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Chapter 15: Problem 31

For each of the given pairs, determine which solution is more acidic. All are water solutions. Explain your answer. (a) \(1 M \mathrm{HCl}\) or \(1 M \mathrm{H}_{2} \mathrm{SO}_{4}\) ? (b) \(1 \mathrm{M} \mathrm{HCl}\) or \(1 M \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) ?

Short Answer

Expert verified
(a) 1 M H鈧係O鈧� is more acidic. (b) 1 M HCl is more acidic.

Step by step solution

01

Determine the Nature of Each Acid

Identify whether the acids are strong or weak. - HCl (hydrochloric acid) is a strong acid. - H鈧係O鈧� (sulfuric acid) is a strong acid. - HC鈧侶鈧僌鈧� (acetic acid) is a weak acid.
02

Compare the First Pair

For the pair of HCl and H鈧係O鈧�, considering both are strong acids: - HCl dissociates completely to give 1 mol of H鈦� ions per mole of HCl.- H鈧係O鈧� partially dissociates to give 2 mol of H鈦� ions per mole of H鈧係O鈧� (one in the first dissociation and one in the second dissociation). Since H鈧係O鈧� provides more H鈦� ions, it is more acidic.
03

Compare the Second Pair

For the pair of HCl and HC鈧侶鈧僌鈧�, considering one is a strong acid and the other is a weak acid: - HCl dissociates completely in water, yielding a high concentration of H鈦� ions. - HC鈧侶鈧僌鈧� does not dissociate completely, yielding fewer H鈦� ions compared to HCl at the same concentration. Therefore, HCl is more acidic.

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Key Concepts

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

Strong Acids
Strong acids are acids that completely dissociate in water. This means they break up entirely into their ions when dissolved. For instance, hydrochloric acid (HCl) is a strong acid. When HCl is added to water, it dissociates completely into H鈦� and Cl鈦� ions.

This complete dissociation results in a high concentration of hydrogen ions (H鈦�) in the solution. More hydrogen ions make the solution more acidic.

Examples of strong acids include:
  • Hydrochloric acid (HCl)
  • Sulfuric acid (H鈧係O鈧�) - although its second hydrogen dissociation is not complete
  • Nitric acid (HNO鈧�)
Understanding the nature of strong acids helps us compare their acidic strength effectively.
Weak Acids
Weak acids do not dissociate completely in water. This means that only a small fraction of the acid molecules break into their ions. Most of the acid remains intact in the solution. An example of a weak acid is acetic acid (HC鈧侶鈧僌鈧�), commonly known as vinegar.

When acetic acid is dissolved in water, it partially dissociates into H鈦� and C鈧侶鈧僌鈧傗伝 ions. Because the dissociation is incomplete, the concentration of hydrogen ions (H鈦�) is lower compared to a solution of a strong acid at the same concentration.

Examples of weak acids include:
  • Acetic acid (HC鈧侶鈧僌鈧�)
  • Formic acid (HCOOH)
  • Citric acid (C鈧咹鈧圤鈧�)
Knowing whether an acid is strong or weak helps us predict the acidity of its solution.
Dissociation in Water
Dissociation is the process by which an acid separates into ions when dissolved in water. For strong acids, dissociation is complete, resulting in many free H鈦� ions in the solution. For weak acids, dissociation is only partial, producing fewer H鈦� ions.

To understand dissociation better, consider these points:
  • Complete Dissociation: Strong acids like HCl dissociate fully, so in a 1 M solution of HCl, nearly all HCl molecules become H鈦� and Cl鈦� ions.
  • Partial Dissociation: Weak acids, such as acetic acid, dissociate only slightly. In a 1 M solution of acetic acid, most of the molecules remain as HC鈧侶鈧僌鈧�, with only a few breaking up into H鈦� and C鈧侶鈧僌鈧傗伝 ions.
This difference in dissociation explains why strong acids create more acidic solutions than weak acids at the same concentration. More H鈦� ions from complete dissociation mean a lower pH and higher acidity.

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Most popular questions from this chapter

Determine the molarity of each of the ions present in the following aqueous salt solutions: (assume \(100 \%\) ionization) (a) \(1.25 M \mathrm{CuBr}_{2}\) (b) \(0.75 \mathrm{M} \mathrm{NaHCO}_{3}\) (c) \(3.50 M \mathrm{~K}_{3} \mathrm{AsO}_{4}\) (d) \(0.65 M\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\)

Calculate the \(\mathrm{pH}\) of solutions having the following \(\left[\mathrm{H}^{+}\right]\): (a) \(0.0020 \mathrm{M}\) (b) \(7.0 \times 10^{-8} M\) (c) \(3.0 \mathrm{M}\)

Two drops \((0.1 \mathrm{~mL})\) of \(1.0 \mathrm{M} \mathrm{HCl}\) are added to water to make \(1.0 \mathrm{~L}\) of solution. What is the \(\mathrm{pH}\) of this solution if the \(\mathrm{HCl}\) is \(100 \%\) ionized?

Write an equation showing how sodium sulfate dissociates in water.

Balance each of the following equations; then change them into balanced net ionic equations: (a) \(\mathrm{Mg}(s)+\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow \mathrm{Cu}(s)+\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) (b) \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{NaOH}(a q) \longrightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) (c) \(\mathrm{K}_{2} \mathrm{SO}_{3}(a q)+\mathrm{HClO}_{4}(a q) \longrightarrow\) \(\mathrm{KClO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{SO}_{2}(g)\)
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