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Chapter 16: Problem 5

What is a hydronium ion? Does H+ exist in solution by itself?

Short Answer

Expert verified
A hydronium ion is \( \text{H}_3\text{O}^+ \) and represents a hydrogen ion bonded to a water molecule. The \( \text{H}^+ \) ion does not exist by itself in solution; it combines with water to form the stable hydronium ion.

Step by step solution

01

Identification of a Hydronium Ion

A hydronium ion is the term for the hydrogen ion in an aqueous solution and is represented by the chemical formula \( \text{H}_3\text{O}^+ \). It is formed when an acid donates a proton (\( \text{H}^+ \)) to a water molecule.
02

Stability of H+ in Solution

In an aqueous solution, the hydrogen ion (\( \text{H}^+ \)) does not exist by itself due to its strong tendency to interact with other molecules. Instead, it associates with water to form the more stable hydronium ion \( \text{H}_3\text{O}^+ \).

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Key Concepts

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

Acid-Base Reactions
Understanding acid-base reactions is crucial in the study of chemistry, particularly when discussing ions such as the hydronium ion. These reactions are characterized by the transfer of protons between molecules. An acid is a substance that can donate protons, while a base is one that can accept them.

When an acid is dissolved in water, an acid-base reaction occurs, resulting in the donation of a proton to a water molecule. This interaction forms new products, one of which is the hydronium ion. The presence of hydronium ions is a key indicator of the acidic nature of a solution; the higher the concentration of hydronium ions, the more acidic the solution is.
Proton Donation
Proton donation is at the heart of acid-base chemistry. A proton, which is simply a hydrogen atom stripped of its electron, carries a positive charge denoted as \( \text{H}^+ \).

In aqueous solutions, acids will donate these protons, but the protons do not exist freely due to their high charge density and instability alone. Thus, they quickly associate with nearby water molecules, resulting in the formation of hydronium ions. This characteristic proton donation process defines why we perceive solutions as acidic and impacts the pH level of the solution.
Aqueous Solutions
An aqueous solution is a solution where water is the solvent. It is the medium in which many chemical reactions, including acid-base interactions, take place. In the context of the hydronium ion, the aqueous nature of the solution is essential.

Water is a polar molecule that readily forms hydrogen bonds with cations such as \( \text{H}^+ \). This unique property of water allows it to stabilize protons by forming hydronium ions. Without the aqueous environment, the chemistry of protons and their bonds with other molecules would be vastly different.
Chemical Formula
A chemical formula represents the types and numbers of atoms in a molecule. For the hydronium ion, the chemical formula is \( \text{H}_3\text{O}^+ \). This formula tells us that a hydronium ion consists of three hydrogen atoms and one oxygen atom, with an overall positive charge.

The formulation of this ion is a direct consequence of proton donation in an aqueous solution. It succinctly conveys the actual structure of the hydronium ion, which is pivotal in understanding acid-base behavior and the resultant chemistry in solutions.

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Most popular questions from this chapter

Morphine is a weak base. A 0.150 M solution of morphine has a pH of 10.5. What is Kb for morphine?

Identify the Lewis acid and Lewis base among the reactants in each equation. a. Ag+(aq) + 2 NH3(aq)Ag(NH3)2+(aq) b. AlBr3 + NH3H3NAlBr3 c. F-(aq) + BF3(aq)BF4-(aq)

A solution of 0.23 mol of the chloride salt of protonated quinine (QH+), a weak organic base, in 1.0 L of solution has pH = 4.58. Find the Kb of quinine (Q).

Write net ionic equations for the reactions that take place when aqueous solutions of each pair of substances are mixed. a. sodium cyanide and nitric acid b. ammonium chloride and sodium hydroxide c. sodium cyanide and ammonium bromide d. potassium hydrogen sulfate and lithium acetate e. sodium hypochlorite and ammonia

Determine the pH of each two-component solution. a. 0.0550 M in HI and 0.00850 M in HF b. 0.112 M in NaCl and 0.0953 M in KF c. 0.132 M in NH4Cl and 0.150 M HNO3 d. 0.0887 M in sodium benzoate and 0.225 M in potassium bromide e. 0.0450 M in HCl and 0.0225 M in HNO3
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