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acid: accepts lone pair electrons
bases:donates lone pair electrons
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∙ 13y ago
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Whose definition of acids and bases emphasizes the role of proton?
Bronsted and Lowry
What are the three Acid Base Theories?
Arrhenius, Bronsted-Lowry, and Lewis theories of acids and bases
What of the three acid definitions is the broadest?
Lewis theory gives the most general argumentation on acids and bases as at the present time.
How does nitric acid act as a base?
Acids or bases change character based on the solution in which they exist. For instance, HCl is a strong acid in water, but is a weak acid when dissolved in glacial acetic acid. This has to do with the proton affinity of the respective acids and bases. So, nitric acid may act as a base when placed in a solvent that has a lower proton affinity, i.e., the nitric acid will accept the proton as a Bronsted-Lowry base. I'm not as familiar with Lewis acids and bases, but Lewis bases donate electron pairs, and Lewis acids accept them. I'm sure there is a circumstance in which nitric acid will donate an electron pair to a Lewis acid.
Who is given credit for giving a broader definition of acids and bases?
The most inclusive definition of acids and basis is the Lewis definition, named after Gilbert N. Lewis. A Lewis acid and base is an electron-pair acceptor and electron-pair donator, respectively.
Why do you think bases are often described the opposite of acids?
1) Bronsted-Lowry acids are proton donors. Bronsted-Lowry bases are proton acceptors. 2) Lewis acids are electron acceptors. Lewis bases are electron donors.
Why do you think bases are often described as the opposite of?
1) Bronsted-Lowry acids are proton donors. Bronsted-Lowry bases are proton acceptors. 2) Lewis acids are electron acceptors. Lewis bases are electron donors.
How do you define salts?
Salts are the products of reactions between bases and acids.
Why do you think bases are often described as the opposites of acids'?
1) Bronsted-Lowry acids are proton donors. Bronsted-Lowry bases are proton acceptors. 2) Lewis acids are electron acceptors. Lewis bases are electron donors.
Whose definition of acids and bases emphasizes the role of proton?
Bronsted and Lowry
What are the three Acid Base Theories?
Arrhenius, Bronsted-Lowry, and Lewis theories of acids and bases
What of the three acid definitions is the broadest?
Lewis theory gives the most general argumentation on acids and bases as at the present time.
How does nitric acid act as a base?
Acids or bases change character based on the solution in which they exist. For instance, HCl is a strong acid in water, but is a weak acid when dissolved in glacial acetic acid. This has to do with the proton affinity of the respective acids and bases. So, nitric acid may act as a base when placed in a solvent that has a lower proton affinity, i.e., the nitric acid will accept the proton as a Bronsted-Lowry base. I'm not as familiar with Lewis acids and bases, but Lewis bases donate electron pairs, and Lewis acids accept them. I'm sure there is a circumstance in which nitric acid will donate an electron pair to a Lewis acid.
Who is given credit for giving a broader definition of acids and bases?
The most inclusive definition of acids and basis is the Lewis definition, named after Gilbert N. Lewis. A Lewis acid and base is an electron-pair acceptor and electron-pair donator, respectively.
Why are bases described as opposites to acids?
Bases have the ion OH- and acids the ion H+; the reaction between acids and bases is called neutralization and the product is a salt. Basic solutions have a pH over 7 and acidic solutions have a pH under 7.
Why are bases sometimes describes as the opposite of acids?
Bases are the opposite of acids due to the fact they are a hydrogen ion acceptor and an acid is a hydrogen ion donor. In the many definitions of bases and acids, bases do the opposite of what acids do. -- In the Lewis definition, acids are electron pair acceptors while bases are electron pair donors. -- In the Bronsted-Lowry definition, acids are substances that donate protons while bases are substances that accepts protons. -- In practicality, acids lower the pH of a solution and bases increase the pH of a solution.
How do you know if a molecule is a base or an acid?
In brief: It could be done by measuring its pH level. Descriptive: There are a few ways to define an acid or a base: Arrhenius Defined acids and bases this way: Arrhenius Acids form H+ in solution Arrhenius Bases form OH- in solution Bronsted and Lowry defined acids and bases this way: Bronsted-Lowry Acids donate an H+ in solution Bronsted-Lowry Bases accept an H+ in solution OR in more general terms: Lewis defined acids and bases this way: Lewis Acids are defined as: Electron pair acceptors Lewis Bases are defined as: Electron pair donors As the user above me has already stated, you can also measure its pH. pH measures the concentration of Hydronium ions in a solution (H3O+) (it is NOT H+; H+ does not really exist by itself in this form). pH measurements range from 0 to 14 at the temperature of 298 K (25 centigrade). IF: pH < 7, it is acidic. pH = 7, it is neutral; neither acidic nor basic pH > 7, it is basic.
