Question

Name each of the following acids. a. HCl b. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) c. \(\mathrm{HNO}_{3}\) d. HI e. \(\mathrm{HNO}_{2}\) f. \(\mathrm{HClO}_{3}\) g. HBr h. HF i. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)

Short answer

a. Hydrochloric acid b. Sulfuric acid c. Nitric acid d. Hydroiodic acid e. Nitrous acid f. Chloric acid g. Hydrobromic acid h. Hydrofluoric acid i. Acetic acid

Step-by-step solution

Identify anion in the acid

In HCl, the anion is Cl⁻.

Name the acid

Since the anion is Cl⁻ and ends with -ide, the name of the acid is Hydrochloric acid. #b. \(\mathrm{H}_{2} \mathrm{SO}_{4}\)#

Identify anion in the acid

In \(\mathrm{H}_{2} \mathrm{SO}_{4}\), the anion is \(\mathrm{SO}_{4}^{2-}\)

Name the acid

Since the anion has an -ate ending (sulfate), the name of the acid is Sulfuric acid. #c. \(\mathrm{HNO}_{3}\)#

Identify anion in the acid

In \(\mathrm{HNO}_{3}\), the anion is \(\mathrm{NO}_{3}^{-}\).

Name the acid

Since the anion has an -ate ending (nitrate), the name of the acid is Nitric acid. #d. HI#

Identify anion in the acid

In HI, the anion is I⁻.

Name the acid

Since the anion is I⁻ and ends with -ide, the name of the acid is Hydroiodic acid. #e. \(\mathrm{HNO}_{2}\)#

Identify anion in the acid

In \(\mathrm{HNO}_{2}\), the anion is \(\mathrm{NO}_{2}^{-}\).

Name the acid

Since the anion has an -ite ending (nitrite), the name of the acid is Nitrous acid. #f. \(\mathrm{HClO}_{3}\)#

Identify anion in the acid

In \(\mathrm{HClO}_{3}\), the anion is \(\mathrm{ClO}_{3}^{-}\).

Name the acid

Since the anion has an -ate ending (chlorate), the name of the acid is Chloric acid. #g. HBr#

Identify anion in the acid

In HBr, the anion is Br⁻.

Name the acid

Since the anion is Br⁻ and ends with -ide, the name of the acid is Hydrobromic acid. #h. HF#

Identify anion in the acid

In HF, the anion is F⁻.

Name the acid

Since the anion is F⁻ and ends with -ide, the name of the acid is Hydrofluoric acid. #i. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)#

Identify anion in the acid

In \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\), the anion is \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\).

Name the acid

Since the anion has an -ate ending (acetate), the name of the acid is Acetic acid.

Key concepts

Anion Identification

When you want to name an acid, the first step is to determine which anion is paired with hydrogen in the formula. Anions are negatively charged ions, and in acids, they are combined with hydrogen to form the compound. To do this, you must be familiar with different types of anions and their typical endings, such as

• \(-\text{ide}\) for simple anions like \(\text{Cl}^-, \text{I}^-, \text{Br}^-, \) and \(\text{F}^-\),
• \(-\text{ate}\) for polyatomic anions like \(\text{SO}_4^{2-} \) and \(\text{NO}_3^-\),
• \(-\text{ite}\) for polyatomic anions like \(\text{NO}_2^-\).

Being able to recognize these suffixes will help you correctly identify the anion present in a given acid, which is the key to correctly naming the acid.

Chemical Formulas

Chemical formulas are your blueprint to understanding any chemical compound. When it comes to acids, the formula typically begins with hydrogen (H). The subscript numbers in each formula indicate how many of each atom are present. For instance:

• In \(\text{HCl}\), there is one hydrogen (H) and one chlorine (Cl).
• In \(\text{H}_2\text{SO}_4\), there are two hydrogens (H), one sulfur (S), and four oxygens (O).
• Similarly, \(\text{HC}_2\text{H}_3\text{O}_2\) includes two hydrogens (H), two carbons (C), and two oxygens (O).

By breaking down the formula step by step, you can trace back each element to its counterpart ion, allowing for accurate identification and proper naming of the acid. The way formulas are written is crucial for understanding the composition and properties of acids.

Acid Naming Rules

Naming acids may seem overwhelming at first, but following a set of simple rules can make the process straightforward. Here are some basic guidelines:

• If the anion ends in \(-\text{ide}\), the acid name begins with 'hydro-' and the anion name ends with '-ic acid'. For example, \(\text{HCl}\) becomes hydrochloric acid.
• If the anion ends in \(-\text{ate}\), the acid name ends with '-ic acid'. For example, \(\text{H}_2\text{SO}_4\) becomes sulfuric acid.
• If the anion ends in \(-\text{ite}\), the acid name changes to end with '-ous acid'. For instance, \(\text{HNO}_2\) becomes nitrous acid.

These rules streamline the naming process, providing consistency and clarity. By understanding these conventions, you can confidently name any acid from its chemical formula.