Ammonia in liquefied form is neutral or basic

• العربية • تۆرکجه • বাংলা • Беларуская • Català • Dansk • Deutsch • Eesti • Español • Esperanto • فارسی • Français • Frysk • 한국어 • हिन्दी • Ido • Bahasa Indonesia • Italiano • Қазақша • Magyar • മലയാളം • Nederlands • 日本語 • Norsk bokmål • Oʻzbekcha / ўзбекча • پنجابی • Polski • Português • Română • Русский • Simple English • Slovenčina • Slovenščina • Српски / srpski • Srpskohrvatski / српскохрватски • Svenska • తెలుగు • Türkçe • Українська • Tiếng Việt • 粵語 • 中文 Chemical compound Ammonia solution, also known as ammonia water, ammonium hydroxide, ammoniacal liquor, ammonia liquor, aqua ammonia, aqueous ammonia, or (inaccurately) ammonia, is a solution of 3(aq). Although the name ammonium hydroxide suggests an alkali with [NH + 4][OH − ], it is actually impossible to isolate samples of NH 4OH. The ions NH + 4 and OH − do not account for a significant fraction of the total amount of ammonia except in extremely dilute solutions. Basicity of ammonia in water [ ] In aqueous solution, ammonia NH 3 + H 2O ↽ − ⇀ NH + 4 + OH −. In a 1 NH + 4]= 0.0042M, [OH −]= 0.0042M, [NH 3]= 0.9958M, and pH= 14+log 10[OH −]= 11.62. The K b = [ NH + 4][OH −] / [NH 3] = 1.77 ×10 −5. Saturated solutions [ ] Like other gases, ammonia exhibits decreasing solubility in solvent liquids as the temperature of the solvent increases. Ammonia solutions decrease in density as the concentration of dissolved ammonia increases. At 15.6°C (60.1°F), the density of a saturated solution is 0.88g/ml and contains 35....

Ammonia - NH 3 What is Ammonia? Ammonia is a colorless gas with a chemical formula NH 3. It consists of hydrogen and nitrogen. In its aqueous form, it is called ammonium hydroxide. This inorganic compound has a pungent smell. In its concentrated form, it is dangerous and caustic. The NH 3 chemical name is ammonia. Table of Contents • • • • • Ammonia is lighter than air with a density of 0.769  kg/m 3 at STP. It is widely used as a fertilizer. It is also used in the manufacturing of explosives such as nitrocellulose and TNT. Also, it is used in the production of With the formula NH3, ammonia is a nitrogen and hydrogen inorganic chemical compound. Ammonia, the simplest pnictogen hydride and a stable binary hydride is a colourless gas with a strong, pungent odour. It contributes considerably to the nutritional demands of terrestrial creatures by serving as a precursor to 45% of the world’s food and fertilisers. Biologically, it is a common nitrogenous waste, especially among aquatic animals. Fertilizers in a variety of compositions, including urea and diammonium phosphate, are made with around 70% of the ammonia produced. Additionally, pure ammonia is sprayed straight onto the ground. Ammonia Structure – NH 3 Ammonia Structure Properties of Ammonia – NH 3 NH 3 Ammonia Molecular Weight/ Molar Mass 17.031 g/mol Density 0.73 kg/m³ Boiling Point -33.34 °C Melting Point −77.73 °C Ammonia is known to behave as a weak base since it combines with many acids to form salts. For e...

\( \newcommand\) • • • • • • • • • Objectives After completing this section, you should be able to • account for the basicity and nucleophilicity of amines. • explain why amines are more basic than amides, and better nucleophiles. • describe how an amine can be extracted from a mixture that also contains neutral compounds illustrating the reactions which take place with appropriate equations. • explain why primary and secondary (but not tertiary) amines may be regarded as very weak acids, and illustrate the synthetic usefulness of the strong bases that can be formed from these weak acids. Study Notes The lone pair of electrons on the nitrogen atom of amines makes these compounds not only basic, but also good nucleophiles. Indeed, we have seen in past chapters that amines react with electrophiles in several polar reactions (see for example the nucleophilic addition of amines in the formation of imines and enamines in Section 19.8). The ammonium ions of most simple aliphatic amines have a p K a of about 10 or 11. However, these simple amines are all more basic (i.e., have a higher p K a) than ammonia. Why? Remember that, relative to hydrogen, alkyl groups are electron releasing, and that the presence of an electron‑releasing group stabilizes ions carrying a positive charge. Thus, the free energy difference between an alkylamine and an alkylammonium ion is less than the free energy difference between ammonia and an ammonium ion; consequently, an alkylamine is more easily prot...

\( \newcommand\) • • • • • • • • • • • • • • • • • • Auto-Ionization of Water Because of its amphoteric nature (i.e., acts as both an acid or a base), water does not always remain as \(H_2O\) molecules. In fact, two water molecules react to form \[ \ce\] As expected for any equilibrium, the reaction can be shifted to the reactants or products: • If an acid (\(H^+\)) is added to the water, the equilibrium shifts to the left and the \(OH^-\) ion concentration decreases • If base ( \(OH^-\)) is added to water, the equilibrium shifts to left and the \(H^+\) concentration decreases. pH and pOH Because the constant of water, K w is \(1.0 \times 10^ is correct only at room temperature since changing the temperature will change \(K_w\). The pH scale is logarithmic, meaning that an increase or decrease of an integer value changes the concentration by a tenfold. For example, a pH of 3 is ten times more acidic than a pH of 4. Likewise, a pH of 3 is one hundred times more acidic than a pH of 5. Similarly a pH of 11 is ten times more basic than a pH of 10. Properties of the pH Scale From the simple definition of pH in Equation \ref\). The Effective Range of the pH Scale It is common that the pH scale is argued to range from 0-14 or perhaps 1-14, but neither is correct. The pH range does not have an upper nor lower bound, since as defined above, the pH is an indication of concentration of H +. For example, at a pH of zero the hydronium ion concentration is one molar, while at pH 14 the ...

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Even if you’ve never set foot in a chemistry lab, chances are you know a thing or two about acids and bases. For instance, have you drunk orange juice or cola? If so, you know some common acidic solutions. And if you’ve ever used baking soda, or even egg whites, in your cooking, then you’re familiar with some bases as well 1 ^1 1 start superscript, 1, end superscript . H 2 \text (aq) start text, left parenthesis, a, q, right parenthesis, end text As shown in the equation, dissociation makes equal numbers of hydrogen (H + ^+ + start superscript, plus, end superscript ) ions and hydroxide (OH − ^- − start superscript, minus, end superscript ) ions. While the hydroxide ions can float around in solution as hydroxide ions, the hydrogen ions are transferred directly to a neighboring water molecule to form hydronium ions (H 3 _3 3 ​ start subscript, 3, end subscript O + ^+ + start superscript, plus, end superscript ). So, there aren't really H + ^+ + start superscript, plus, end superscript ions floating around freely in water. However, scientists still refer to hydrogen ions and their concentration as if they were free-floating, not in hydronium form – this is just a shorthand we use by convention. Is that a lot or a little? Although the number of hydrogen ions in a liter of pure water is large on the scale of what we usually think about (in the quadrillions), the number of total water molecules in a liter – dissociated and undissociated – is about 33,460,000,000,000,000,000,000...