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Chapter 15: Problem 44

Determine whether each of the following is a strong acid, weak acid, strong base, or weak base. Then write an equation describing the process that occurs when the substance is dissolved in water. (a) \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) (b) \(\mathrm{Ba}(\mathrm{OH})_{2}\) (c) \(\mathrm{HClO}_{4}\) (d) \(\mathrm{HBr}\)

Short Answer

Expert verified
Weak acid - \( \text{H}_{2} \text{C}_2 \text{O}_4 \), Strong base - \( \text{Ba(OH)}_2 \), Strong acids - \( \text{HClO}_4 \) and \( \text{HBr} \)

Step by step solution

01

- Identify \(\text{H}_{2} \text{C}_2 \text{O}_4\)

\( \text{H}_{2} \text{C}_2 \text{O}_4 = \text{oxalic acid}. \) It is a weak acid. Because it does not completely ionize in water.\[ \text{H}_{2} \text{C}_2 \text{O}_4(aq) \leftrightarrow 2\text{H}^+ (aq) + \text{C}_2 \text{O}_4^{2-}(aq) \]
02

- Identify \(\text{Ba(OH)}_2\)

\( \text{Ba(OH)}_2 = Barium hydroxide. \) It is a strong base. Because it completely ionizes in water.\[ \text{Ba(OH)}_2(aq) \rightarrow \text{Ba}^{2+}(aq) + 2\text{OH}^-(aq) \]
03

- Identify \(\text{HClO}_4\)

\( \text{HClO}_4 = Perchloric acid. \) It is a strong acid. Because it completely ionizes in water.\[ \text{HClO}_4(aq) \rightarrow \text{H}^+(aq) + \text{ClO}_4^-(aq) \]
04

- Identify \(\text{HBr}\)

\( \text{HBr} = Hydrobromic acid. \) It is a strong acid. Because it completely ionizes in water.\[ \text{HBr}(aq) \rightarrow \text{H}^+(aq) + \text{Br}^-(aq) \]

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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 a type of acid that completely dissociate in water. That means they release all their available hydrogen ions (\(H^+\)) when mixed with water. This complete dissociation is what makes them 'strong'.
Common examples of strong acids include:
  • Hydrochloric Acid (\(HCl\))
  • Perchloric Acid (\(HClO_4\))
  • Hydrobromic Acid (\(HBr\))
In an aqueous solution, these acids dissociate as follows:
$$ HClO_4 (aq) \rightarrow H^+ (aq) + ClO_4^- (aq) $$
$$ HBr (aq) \rightarrow H^+ (aq) + Br^- (aq) $$
This full release of \(H^+\) ions leads to a high level of acidity in the solution.
weak acids
Weak acids only partially dissociate in water. This means that not all their molecules release hydrogen ions into the solution. As a result, the solution contains both the acid and its ions in equilibrium.
Examples of weak acids include:
  • Acetic Acid (\(CH_3COOH\))
  • Oxalic Acid (\(H_2C_2O_4\))
  • Formic Acid (\(HCOOH\))
For weak acids, the dissociation can be represented as:
$$ H_2C_2O_4 (aq) \leftrightarrow 2H^+ (aq) + C_2O_4^{2-} (aq) $$
The double-headed arrow (\(\leftrightarrow\)) indicates that the reaction is in equilibrium, meaning not all molecules convert to ions.
strong bases
Strong bases fully dissociate in water, releasing hydroxide ions (\(OH^-\)). This complete dissociation characterizes their 'strength'.
Examples of strong bases include:
  • Sodium Hydroxide (\(NaOH\))
  • Potassium Hydroxide (\(KOH\))
  • Barium Hydroxide (\(Ba(OH)_2\))
In solution, they dissociate as follows:
$$ Ba(OH)_2 (aq) \rightarrow Ba^{2+} (aq) + 2OH^- (aq) $$
This release of \(OH^-\) ions increases the alkalinity of the solution significantly.
weak bases
Weak bases only partially dissociate in water. This means that not all molecules release hydroxide ions (\(OH^-\)).
Common examples of weak bases include:
  • Ammonia (\(NH_3\))
  • Methylamine (\(CH_3NH_2\))
For instance, Ammonia dissociates in water as follows:
$$ NH_3 (aq) + H_2O (l) \leftrightarrow NH_4^+ (aq) + OH^- (aq) $$
The equilibrium symbol (\(\leftrightarrow\)) indicates that the reaction doesn’t go to completion.
ionization in water
Ionization in water refers to the process by which an acid or base splits into its ions when dissolved in water. This can differ drastically between strong and weak substances.
For strong acids and bases, ionization is complete, producing high concentrations of ions. For example:
$$ HClO_4 (aq) \rightarrow H^+ (aq) + ClO_4^- (aq) $$
Weak acids and bases only partially ionize, leading to an equilibrium mixture of molecules and ions. For instance:
$$ H_2C_2O_4 (aq) \leftrightarrow 2H^+ (aq) + C_2O_4^{2-} (aq) $$
This concept is crucial for understanding solutions' properties and behaviors in various chemical reactions.

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Most popular questions from this chapter

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) \(3.0 \mathrm{M}\)

What volume of \(\mathrm{H}_{2}\) gas, measured at \(27^{\circ} \mathrm{C}\) and 700 . torr, can be obtained by reacting \(5.00 \mathrm{~g}\) of zinc metal with \(200 . \mathrm{mL}\) of \(0.350\) \(M \mathrm{HCl}\) ? The equation is $$ \mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g) $$

Determine the molarity of each of the ions present in the following aqueous salt solutions: (assume \(100 \%\) ionization) (a) \(2.25 \mathrm{M} \mathrm{} \mathrm{FeCl}_{3}\) (b) \(1.20 \mathrm{M} \mathrm{MgSO}_{4}\) (c) \(0.75 \mathrm{M} \mathrm{NaH}_{2} \mathrm{PO}_{4}\) (d) \(0.35 \mathrm{M} \mathrm{Ca}\left(\mathrm{ClO}_{3}\right)_{2}\)

What volume (mL) of \(0.4233 M \mathrm{H}_{2} \mathrm{SO}_{4}\) is needed to neutralize \(6.38 \mathrm{~g} \mathrm{KOH}\) ?

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