Sulfur Daily Question, March 28------5 rewards for participation, 10 rewards for correct answers

Main chemical properties: 1. NH₃ (volatile) produces white smoke when it comes into contact with HCl (volatile) gas, and it can react with chlorine gas. 2. Ammonium hydroxide (ammonia monohydrate, NH₃·H₂O) can corrode many metals; therefore, if ammonia hydroxide is stored in iron tanks, those tanks should be coated with asphalt on the inside. 3. The catalytic oxidation of ammonia is an exothermic reaction, with NO as the product. This reaction is important for the industrial production of nitric acid, and ammonia can also be oxidized to N₂. 4. NH₃ can turn moist red litmus paper blue. Ionization equation: In water, it produces a small amount of hydroxide ions, giving it weak basic properties. 5. Ammonia reacts with acids to form ammonium salts: NH₃ + HCl = NH₄Cl. In English, ammonia is sometimes referred to as “anhydrous ammonia” to distinguish it from ammonia hydroxide, which has a similar name in English. In Chinese, few people confuse ammonia gas with ammonia hydroxide. Ammonia gas dissolves in water to form ammonia hydroxide, and the main component of ammonia hydroxide is ammonia monohydrate; however, ammonia monohydrate is not synonymous with ammonia hydroxide. The alkaline nature of ammonia hydroxide arises from the ionization of ammonia monohydrate in water, producing hydroxide ions. Commercially available ammonia hydroxide has a concentration of 25%-28%. NH₃·H₂O ⇌ NH₄⁺ + OH⁻; its properties are completely different from those of ammonia gas. The concentration of dilute ammonia used in laboratories is generally between 1M and 2M. The density of a saturated aqueous solution of ammonia (approximately 18M) is 0.880 g/cm³, so it can be referred to as “0.880 ammonia”. Physical properties of ammonia: (1) It is a gas with a pungent odor. Ammonia irritates the eyes, nose, and throat. Inhaling large amounts of ammonia can cause short-term nasal congestion and a feeling of suffocation. Contact with the eyes can cause tearing; caution is necessary when handling it. If excessive exposure to ammonia leads to illness, it is important to inhale fresh air and water vapor immediately, and rinse the eyes thoroughly with water. (2) It has a low density. The density of ammonia gas is 0.771 g/L under standard conditions. (3) It has a relatively high boiling point. Ammonia easily liquefies; at normal pressure, cooling it to -33.5°C or applying pressure of 700KPa to 800KPa at room temperature will cause gaseous ammonia to turn into a colorless liquid, with a large amount of heat being released in the process. When liquid ammonia vaporizes, it absorbs a large amount of heat, causing the temperature of surrounding substances to drop sharply. Therefore, ammonia is often used as a refrigerant. Some old-fashioned ice pops were made using ammonia gas. (4) It is highly soluble in water. Ammonia dissolves very easily in water; at room temperature and pressure, 1 volume of water can dissolve about 700 volumes of ammonia.

With the molecular formula NH₃, it is a colorless gas with a strong, pungent odor. It is highly soluble in water; at normal temperature and pressure, 1 volume of water can dissolve 700 volumes of ammonia, and its aqueous solution is also known as ammonia water. It can be turned into a liquid by cooling and applying pressure; liquid ammonia is a type of refrigerant. Ammonia is also an important raw material for producing *ao acid, fertilizers, and **.

Physical properties: It is usually colorless with a strong pungent odor; it can be liquefied under pressure at room temperature. Its critical temperature is 132.9°C and its critical pressure is 11.38 MPa; it liquefies when cooled to –33.35°C at atmospheric pressure. Liquid ammonia is highly volatile; it absorbs a large amount of heat during vaporization, and it solidifies into colorless crystals at –77.75°C. Ammonia is highly soluble in water and releases heat. An aqueous solution of ammonia is called ammonia water; it is weakly alkaline and volatile. The auto-ignition temperature is 630°C, and it can explode when exposed to fire in air. The explosion limit in air at normal temperature and pressure is 16% to 28% (by volume). Chemical properties: 1. NH3 (volatile) produces white smoke when it comes into contact with HCl (volatile) gas, and it can react with chlorine gas. 　　2. Ammonia water (also known as ammonium hydroxide, NH3·H2O) can corrode many metals; generally, if ammonia water is stored in iron tanks, those tanks should be coated with asphalt on the inside. 　　3. The catalytic oxidation of ammonia is an exothermic reaction; the product is NO, and it is an important reaction in the industrial production of nitric acid. NH3 can also be oxidized to N2. 　　4. NH3 can turn moist red litmus paper blue. It produces a small amount of hydroxide ions in water, giving it a weakly alkaline nature. 5. Ammonia reacts with acids to form ammonium salts

Physical properties: A colorless gas with a pungent odor; it is lighter than air, highly soluble in water, and easily liquefied. Chemical properties: Reducing property: 4NH3 + 5O2 → 4NO + 6H2O; 4NH3 + 3O2 (pure) → 2N2 + 6H2O; 8NH3 + 3Cl2 → 6NH4Cl + N2. Basic properties: NH3 + HCl → NH4Cl (white smoke); NH3 + HNO3 → NH4NO3; 2NH3 + H2SO4 → (NH4)2SO4; NH3 + H3PO4 → NH4H2PO4; NH3 + H2O + CO2 → NH4HCO3. The aqueous solution of ammonia is called ammonium hydroxide; it is a soluble weak base with the typical properties of bases. Uses: It is widely used in the production of urea, ammonium-based nitrogen fertilizers, and amino acids. Ammonia can also be used as a refrigerant

Chemical properties: 1. Combustion and oxidation: Ammonia can burn in pure oxygen, with the products being components of air; it does not pollute the environment, hence it holds certain potential for utilization. 2. Reaction with water: Ammonia dissolves very easily in water; when it does so, it reacts with water to form ammonium hydroxide, commonly known as ammonia water. The concentration of ammonia water available on the market is between 25% and 28%. Ammonia water is weakly basic because of such ionization in water. 3. Reaction with metals: NH3 can also form complexes with metal ions such as Ag and Cu. 4. Reaction with acids: Ammonia can react with acids to form ammonium salts; these reactions can be used to detect the presence of ammonia gas. 5. Redox reactions: The catalytic oxidation of ammonia is an exothermic reaction; the product is NO, and it is an important reaction in the industrial production of nitric acid. Physical properties ； (1) Gases with an irritating odor: Ammonia irritates the eyes, nose, throat, and other parts of the body. Inhaling large amounts of ammonia can cause short-term nasal congestion and a feeling of suffocation; contact with the eyes can lead to tearing, so caution is needed when handling it. If symptoms occur due to accidental exposure to excessive ammonia, it is necessary to inhale fresh air and water promptly, and rinse the eyes with plenty of water. (2) Low density: The density of ammonia is 0.771 g/L under standard conditions. (3) High boiling point: Ammonia liquefies very easily; by cooling it to -33.5°C at atmospheric pressure, or by increasing the pressure to 700–800 KPa at room temperature, gaseous ammonia turns into a colorless liquid, with a large amount of heat being released in the process. When liquid ammonia vaporizes, it absorbs a large amount of heat, causing the temperature of the surrounding substances to drop sharply; therefore, ammonia is often used as a refrigerant. Some old-fashioned ice pops were made using ammonia. (4) Solubility in water: Ammonia is highly soluble in water; at normal temperature and pressure, 1 volume of water can dissolve approximately 700 volumes of ammonia.

What are the basic properties of ammonia? Chemical properties: 1. Combustion and oxidation: Ammonia can burn in pure oxygen, with the products being components of air; it does not pollute the environment, hence it holds certain potential for utilization. 2. Reaction with water: Ammonia dissolves very easily in water; when it does so, it reacts with water to form ammonium hydroxide, commonly known as ammonia water. The concentration of ammonia water available on the market is between 25% and 28%. Ammonia water is weakly basic because of such ionization in water. 3. Reaction with metals: NH3 can also form complexes with metal ions such as Ag and Cu. 4. Reaction with acids: Ammonia can react with acids to form ammonium salts; these reactions can be used to detect the presence of ammonia gas. 5. Redox reactions: The catalytic oxidation of ammonia is an exothermic reaction; the product is NO, and it is an important reaction in the industrial production of nitric acid. Physical properties ； (1) Gases with an irritating odor: Ammonia irritates the eyes, nose, throat, and other parts of the body. Inhaling large amounts of ammonia can cause short-term nasal congestion and a feeling of suffocation; contact with the eyes can lead to tearing, so caution is needed when handling it. If symptoms occur due to accidental exposure to excessive ammonia, it is necessary to inhale fresh air and water promptly, and rinse the eyes with plenty of water. (2) Low density: The density of ammonia is 0.771 g/L under standard conditions. (3) High boiling point: Ammonia liquefies very easily; by cooling it to -33.5°C at atmospheric pressure, or by increasing the pressure to 700–800 KPa at room temperature, gaseous ammonia turns into a colorless liquid, with a large amount of heat being released in the process. When liquid ammonia vaporizes, it absorbs a large amount of heat, causing the temperature of the surrounding substances to drop sharply; therefore, ammonia is often used as a refrigerant. Some old-fashioned ice pops were made using ammonia. (4) Solubility in water: Ammonia is highly soluble in water; at normal temperature and pressure, 1 volume of water can dissolve approximately 700 volumes of ammonia.

1. NH3 (volatile) produces white smoke when it comes into contact with HCl (volatile) gas, and it can react with chlorine gas. 2. Ammonia water (ammonium hydroxide, NH3·H2O) can corrode many metals; generally, if ammonia water is stored in iron tanks, those tanks should be coated with asphalt on the inside. 3. The catalytic oxidation of ammonia is an exothermic reaction; the product is NO, and it is an important reaction in the industrial production of nitric acid. NH3 can also be oxidized to N2. 4. NH3 can turn moist red litmus paper blue. The ionization equation produces a small amount of hydroxide ions in water, giving it weak basic properties. 5. Ammonia reacts with acids to form ammonium salts: NH3 + HCl = NH4Cl. Ammonia is sometimes referred to in English as anhydrous ammonia, in order to distinguish it from ammonia water, which has a similar name in English. In Chinese, few people confuse ammonia gas with ammonia solution. Ammonium hydroxide, also known as ammonia water, is an aqueous solution of ammonia; such solutions are basic: NH3 + H2O ⇌ NH4+ + OH-. Its properties are completely different from those of gaseous ammonia. The concentration of dilute ammonia solution in the laboratory is generally between 1M and 2M. The density of a saturated aqueous solution of ammonia (about 18 M) is 0.880 g/cm3, so it can be referred to as 0.880 Ammonia.

Main chemical properties: 1. NH₃ (volatile) produces white smoke when it comes into contact with HCl (volatile) gas, and it can react with chlorine gas. 2. Ammonia water (ammonium hydroxide, NH₃·H₂O) can corrode many metals; therefore, if ammonia water is stored in iron tanks, those tanks should be coated with asphalt on the inside. 3. The catalytic oxidation of ammonia is an exothermic reaction, with NO as the product – this reaction is important for the industrial production of nitric acid. NH₃ can also be oxidized to N₂. 4. NH₃ can turn moist red litmus paper blue. Ionization equation: In water, it produces a small amount of hydroxide ions, giving it weak basic properties. 5. Ammonia reacts with acids to form ammonium salts: NH₃ + HCl = NH₄Cl.

Physical properties of ammonia: (1) It is a gas with a pungent odor. Ammonia irritates the eyes, nose, and throat. Inhaling large amounts of ammonia can cause short-term nasal congestion and a feeling of suffocation. Contact with the eyes can lead to tearing; caution is necessary when handling it. If excessive exposure to ammonia causes illness, it is important to inhale fresh air and steam immediately, and rinse the eyes thoroughly with water. (2) Low density: The density of ammonia gas is 0.771 g/L under standard conditions. (3) High boiling point: Ammonia easily liquefies. At normal pressure, cooling it to -33.5°C, or under pressure of 700–800 KPa at room temperature, gaseous ammonia turns into a colorless liquid, releasing a large amount of heat in the process. When liquid ammonia vaporizes, it absorbs a large amount of heat, causing the temperature of surrounding substances to drop sharply. This property makes ammonia useful as a refrigerant. Some old-fashioned ice pops were made using ammonia gas. (4) Highly soluble in water: Ammonia is highly soluble in water. Under normal temperature and pressure, 1 volume of water can dissolve approximately 700 volumes of ammonia.

Physical properties of ammonia: (1) It is a gas with an irritating odor; ammonia can irritate the eyes, nose, throat, and other parts of the human body, so caution should be exercised when coming into contact with it. If symptoms occur due to accidental exposure to excessive ammonia, it is necessary to inhale fresh air and steam promptly, and rinse the eyes with plenty of water. (2) Low density: the density of ammonia is 0.771 g/L under standard conditions. (3) High boiling point: ammonia can be easily liquefied; by cooling it to -33.5°C at atmospheric pressure, or by increasing the pressure to 700–800 KPa at room temperature, gaseous ammonia turns into a colorless liquid, with a large amount of heat being released in the process. When liquid ammonia vaporizes, it absorbs a large amount of heat, causing the temperature of the surrounding substances to drop sharply; therefore, ammonia is often used as a refrigerant. (4) It is highly soluble in water; ammonia is extremely soluble in water. At normal temperature and pressure, 1 volume of water can dissolve approximately 700 volumes of ammonia. Basic uses: NH3 is used to produce ammonia water, liquid ammonia, nitrogen-based fertilizers (such as urea and ammonium carbonate), HNO3, ammonium salts, and soda ash. It is widely applied in the chemical industry, light industry, fertilizer production, pharmaceuticals, synthetic fibers, plastics, dyes, refrigerants, and more. Effects of different ammonia concentrations on humans: Concentration/(mg/m3), Exposure time/min, Degree of harm, Harm classification: 0.7. Ammonia has a strong odor; it is primarily present in dyes in furniture, evaporates relatively quickly, and poses little hazard.

With the molecular formula NH₃, it is a colorless gas with a strong, pungent odor. It is highly soluble in water; at normal temperature and pressure, 1 volume of water can dissolve 700 volumes of ammonia, and its aqueous solution is also known as ammonia water. It can be turned into a liquid by cooling and applying pressure; liquid ammonia is a type of refrigerant. Ammonia is also an important raw material for producing *ao acid, fertilizers, and **.