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  2. Conjugate (acid-base theory) - Wikipedia

    en.wikipedia.org/wiki/Conjugate_(acid-base_theory)

    The conjugate acid in the after side of an equation gains a hydrogen ion, so in the before side of the equation the compound that has one less hydrogen ion of the conjugate acid is the base. The conjugate base in the after side of the equation lost a hydrogen ion, so in the before side of the equation, the compound that has one more hydrogen ...

  3. Sulfuric acid - Wikipedia

    en.wikipedia.org/wiki/Sulfuric_acid

    Sulfuric acid (American spelling and the preferred IUPAC name) or sulphuric acid (Commonwealth spelling), known in antiquity as oil of vitriol, is a mineral acid composed of the elements sulfur, oxygen, and hydrogen, with the molecular formula H 2 SO 4. It is a colorless, odorless, and viscous liquid that is miscible with water. [7] Structure ...

  4. Acid strength - Wikipedia

    en.wikipedia.org/wiki/Acid_strength

    Such a statement is incorrect. For example, acetic acid is a weak acid which has a = 1.75 x 10 −5. Its conjugate base is the acetate ion with K b = 10 −14 /K a = 5.7 x 10 −10 (from the relationship K a × K b = 10 −14), which certainly does not correspond to a strong base

  5. Sulfurous acid - Wikipedia

    en.wikipedia.org/wiki/Sulfurous_acid

    Sulfuric(IV) acid (United Kingdom spelling: sulphuric(IV) acid), also known as sulfurous (UK: sulphurous) acid and thionic acid, [citation needed] is the chemical compound with the formula H 2 SO 3. Raman spectra of solutions of sulfur dioxide in water show only signals due to the SO 2 molecule and the bisulfite ion, HSO − 3. [2]

  6. Gallium(III) sulfate - Wikipedia

    en.wikipedia.org/wiki/Gallium(III)_sulfate

    Gallium(III) sulfate refers to the chemical compound, a salt, with the formula Ga 2 (SO 4) 3, or its hydrates Ga 2 (SO 4) 3 ·xH 2 O. Gallium metal dissolves in sulfuric acid to form solutions containing [Ga(OH 2) 6] 3+ and SO 4 2− ions. The octadecahydrate Ga 2 (SO 4) 3 ·18H 2 O crystallises from these solutions at room temperature.

  7. Sulfur oxoacid - Wikipedia

    en.wikipedia.org/wiki/Sulfur_oxoacid

    Polysulfuric acids including disulfuric acid (pyrosulfuric acid) H 2 SO 4 ·nSO 3 +6 Disulfate (commonly known as pyrosulfate), S 2 O 2− 7 and trisulfate, S 3 O 2− 10: Pure disulfuric acid melts at 36 °C. Present in fuming sulfuric acid, oleum. Examples known for n = 1 and n = 2. Peroxymonosulfuric acid: H 2 SO 5 +6 Peroxomonosulfate, OOSO ...

  8. Organosulfate - Wikipedia

    en.wikipedia.org/wiki/Organosulfate

    A less common family of organosulfates have the formula RO-SO 2-OR'. They are prepared from sulfuric acid and the alcohol. The main examples are diethyl sulfate and dimethyl sulfate, colourless liquids that are used as reagents in organic synthesis. These compounds are potentially dangerous alkylating agents. Dialkylsulfates do not occur in nature.

  9. Bunsen reaction - Wikipedia

    en.wikipedia.org/wiki/Bunsen_Reaction

    The Bunsen reaction is a chemical reaction that describes water, sulfur dioxide, and iodine reacting to form sulfuric acid and hydrogen iodide: 2H 2 O + SO 2 + I 2 → H 2 SO 4 + 2HI This reaction is the first step in the sulfur-iodine cycle to produce hydrogen .