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Chapter 16: Problem 21

Write the formula for the hydronium ion. Write an equation for the formation of the hydronium ion when an acid is dissolved in water.

Short Answer

Expert verified
The formula for the hydronium ion is \(H_3O^+\). When a generic acid, HA, dissolves in water, the formation of the hydronium ion can be represented by the following equation: \(HA (aq) + H_2O (l) \rightarrow H_3O^+ (aq) + A^- (aq)\)

Step by step solution

01

Hydronium Ion Formula

The formula for the hydronium ion is H鈧僌鈦�.
02

Formation of Hydronium Ion Equation

Now let's consider a generic acid, HA, where H represents a hydrogen atom, and A represents the rest of the acid molecule. When HA dissolves in water, it donates a proton (H鈦�) to a water molecule. This forms the hydronium ion (H鈧僌鈦�) and a negatively charged anion (A鈦�). The general equation for this reaction is: HA (aq) + H鈧侽 (l) 鈫� H鈧僌鈦� (aq) + A鈦� (aq)

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Key Concepts

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

Hydronium Ion
The hydronium ion is a crucial part of acid-base chemistry. It is formed when an acid, like hydrogen chloride (HCl), donates a proton (H鈦�) to a water molecule (H鈧侽). When this happens, the water molecule accepts the proton and becomes the hydronium ion, denoted as H鈧僌鈦�. Understanding the role of the hydronium ion is important because it helps explain the behavior of acids in water. Remember, the hydronium ion carries a positive charge due to the extra hydrogen atom, making it responsible for the acidic characteristics of a solution.
Chemical Equations
Chemical equations are used to represent the transformations that occur during chemical reactions. They offer a concise way to illustrate the reactants transforming into products. In the case of forming hydronium ions, the chemical equation can be written as follows: \[ HA (aq) + H鈧侽 (l) \rightarrow H鈧僌鈦� (aq) + A鈦� (aq) \]
  • HA represents any acid that dissolves in water.
  • H鈧侽 is the solvent, water.
  • H鈧僌鈦� is the produced hydronium ion.
  • A鈦� is the anion left after the acid donates its proton.
This equation shows the interaction between an acid and water, resulting in the creation of hydronium ions and anions.
Dissociation Reactions
Dissociation reactions describe how compounds break apart into their ionic components. When an acid like HA is dissolved in water, it dissociates to form H鈦� ions and conjugate base ions (A鈦�). However, the process doesn't stop there. The H鈦� ions bond with water molecules to form hydronium ions (H鈧僌鈦�). This transformation is crucial for understanding the behavior of acids in aqueous solutions.
  • The breakdown of HA into H鈦� and A鈦� is termed dissociation.
  • The interaction of H鈦� with water to form H鈧僌鈦� emphasizes the concentration of hydronium ions in the solution.
  • These reactions highlight how acids function at the molecular level.
Dissociation reactions, therefore, help us grasp the complexities of solutions and the way that acids and bases interact in them.

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Most popular questions from this chapter

Strong bases are bases that completely ionize in water to produce hydroxide ion, \(\mathrm{OH}^{-}\). The strong bases include the hydroxides of the Group 1 elements. For example, if 1.0 mole of \(\mathrm{NaOH}\) is dissolved per liter, the concentration of \(\mathrm{OH}^{-}\) ion is \(1.0 \mathrm{M}\). Calculate the \(\left[\mathrm{OH}^{-}\right], \mathrm{pOH},\) and \(\mathrm{pH}\) for each of the following strong base solutions. a. \(0.10 M \mathrm{NaOH}\) b. \(2.0 \times 10^{-4} M \mathrm{KOH}\) c. \(6.2 \times 10^{-3} M \mathrm{CsOH}\) d. \(0.0001 M \mathrm{NaOH}\)

Given the general equation illustrating the reaction of the acid HA in water, $$ \mathrm{HA}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{A}^{-}(a q) $$ explain why water is considered a base in the Bronsted-Lowry model.

Choose pairs in which the species listed first is the conjugate base of the species listed second. a. \(\mathrm{S}^{2-}, \mathrm{HS}^{-}\) b. \(\mathrm{H}^{+}, \mathrm{OH}^{-}\) c. \(\mathrm{HBr}, \mathrm{Br}^{-}\) d. \(\mathrm{NO}_{2}^{-}, \mathrm{HNO}_{2}\)

Calculate the hydrogen ion concentration and the pH of each of the following solutions of strong acids. a. \(1.4 \times 10^{-3} M \mathrm{HClO}_{4}\) b. \(3.0 \times 10^{-5} M \mathrm{HCl}\) c. \(5.0 \times 10^{-2} M \mathrm{HNO}_{3}\) d. \(0.0010 M \mathrm{HCl}\)

For each hydrogen or hydroxide ion concentration listed, calculate the concentration of the complementary ion and the \(\mathrm{pH}\) and \(\mathrm{pOH}\) of the solution. a. \(\left[\mathrm{H}^{+}\right]=5.72 \times 10^{-4} M\) b. \(\left[\mathrm{OH}^{-}\right]=8.91 \times 10^{-5} M\) c. \(\left[\mathrm{H}^{+}\right]=2.87 \times 10^{-12} M\) d. \(\left[\mathrm{OH}^{-}\right]=7.22 \times 10^{-8} M\)
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