Logout Open In App
Open In App
Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

Chapter 16: Problem 51

Without referring to the text, write the formulas of four weak acids.

Short Answer

Expert verified
The formulas of four weak acids are \( \text{CH}_3\text{COOH} \), \( \text{C}_6\text{H}_8\text{O}_7 \), \( \text{HF} \), and \( \text{H}_2\text{SO}_3 \).

Step by step solution

Achieve better grades quicker with Premium

  • Unlimited AI interaction
  • Study offline
  • Say goodbye to ads
  • Export flashcards
Start your free trial Skip

Over 22 million students worldwide already upgrade their learning with Vaia!

01

Identify Weak Acids

Weak acids partially dissociate in water, meaning they do not completely ionize into their ions. Common examples include acetic acid, citric acid, hydrogen fluoride, and sulfurous acid.
02

Write the Formula for Acetic Acid

Acetic acid is a common weak acid used in vinegar. Its chemical formula is \( \text{CH}_3\text{COOH} \).
03

Write the Formula for Citric Acid

Citric acid, found in citrus fruits, has a chemical formula of \( \text{C}_6\text{H}_8\text{O}_7 \).
04

Write the Formula for Hydrogen Fluoride

Hydrogen fluoride is a weak acid in aqueous solution, and its formula is \( \text{HF} \).
05

Write the Formula for Sulfurous Acid

Sulfurous acid, often found in acid rain, has the chemical formula \( \text{H}_2\text{SO}_3 \).

Key Concepts

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

Chemical Formulas
Chemical formulas are representations of molecules using symbols for the elements and numbers to tell us how many of each element are present. This helps us understand what a compound is made of.
For weak acids, these formulas are key to identifying them and understanding their behavior in reactions.
  • They provide information about the types and numbers of atoms in a molecule.
  • For example, in the formula for acetic acid, \( \text{CH}_3\text{COOH} \), "C" stands for carbon, "H" for hydrogen, and "O" for oxygen.
  • This symbolic language lets scientists and students alike decode and work with chemical substances effectively.
Recognizing and writing chemical formulas is crucial for studying chemistry and understanding how different substances interact.
Acetic Acid
Acetic acid is a familiar weak acid, most commonly known as the acidic component of vinegar. Its chemical formula is \( \text{CH}_3\text{COOH} \), and it has distinct properties that make it important in everyday life.
This acid is characterized by its sour taste and strong smell, typical of vinegar. It partially dissociates in water, meaning it releases some hydrogen ions but not all.
  • It is used widely in the food industry as a preservative and flavoring agent.
  • In chemistry, it serves as an important reagent and solvent.
  • The molecule consists of two carbons, four hydrogens, and two oxygens, arranged in a specific structure that affects how it behaves.
Understanding acetic acid's formula and structure is essential for its applications in both industrial and household settings.
Citric Acid
Citric acid is another well-known weak acid, naturally occurring in citrus fruits like lemons and oranges. It has the chemical formula \( \text{C}_6\text{H}_8\text{O}_7 \), indicating its rich composition of carbon, hydrogen, and oxygen.
This acid contributes to the sour taste of fruits and is also used as a preservative in foods.
  • It plays a vital role in the metabolism process within cells, known as the citric acid cycle.
  • Its ability to form complexes with metals makes it valuable in cleaning products.
  • The presence of three carboxyl groups \((\text{COOH})\) makes it more complex compared to acetic acid.
Learning about citric acid's structure expands our understanding of its diverse roles in nature and industry.
Sulfurous Acid
Sulfurous acid is a weak acid recognized by its chemical formula \( \text{H}_2\text{SO}_3 \). This compound is known to form naturally in the environment, particularly in acid rain.
It is created when sulfur dioxide mixes with water in the atmosphere, leading to its weak acidic nature.
  • It doesn’t exist as a free substance but is part of other acidic processes.
  • It plays a role in chemical reactions that reduce other substances.
  • Consists of two hydrogens, one sulfur, and three oxygens, providing it with unique properties to engage in natural and industrial chemical processes.
Grasping sulfurous acid's characteristics is crucial for understanding both environmental science and chemical reactions.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Which of the following is the stronger base: \(\mathrm{NF}_{3}\) or \(\mathrm{NH}_{3}\) ? (Hint: \(\mathrm{F}\) is more electronegative than \(\mathrm{H}\).)

Calculate the \(\mathrm{pH}\) of an aqueous solution at \(25^{\circ} \mathrm{C}\) that is \(0.095 M\) in hydrocyanic acid \((\mathrm{HCN}) .\left(K_{\mathrm{a}}\right.\) for hydrocyanic acid \(\left.=4.9 \times 10^{-10} .\right)\)

In terms of orbitals and electron arrangements, what must be present for a molecule or an ion to act as a Lewis acid (use \(\mathrm{H}^{+}\) and \(\mathrm{BF}_{3}\) as examples)? What must be present for a molecule or ion to act as a Lewis base (use \(\mathrm{OH}^{-}\) and \(\mathrm{NH}_{3}\) as examples)?

Tooth enamel is largely hydroxyapatite \(\left[\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{3} \mathrm{OH}\right]\). When it dissolves in water (a process called demineralization), it dissociates as follows: $$ \mathrm{Ca}_{5}\left(\mathrm{PO}_{4}\right)_{3} \mathrm{OH} \longrightarrow 5 \mathrm{Ca}^{2+}+3 \mathrm{PO}_{4}^{3-}+\mathrm{OH}^{-} $$ The reverse process, called remineralization, is the body's natural defense against tooth decay. Acids produced from food remove the \(\mathrm{OH}^{-}\) ions and thereby weaken the enamel layer. Most toothpastes contain a fluoride compound such as \(\mathrm{NaF}\) or \(\mathrm{SnF}_{2}\). What is the function of these compounds in preventing tooth decay?

Calculate the \(\mathrm{pH}\) at \(25^{\circ} \mathrm{C}\) of a \(0.25-M\) aqueous solution of oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right) \cdot\left(K_{\mathrm{a}_{1}}\right.\) and \(K_{\mathrm{a}_{2}}\) for oxalic acid are \(6.5 \times 10^{-2}\) and \(6.1 \times 10^{-5}\), respectively.)
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Analysis

Read Explanation

Making Measurements

Read Explanation

Ionic and Molecular Compounds

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free