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

a. HCl

This acid consists of hydrogen (H) and chloride (Cl) ions. The anion is "chloride", so the acid name is "hydrochloric acid".

b. H2SO4

This acid contains hydrogen (H) and sulfate (SO4) ions. The anion is "sulfate", so the acid name is "sulfuric acid".

c. HNO3

This acid is composed of hydrogen (H) and nitrate (NO3) ions. The anion is "nitrate", so the acid name is "nitric acid".

d. HI

This acid consists of hydrogen (H) and iodide (I) ions. The anion is "iodide", so the acid name is "hydroiodic acid".

e. HNO2

This acid contains hydrogen (H) and nitrite (NO2) ions. The anion is "nitrite", so the acid name is "nitrous acid".

f. HClO3

This acid is composed of hydrogen (H) and chlorate (ClO3) ions. The anion is "chlorate", so the acid name is "chloric acid".

g. HBr

This acid consists of hydrogen (H) and bromide (Br) ions. The anion is "bromide", so the acid name is "hydrobromic acid".

h. HF

This acid contains hydrogen (H) and fluoride (F) ions. The anion is "fluoride", so the acid name is "hydrofluoric acid".

i. HC2H3O2

This acid is composed of hydrogen (H) and acetate (C2H3O2) ions. The anion is "acetate", so the acid name is "acetic acid".

Key concepts

Acid-Base Nomenclature

Understanding the names of acids in chemistry is crucial for recognizing their behavior and function. The nomenclature follows set rules according to the type of acid. Binary acids, composed of hydrogen and one nonmetal element, are named by adding the prefix 'hydro-' to the nonmetal and changing the ending to '-ic,' followed by the word 'acid.' For example, with hydrogen chloride ( \( HCl \) ), we arrive at 'hydrochloric acid.'

On the other hand, oxyacids contain hydrogen, oxygen, and another element. When the polyatomic ion (the part that is not hydrogen) ends in '-ate,' the acid name ends in '-ic.' If the polyatomic ion ends in '-ite,' the acid name ends in '-ous.' Thus, \( \mathrm{H}_{2} \mathrm{SO}_{4} \) (hydrogen sulfate) is 'sulfuric acid' and \( \mathrm{HClO}_{3} \) (hydrogen chlorate) is 'chloric acid.' This systematic approach to naming ensures that students and chemists can deduce the composition of an acid solely from its name.

Chemical Formula of Acids

An acid's chemical formula is a concise way of representing the atoms and ions that constitute the acid. For binary acids, the formula begins with hydrogen (denoted \( H \) ) followed by the symbol of the nonmetallic element. For example, hydroiodic acid, which consists of hydrogen and iodine ions, is designated as \( HI \) .

Oxyacids, on the other hand, have more complex formulas. They are generally written starting with hydrogen, but followed by a polyatomic ion containing oxygen and another element. A classic example is acetic acid, \( \mathrm{HC}_{2}\mathrm{H}_{3}\mathrm{O}_{2} \). Understanding these formulas allows students not only to identify the acid but also to predict its properties and reactivity patterns.

Properties of Acids

Acids are chemical compounds with distinct properties. They taste sour, react strongly with bases to form salts and water, and can conduct electricity when dissolved in water due to the breakdown into ions—a process known as dissociation. Acids can turn blue litmus paper red and are usually corrosive to metals, releasing hydrogen gas in the process.

Moreover, the strength of an acid is determined by its ability to donate hydrogen ions (protons) to bases – strong acids fully dissociate in solution, whereas weak acids only partially dissociate. For instance, hydrochloric acid ( \( HCl \)) is a strong acid that completely dissociates in water, while acetic acid ( \( \mathrm{HC}_2\mathrm{H}_3\mathrm{O}_2 \)) is a weak acid that dissociates to a lesser extent.