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Arrhenius, Bronsted-Lowry, and Lewis theories of acids and bases
It had so many limitations which was found out by the later scientists; Bronsted and Lowry, who came up with their theories afterwards
Bronsted-Lowry
The Bronsted-Lowry definition describes acids as being proton (H+) donators and bases as being proton acceptors. So the answer would be C, because the carbonate anion is accepting a proton (H+ cation) to become the HCO3-
Bronsted and Lowry
Arrhenius, Bronsted-Lowry, and Lewis theories of acids and bases
It had so many limitations which was found out by the later scientists; Bronsted and Lowry, who came up with their theories afterwards
Bronsted-Lowry
The Bronsted-Lowry definition describes acids as being proton (H+) donators and bases as being proton acceptors. So the answer would be C, because the carbonate anion is accepting a proton (H+ cation) to become the HCO3-
1) Bronsted-Lowry acids are proton donors. Bronsted-Lowry bases are proton acceptors. 2) Lewis acids are electron acceptors. Lewis bases are electron donors.
Bronsted and Lowry
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.
1) Bronsted-Lowry acids are proton donors. Bronsted-Lowry bases are proton acceptors. 2) Lewis acids are electron acceptors. Lewis bases are electron donors.
According to Arrhenius, acids produce a proton in aqueous solution, and bases produce a hydroxide ion in aqueous solution. Hydrochloric acid is an Arrhenius acid because it gives up its proton as it dissolves in water. Sodium hydroxide is an Arrhenius base because it gives up its hydroxide as it dissolves in water.
Bronsted and Lowry.
The Arrhenius definition of acids and bases explains a number of things. Arrhenius's theory explains why all acids have similar properties to each other (and, conversely, why all bases are similar): because all acids release H+ into solution (and all bases release OH-). The Arrhenius definition also explains Boyle's observation that acids and bases counteract each other. This idea, that a base can make an acid weaker, and vice versa, is called neutralization. hope that helped
1) Bronsted-Lowry acids are proton donors. Bronsted-Lowry bases are proton acceptors. 2) Lewis acids are electron acceptors. Lewis bases are electron donors.