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Comparison of the physical properties of NH 3 with those of water shows NH 3 has the lower melting point, boiling point, density, viscosity, dielectric constant and electrical conductivity. These differences are attributed at least in part to the weaker hydrogen bonding in NH 3.
At 15.6 °C (60.1 °F), the density of a saturated solution is 0.88 g/ml; it contains 35.6% ammonia by mass, 308 grams of ammonia per litre of solution, and has a molarity of approximately 18 mol/L. At higher temperatures, the molarity of the saturated solution decreases and the density increases. [ 8 ]
[NH 4] + + B − → HB + NH 3. Thus, the treatment of concentrated solutions of ammonium salts with a strong base gives ammonia. When ammonia is dissolved in water, a tiny amount of it converts to ammonium ions: H 2 O + NH 3 ⇌ OH − + [NH 4] + The degree to which ammonia forms the ammonium ion depends on the pH of the solution. If the pH is ...
For example, water has a molar mass of 18.0153(3) g/mol, but individual water molecules have molecular masses which range between 18.010 564 6863(15) Da (1 H 2 16 O) and 22.027 7364(9) Da (2 H 2 18 O). Atomic and molecular masses are usually reported in daltons, which is defined in terms of the mass of the isotope 12 C (carbon-12).
These properties include its relatively high melting and boiling point temperatures: more energy is required to break the hydrogen bonds between water molecules. In contrast, hydrogen sulfide (H 2 S), has much weaker hydrogen bonding due to sulfur's lower electronegativity. H 2 S is a gas at room temperature, despite hydrogen sulfide having ...
Obsolete terms for molar mass include gram atomic mass for the mass, in grams, of one mole of atoms of an element, and gram molecular mass for the mass, in grams, of one mole of molecules of a compound. The gram-atom is a former term for a mole of atoms, and gram-molecule for a mole of molecules. [7] Molecular weight (M.W.) (for molecular ...
2 NH 3 + H 2 SO 4 → (NH 4) 2 SO 4. A mixture of ammonia gas and water vapor is introduced into a reactor that contains a saturated solution of ammonium sulfate and about 2% to 4% of free sulfuric acid at 60 °C. Concentrated sulfuric acid is added to keep the solution acidic, and to retain its level of free acid.
For propane (C 3 H 8) reacting with oxygen gas (O 2), the balanced chemical equation is: C 3 H 8 + 5 O 2 → 3 CO 2 + 4 H 2 O. The mass of water formed if 120 g of propane (C 3 H 8) is burned in excess oxygen is then =