Test: Study of Compounds - Ammonia and Nitric Acid - Class 10 MCQ

When nitric acid reacts with alkaline earth metals, it produces metal nitrates and releases nitrogen dioxide gas. This reaction illustrates the strong oxidizing nature of nitric acid, particularly with reactive metals.

Nitric acid is classified as a monobasic acid because it can donate only one proton (H+) per molecule in an aqueous solution. This characteristic makes it a strong acid, fully ionizing in water, which is significant in various chemical reactions.

Nitric acid oxidizes sulfur to produce sulfuric acid. This reaction showcases nitric acid's strong oxidizing capacity, which allows it to convert elements into their highest oxidation states.

When nitric acid reacts with sodium bicarbonate, it produces sodium nitrate, water, and carbon dioxide gas. The release of carbon dioxide is a characteristic of reactions involving bicarbonates and acids.

Nitric acid decomposes when exposed to sunlight. This decomposition can lead to the formation of nitrogen dioxide, which is a brown gas. This behavior necessitates the storage of nitric acid in dark containers to minimize degradation.

The specific gravity of pure nitric acid is 1.54, which means it is heavier than water. Specific gravity is a useful property for identifying substances and understanding their behavior in mixtures and reactions.

When concentrated nitric acid reacts with metals, it produces metal nitrates and liberates nitric oxide. This reaction is characteristic of the strong oxidizing properties of nitric acid, which can oxidize metals.

A strong acid like nitric acid completely ionizes in water, meaning it dissociates fully into hydrogen ions (H+) and nitrate ions (NO3-). This complete ionization is what gives strong acids their significant acidic properties.

The boiling point of pure nitric acid is 86°C. This property indicates that nitric acid can easily transition from a liquid to a gaseous state when heated. Understanding boiling points is important in chemical processes where temperature control is critical.

Mixing nitric acid with concentrated hydrochloric acid produces aqua regia, a powerful solvent capable of dissolving noble metals. This mixture is important in various chemical processes and metal refining due to its unique properties.

Aqua regia is particularly known for its ability to dissolve noble metals such as gold and platinum. This property is due to the presence of nascent chlorine, which can react with these metals to form soluble chlorides.

The reaction 3Cu + 8HNO₃ → Cu(NO₃)₂ + 2H₂O + 2NO₂ illustrates nitric acid acting as an oxidizing agent, converting copper to copper nitrate while itself being reduced. This property is crucial in various chemical syntheses and during metal processing.

Aqua regia is a mixture of nitric acid and hydrochloric acid, commonly used to dissolve noble metals such as gold and platinum. Its name, which means "royal water" in Latin, reflects its ability to dissolve metals that other acids cannot.

The reaction HNO₃ + NaOH → NaNO₃ + H₂O represents the neutralization of nitric acid by sodium hydroxide, resulting in the formation of sodium nitrate and water. Neutralization reactions are fundamental in chemistry, illustrating how acids and bases interact to form salts and water.

Nitric acid is used in the production of fertilizers, such as calcium nitrate (Ca(NO₃)₂) and ammonium nitrate (NH₄NO₃). These fertilizers are essential for promoting plant growth and increasing agricultural yields.

The molecular formula of nitric acid is HNO₃. This compound consists of one nitrogen atom, three oxygen atoms, and one hydrogen atom. Nitric acid is commonly used in laboratories and is known for its strong acidic properties.

Nitric acid is used as an oxidant in rocket fuel formulations. Its strong oxidizing properties enhance the combustion of fuel, allowing for efficient propulsion in rocket engines, which is crucial for space exploration.

Pure nitric acid is unstable and decomposes slightly even at room temperature and in the presence of sunlight. This decomposition can lead to the release of nitrogen dioxide, emphasizing the need for careful handling and storage of nitric acid.

Nitric acid reacts with carbonates to produce salt, water, and carbon dioxide. For example, the reaction with sodium carbonate yields sodium nitrate, water, and carbon dioxide gas. This is an important reaction in various applications, including laboratory preparations.

The freezing point of pure nitric acid is -42°C. This low freezing point indicates that nitric acid remains in a liquid state at much lower temperatures than water, which can influence its use in various applications.