quantity of alkali does not define acid strength. 2. Corrosiveness also does not determine strength. 3. Complete ionization in an aqueous solution describes a strong acid. 4. Partial ionization describes a weak acid.
04

- Select the Correct Answer

Given the evaluation, option (3) 'It ionizes completely into ions in an aqueous solution' is the reason why Hydrochloric acid is stronger than acetic acid.

Key Concepts

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

ionization
Ionization refers to the process in which a molecule splits into ions when mixed with a solvent, typically water. This splitting allows the substance to participate more readily in chemical reactions.
For instance, when hydrochloric acid (HCl) is dissolved in water, it ionizes completely into hydrogen ions (H+) and chloride ions (Cl-).
Acetic acid (CH3COOH), on the other hand, only partially ionizes when in water. This results in fewer available hydrogen ions for reactions.
Complete ionization is what makes hydrochloric acid a strong acid, while partial ionization is why acetic acid is considered a weak acid.
  • Important takeaway: ionization extent directly affects acid strength.
aqueous solution
An aqueous solution is simply a solution where water acts as the solvent.
When an acid dissolves in water, it forms an aqueous solution, which allows the acid to ionize.
For example, when HCl is added to water, it forms an aqueous hydrochloric acid solution, where HCl dissociates completely into ions.
This complete ionization helps increase the solution's conductivity and its acidic properties.
Acetic acid in water forms an aqueous acetic acid solution but only partially separates into ions, resulting in lower conductivity.
  • Important takeaway: The nature of the aqueous solution affects how completely an acid can ionize.
strong acid
A strong acid is just an acid that completely ionizes in water, meaning it fully breaks up into ions.
This is key because the more an acid ionizes, the more hydrogen ions are released, making the solution more acidic.
Examples of strong acids include hydrochloric acid (HCl), sulfuric acid (H2SO4), and nitric acid (HNO3).
In contrast, acetic acid is a weak acid because it does not completely ionize in water.
  • Important takeaway: The extent of ionization determines if an acid is strong or weak.

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Most popular questions from this chapter

Let the solubilities of \(\mathrm{AgCl}\) in \(\mathrm{H}_{2} \mathrm{O}, 0.01 \mathrm{M} \mathrm{CaCl}_{2}\); \(0.01 \mathrm{M} \mathrm{NaCl}\) and \(0.05 \mathrm{M} \mathrm{AgNO}_{3}\) be \(\mathrm{S}_{1}, \mathrm{~S}_{2}, \mathrm{~S}_{3}\) and \(\mathrm{S}_{4}\) respectively. What is the correct relationship between these quantities? (1) \(S_{1}>S_{2}>S_{3}>S_{4}\) (2) \(S_{1}>S_{2}=S_{3}>S_{4}\) (3) \(S_{1}>S_{3}>S_{2}>S_{4}\) (4) \(S_{4}>S_{2}>S_{3}>S_{1}\)

To \(100 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{AgNO}_{3}\) solution, solid \(\mathrm{K}_{2} \mathrm{SO}_{4}\) is added. The concentration of \(\mathrm{K}_{2} \mathrm{SO}_{4}\) that shows the precipitation is \(\left(K_{s p}\right.\) for \(\left.\mathrm{A}_{\mathrm{g}_{2}} \mathrm{SO}_{4}=6.4 \times 10^{-5} \mathrm{M}\right)\) (1) \(0.1 \mathrm{M}\) (2) \(6.4 \times 10^{-3} \mathrm{M}\) (3) \(6.4 \times 10^{-7} \mathrm{M}\) (4) \(6.4 \times 10^{-5} \mathrm{M}\)

The ionic product of water is defined as (1) The product of the concentration of proton and hydroxyl ion in pure water (2) The product of the concentration of acid and hydroxyl ion in aqueous solution (3) The ratio of the concentration of dissociated water to the undissociated water (4) All the above

For the reaction \(\mathrm{Ag}_{2} \mathrm{CO}_{3}(\mathrm{~s}) \rightleftharpoons \mathrm{Ag}_{2} \mathrm{O}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})\) the value of the equilibrium constant \(\mathrm{K}_{\mathrm{p}}\) is \(3.16 \times 10^{3}\) atm at \(298 \mathrm{~K}\) and is \(1.48 \mathrm{~atm}\) at \(500 \mathrm{~K}\); then which one of the following statements is correct? (1) The yield of \(\mathrm{CO}_{2}\) is independent of temperature. (2) The yield of \(\mathrm{CO}_{2}\) will increase at high pressure. (3) The value of \(\Delta H\) for the forward reaction is negligible. (4) The forward reaction is endothermic.

Degrec of dissociation of weak acid and weak base are the same. If \(0.001 \mathrm{M}\) solution of weak acid has \(\mathrm{pII}=5.0\) then the pII of \(0.001 \mathrm{M}\) weak base is (1) 9 (2) 5 (3) 10 (4) 8
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