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- Weak_base abstract "In chemistry, a weak base is a chemical base that does not ionize fully in an aqueous solution. As Brønsted–Lowry bases are proton acceptors, a weak base may also be defined as a chemical base in which protonation is incomplete. This results in a relatively low pH compared to strong bases. Bases range from a pH of greater than 7 (7 is neutral, like pure water) to 14 (though some bases are greater than 14). pH has the formula:Since bases are proton acceptors, the base receives a hydrogen ion from water, H2O, and the remaining H+ concentration in the solution determines pH. Weak bases will have a higher H+ concentration because they are less completely protonated than stronger bases and, therefore, more hydrogen ions remain in the solution. If you plug in a higher H+ concentration into the formula, a low pH results. However, pH of bases is usually calculated using the OH- concentration to find the pOH first. This is done because the H+ concentration is not a part of the reaction, while the OH- concentration is.By multiplying a conjugate acid (such as NH4+) and a conjugate base (such as NH3) the following is given:Since then, By taking logarithms of both sides of the equation, the following is reached:Finally, multiplying throughout the equation by -1, the equation turns into:After acquiring pOH from the previous pOH formula, pH can be calculated using the formula pH = pKw - pOH where pKw = 14.00.Weak bases exist in chemical equilibrium much in the same way as weak acids do, with a base dissociation constant (Kb) indicating the strength of the base. For example, when ammonia is put in water, the following equilibrium is set up:Bases that have a large Kb will ionize more completely and are thus stronger bases. As stated above, pH of the solution depends on the H+ concentration, which is related to the OH- concentration by the self-ionization constant (Kw = 1.0x10−14). A strong base has a lower H+ concentration because they are fully protonated and less hydrogen ions remain in the solution. A lower H+ concentration also means a higher OH- concentration and therefore, a larger Kb.NaOH (s) (sodium hydroxide) is a stronger base than (CH3CH2)2NH (l) (diethylamine) which is a stronger base than NH3 (g) (ammonia). As the bases get weaker, the smaller the Kb values become.".
- Weak_base wikiPageExternalLink lect16.htm.
- Weak_base wikiPageExternalLink bases.html.
- Weak_base wikiPageExternalLink p01154.htm.
- Weak_base wikiPageID "487315".
- Weak_base wikiPageRevisionID "605657409".
- Weak_base hasPhotoCollection Weak_base.
- Weak_base subject Category:Bases.
- Weak_base type Abstraction100002137.
- Weak_base type Bases.
- Weak_base type Footing113790912.
- Weak_base type Foundation113790712.
- Weak_base type Relation100031921.
- Weak_base comment "In chemistry, a weak base is a chemical base that does not ionize fully in an aqueous solution. As Brønsted–Lowry bases are proton acceptors, a weak base may also be defined as a chemical base in which protonation is incomplete. This results in a relatively low pH compared to strong bases. Bases range from a pH of greater than 7 (7 is neutral, like pure water) to 14 (though some bases are greater than 14).".
- Weak_base label "Base debole".
- Weak_base label "Base faible".
- Weak_base label "Base fraca".
- Weak_base label "Weak base".
- Weak_base label "Zwakke base".
- Weak_base label "قلوي ضعيف".
- Weak_base label "弱碱".
- Weak_base sameAs Base_faible.
- Weak_base sameAs Base_debole.
- Weak_base sameAs Zwakke_base.
- Weak_base sameAs Base_fraca.
- Weak_base sameAs m.02gd8t.
- Weak_base sameAs Q2155237.
- Weak_base sameAs Q2155237.
- Weak_base sameAs Weak_base.
- Weak_base wasDerivedFrom Weak_base?oldid=605657409.
- Weak_base isPrimaryTopicOf Weak_base.