What species can be Brønsted-Lowry acids?
A Brønsted-Lowry acid is any species that can donate a proton, H+start text, H, end text, start superscript, plus, end superscript, and a base is any species that can accept a proton.
A Bronsted-Lowry base is any species that will increase the concentration of OH− in water. Hydroxide anion, OH− , fits this description by definition. So a Bronsted-Lowry base is by this definition a proton acceptor (from H2O ), that will increase the concentration of hydroxide anion, OH− , in water.
The Brønsted-Lowry Theory of Acids and Bases
Therefore, HCl is a Brønsted-Lowry acid (donates a proton) while the ammonia is a Brønsted-Lowry base (accepts a proton). Also, Cl- is called the conjugate base of the acid HCl and NH4+ is called the conjugate acid of the base NH3.
HCl(g) is the proton donor and therefore a Brønsted-Lowry acid, while H2O is the proton acceptor and a Brønsted-Lowry base.
Furthermore, because hydrofluoric acid, HF, loses a proton, H+1, to generate its conjugate in the reaction that is shown above, this reactant can be classified as a Brønsted-Lowry acid, and, consequently, the fluoride ion, F–1, is the conjugate base of this acid.
To determine whether a substance is an acid or a base, count the hydrogens on each substance before and after the reaction. If the number of hydrogens has decreased that substance is the acid (donates hydrogen ions). If the number of hydrogens has increased that substance is the base (accepts hydrogen ions).
Explanation: A Brønsted-Lowry base is a substance that behaves as a proton acceptor. The NH3 is accepting a proton from the HCl , so it is behaving as a Brønsted-Lowry base.
Because the water molecule donates a hydrogen ion to the ammonia, it is the Brønsted-Lowry acid, while the ammonia molecule—which accepts the hydrogen ion—is the Brønsted-Lowry base. Thus, ammonia acts as a base in both the Arrhenius sense and the Brønsted-Lowry sense.
In the reverse reaction, Cl¯ acts as a base and H3O+ acts as an acid. When HCl acts as an acid, it becomes Cl¯, which is a base and is called the conjugate base of HCl. When water acts as a base, it becomes H3O+, which is an acid and is called the conjugate acid of water.
Oxygen is another atom with lone pair electrons that can function as a Brønsted-Lowry base.
Is nh2 a Bronsted base or acid?
The NH 2 − ion (called the amide ion) is accepting the H + ion to become NH 3, so it is the Brønsted-Lowry base.
Bicarbonate(HCO3–) accepts the proton from HCl and forms conjugate acid(H2CO3). Hence, it is a Bronsted-Lowry base.
Ammonia, NH3, is a Lewis base and has a lone pair.
The bronsted lowry acid is the species which donates a proton H+ ion . Now, HSO4- is a base since it has the ability to accept a proton but it is a conjugate base to H2SO4 since it is formed by the H2SO4 after donating a proton.
Of the given substances: NH+4 N H 4 + is a Bronsted Lowry acid because it is rich in protons and can donate one to become a more stable... See full answer below.
The NH 2 − ion (called the amide ion) is accepting the H + ion to become NH 3, so it is the Brønsted-Lowry base.
As we already discussed, HNO3 is Bronsted-Lowry acid because it donates the proton when reacts with less acidic compounds than it such as H2O and forms the conjugate base. Therefore, HNO3 also acts as lewis acid.
Therefore, the sulfate ion (SO42−) is the conjugate base of HSO4− Was this answer helpful?
