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Hydrogen sulfate ions

Example The pK s for the first and second ionizations of sulfuric acid are —48 and 2 0 respectively Sulfuric acid (HOSO2OH) is a strong acid hydrogen sulfate ion (H0S020 ) is a weak acid... [Pg.44]

Step 3 in Figure 5 6 shows water as the base which ab stracts a proton from the car bocation Other Bronsted bases present in the reaction mixture that can function in the same way include tert butyl alcohol and hydrogen sulfate ion... [Pg.206]

Alkenes react with sulfuric acid to form alkyl hydrogen sulfates A proton and a hydrogen sulfate ion add to the double bond in accordance with Markovnikov s rule Alkenes that yield tertiary carboca tions on protonation tend to polymerize in concentrated sulfuric acid (Section 6 21)... [Pg.272]

Step 2 A proton is lost from the sp hybridized carbon of the intermediate to restore the aromaticity of the ring The species shown that abstracts the proton is a hydrogen sulfate ion formed by ionization of sulfunc acid... [Pg.479]

Ethanol Sulfuric acid Ethyloxonium ion Hydrogen sulfate ion... [Pg.637]

H2 SO4 (a q) + H2 O (/) HSO4 (q q) + H3 O (q q) However, the second hydrogen atom remains attached to HSO4. Thus, an aqueous solution of sulfuric acid contains H3 O and HSO4 ions. Like other weak acids, the hydrogen sulfate ion reacts quantitatively with hydroxide to give sulfate ion and water. [Pg.239]

Phosphoric acid, sulfuric acid, and the hydrogen sulfate ion are members of a group of acids known as oxoacids. An oxoacid has a central atom bonded to a variable number of oxygen atoms and OH groups. Except for the three oxoacids shown in Table (sulfuric acid, nitric acid, and perchloric acid), all of the oxoacids described in this textbook are weak acids. Chapter 17 describes in detail the chemistry of strong and weak acids, including carboxylic acids and oxoacids. [Pg.241]

In the second step, the carbocation reacts with a hydrogen sulfate ion to form an alkyl hydrogen sulfate. [Pg.329]

Carbocation Hydrogen sulfate ion Alkyl hydrogen sulfate... [Pg.329]

Sulfuric acid is a far stronger acid than the hydrogen sulfate ion, because much more energy is required to remove a proton from a negatively charged ion. The strength of a polyprotic acid decreases as the number of hydrogen atoms that have dissociated increases. [Pg.384]

Sulfuric acid is a strong diprotic acid. In dilute aqueous solution, ionization of the first hydrogen is complete and the Ka value for the hydrogen sulfate ion, HSO4 at 25°C is 1.2x10 2. It neutrahzes bases forming corresponding salts and water. Thus, with caustic soda, sodium sulfate is obtained on evaporation of the solution ... [Pg.901]

See other pages where Hydrogen sulfate ions is mentioned: [Pg.36]    [Pg.246]    [Pg.246]    [Pg.267]    [Pg.267]    [Pg.267]    [Pg.479]    [Pg.479]    [Pg.844]    [Pg.36]    [Pg.246]    [Pg.246]    [Pg.267]    [Pg.267]    [Pg.267]    [Pg.479]    [Pg.479]    [Pg.361]    [Pg.371]    [Pg.451]    [Pg.454]    [Pg.55]    [Pg.530]    [Pg.530]    [Pg.544]    [Pg.106]    [Pg.137]    [Pg.1113]    [Pg.354]    [Pg.417]    [Pg.97]    [Pg.1095]    [Pg.228]    [Pg.229]   
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Hydrogen sulfate

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