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Ammonium sulfamate, with the chemical formula NH4SO3, is a colorless crystalline solid with strong hygroscopicity. Its molecular weight is 116.12 and density is 1.54g/cm3. In dry conditions, the stability of ammonium sulfate suppliers is poor, while in high temperature and humid environments, their stability will be improved. This compound has a high solubility in water and is highly soluble in water. The aqueous solution is weakly acidic, with a pH value of 4-6 for a 10% aqueous solution. It is slightly soluble in ethanol, methanol, propylene glycol, and formamide, but easily soluble in water and liquid ammonia; It can absorb moisture from the air. It is a strong alkaline weak acid salt, and its hydrolysis reaction is NH4SO3+H2O ⇌ NH3 · H2O+HSO3-. Due to the existence of hydrolysis equilibrium, as the ambient temperature increases, the hydrolysis reaction will shift to the right, leading to an increase in the alkalinity of the solution. Thermal decomposition releases a large amount of inert gas, explodes upon heating, and self explodes in a hot acid solution. Burning produces toxic nitrogen oxide and sulfur oxide gases. In addition, under acidic conditions, ammonium sulfate undergoes a decomposition reaction, producing hydrogen sulfide gas, ammonia gas, and water.
Mainly used as chemical reagents, analytical reagents, and alkaline agents. In addition, it is also used in the production of other organic compounds and drugs. Due to its high alkalinity, it can be used to determine the concentration of certain acids or bases in titration experiments. At the same time, it is also a catalyst and solvent for some chemical reactions.
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Chemical Formula |
H6N2O3S |
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Exact Mass |
114 |
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Molecular Weight |
114 |
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m/z |
114 (100.0%), 116 (4.5%) |
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Elemental Analysis |
H, 5.30; N, 24.55; O, 42.06; S, 28.09 |
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Method 1 is a laboratory synthesis method that generates Ammonium sulfamate by reacting sodium sulfite and dilute sulfuric acid with ammonia water.
Step 1:
Prepare sodium sulfite solution. Add an appropriate amount of sodium sulfite (Na2SO3) to water, stir until dissolved, and obtain a sodium sulfite solution.
Step 2:
Prepare a dilute sulfuric acid solution. Add an appropriate amount of concentrated sulfuric acid (H2SO4) to water, dilute to the desired concentration, and obtain a dilute sulfuric acid solution.
Step 3:
Add dilute sulfuric acid to the sodium sulfite solution. Add a dilute sulfuric acid solution to a sodium sulfite solution and allow it to react to produce sodium sulfate (Na2SO4) and sulfite (H2SO3). The chemical equation for this reaction is:
Na2SO3 + H2SO4 → Na2SO4 + H2SO3.
Step 4:
Add ammonia water to the reaction solution. Add an appropriate amount of ammonia (NH3 · H2O) to the above reaction solution to achieve acid-base equilibrium in the solution, thereby generating ammonium sulfate. The chemical equation for this reaction is:
NH3 · H2O + H2SO3 → NH4SO3 + H2O.
Step 5:
Collect crystals. Let the above solution stand for a period of time to allow crystals to precipitate. Then filter to obtain crystals.
Step 6:
Wash and dry. Wash the obtained crystals with an appropriate amount of water to remove soluble impurities. Then dry to obtain the final product.
Method 2 is a laboratory synthesis method that generates ammonium sulfate through the reaction of potassium thiocyanate and ammonium nitrate.
Step 1:
Prepare potassium thiocyanate solution. Add an appropriate amount of potassium thiocyanate (KSCN) to water and stir until dissolved to obtain a potassium thiocyanate solution.
Step 2:
Prepare ammonium nitrate solution. Add an appropriate amount of ammonium nitrate (NH4NO3) to water, stir until dissolved, and obtain an ammonium nitrate solution.
Step 3:
Add ammonium nitrate solution to potassium thiocyanate solution. Add ammonium nitrate solution to potassium thiocyanate solution and allow it to react to produce ammonium sulfate and potassium thiocyanate. The chemical equation for this reaction is:
NH4NO3 + KSCN → NH4SO3 + KCN.
Step 4:
Collect crystals. Let the above solution stand for a period of time to allow ammonium sulfate crystals to precipitate. Then filter to obtain ammonium sulfonate crystals.
Step 5:
Wash and dry. Wash the obtained ammonium sulfate crystals with an appropriate amount of water to remove soluble impurities. Then dry to obtain the final product.
Ammonium sulfamate can be used as a reference reagent in acid-base titration in analytical chemistry and has multiple uses.
In acid-base titration experiments, it is usually necessary to use a stable substance as a reference reagent to help determine the endpoint of the titration reaction. As a strong base and weak acid salt, it has relatively high stability and purity, so it can be used as a reference reagent. The selection of reference reagents is crucial in acid-base titration experiments. An ideal reference reagent should have high purity, stability, and high sensitivity and reversibility in the reaction with the titrant. It meets these requirements and is therefore widely used in acid-base titration experiments.
In acid-base titration experiments, using ammonium sulfate as a reference reagent can help draw titration curves. The titration curve is a curve that describes the variation of pH value with the amount of titrant added during the titration reaction process. By using ammonium sulfate as a reference reagent, more accurate data can be obtained in the titration curve, leading to more accurate experimental results.
It can be used for the identification of acid-base ions. In acid-base titration experiments, using Ammonium sulfate as a reference reagent can assist in identifying acid-base ions. By observing the pH changes of the solution during the titration reaction and the reaction with ammonium sulfate, it is possible to preliminarily determine whether there are certain acid-base ions present in the tested solution.
Choosing the appropriate indicator is crucial for accurately determining the endpoint of acid-base titration. Ammonium aminosulfonate can be used as a complex for certain indicators to improve their sensitivity and accuracy. For example, when using phenolphthalein as an indicator, adding an appropriate amount of ammonium aminosulfonate can increase the color change range of phenolphthalein, making it easier to observe the titration endpoint.
The addition of ammonium aminosulfonate can also optimize acid-base titration methods. For example, when determining the concentration of strong acids or bases, using reverse titration can avoid errors that may occur during direct titration. At this point, the test solution can be reacted with excess ammonium aminosulfonate first, and then the remaining ammonium aminosulfonate can be titrated with a standard solution to indirectly determine the concentration of the test solution. This method has the advantages of easy operation and high accuracy.
Ammonium aminosulfonate can form stable complexes with various metal ions, making it suitable for the determination of metal ions. For example, when measuring the concentration of copper ions, spectrophotometry can be used. React the test solution with an appropriate amount of ammonium aminosulfonate to generate a blue complex. Then measure the absorbance of the complex, and based on the relationship between absorbance and copper ion concentration, the concentration of copper ions in the test solution can be calculated.
Ammonium aminosulfonate can also be used for the separation and determination of anions. For example, ion exchange method can be used to determine the concentration of sulfate ions. Pass the test solution through an ion exchange resin column to exchange sulfate ions with cations on the resin. Then wash the sulfate ions on the resin with an appropriate amount of ammonium aminosulfonate solution to generate ammonium sulfate. Finally, the concentration of ammonium sulfate is determined, and based on the relationship between concentration and sulfate ions, the concentration of sulfate ions in the test solution can be calculated.
In certain chemical reactions, ammonium aminosulfonate can be used as a catalyst. For example, in the preparation of certain organic compounds, adding an appropriate amount of ammonium aminosulfonate can increase the reaction rate and yield. This is because ammonium aminosulfonate can adsorb on the surface of reactants, reducing the activation energy of the reaction and promoting its progress. In acid-base titration experiments, using ammonium sulfate as a reference reagent can assist in studying reaction rates. By observing the changes in concentration of various substances during the titration reaction, parameters such as reaction rate constants can be calculated to understand the kinetic characteristics of the reaction.
Ammonium sulfamate can also be used in wastewater treatment. For example, when treating wastewater containing heavy metal ions, an appropriate amount of ammonium aminosulfonate can be added to form insoluble precipitates with heavy metal ions, thereby achieving the removal of heavy metal ions. In addition, ammonium aminosulfonate can also be used to adjust the pH value of wastewater to meet discharge standards.
adverse reaction
Ammonium Sulfamate, with the chemical formula H ₆ N ₂ O ∝ S (or written NH ₄ SO ∝ NH ₂), is a white crystalline solid with hygroscopicity and easy solubility in water. As a multifunctional compound, it has a wide range of applications in agriculture, industry, and scientific research fields. In agriculture, it is often used as a broad-spectrum herbicide to effectively control various weeds without damaging crops; In the industrial field, it plays an important role as a flame retardant, composting accelerator, and chemical synthesis intermediate. However, with the popularization of its application, the adverse reactions of Ammonium Sulfamate have gradually attracted attention.
Acute toxic reaction
Oral toxicity
The oral acute toxicity of Ammonium Sulfamate is low, but high-dose intake may still cause serious adverse reactions. Animal experiments showed that the oral dose of LD ₅₀ in rats was 2000 mg/kg, and in mice it was 3100 mg/kg, indicating that it is a low toxicity substance. However, although acute poisoning cases in humans are rare, excessive intake may lead to the following symptoms:
Gastrointestinal irritation: Nausea, vomiting, and diarrhea are common reactions that may be related to direct irritation of the gastrointestinal mucosa by ammonium thiosulfate. For example, in a certain case, a patient mistakenly ingested herbicides containing high concentrations of ammonium sulfonamide and experienced persistent vomiting and diarrhea, which needed to be relieved through gastric lavage and symptomatic treatment.
Systemic symptoms: High dose intake may lead to fatigue, dizziness, and even coma. This may be related to the inhibitory effect of sulfamethoxazole metabolites on the central nervous system in the body.
Skin contact toxicity
Ammonium thiosulfate is irritating to the skin. According to the Globally Harmonized System of Classification and Labelling of Chemicals (GHS), its skin irritation category is 2, indicating that long-term exposure to undiluted powders may lead to:
Dry and flaky skin: The hygroscopicity of ammonium sulfonamide may disrupt the skin barrier function, leading to the loss of moisture from the stratum corneum.
Contact dermatitis: Sensitive individuals may experience redness, itching, or blisters. For example, a certain agricultural worker was diagnosed with contact dermatitis through patch testing due to diffuse erythema and flaking on his hands caused by long-term exposure to ammonium thiosulfate powder.
Eye contact toxicity
Ammonium thiosulfate powder or solution entering the eyes may cause serious irritation. In the GHS classification, its eye irritation category is 2B, indicating that it may cause:
Conjunctival congestion: After eye contact, the conjunctival blood vessels dilate, resulting in redness and swelling.
Corneal injury: High concentration ammonium thiosulfate solution may damage corneal epithelial cells, leading to blurred vision or pain. For example, a laboratory staff member accidentally splashed the solution into the eyes while operating ammonium thiosulfate without wearing goggles, resulting in corneal epithelial detachment. Emergency flushing and medical attention are required.
Inhalation toxicity
Inhalation of ammonium thiosulfate dust may cause respiratory irritation. In the GHS classification, its inhalation toxicity category is 3, indicating that high concentration exposure may lead to:
Upper respiratory tract irritation: Coughing and burning sensation in the throat are common symptoms, which may be related to direct irritation of mucous membranes by dust.
Asthma like reactions: Sensitive individuals may experience wheezing and difficulty breathing, which require the use of bronchodilators for relief.
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