There is no conjugate) base coupled to bromide, Br-, because this Br- can NOT donate (by protolysing) a proton (H+) in water.
However Br- itself is the very, very weakest base of the (very, very) strong conjugate acid HBr.
This is the only possible conjugate acid/base pair:
HBr/Br-
The conjugate base of HBr is Br-. It is formed when HBr loses a proton (H+).
The conjugate base of HBr is the bromide ion , Br-
Br^-
O2-
In the reaction, HBr donates a proton (H+) to H2O, making HBr the acid and H2O the base. The resulting products are Br- (conjugate base of HBr) and H3O+ (conjugate acid of H2O).
No, Br- is not an Arrhenius base. It is the conjugate base of hydrobromic acid (HBr) and would act as a base in a BrΓΈnsted-Lowry sense by accepting a proton.
The conjugate acid in the reaction is H3O+. It is formed when HBr donates a proton (H+) to water, resulting in the formation of the hydronium ion (H3O+).
No, Cl is not a stronger base than Br. In the periodic table, as you move down a group, basicity usually increases. Therefore, Br, being lower in the group than Cl, is a stronger base.
The conjugate base and conjugate acid for HS04 is: Conjugate acid is H2SO4 Conjugate base is SO42
No, Cl is not a stronger base than Br. In the periodic table, as you move down a group, basicity usually increases. Therefore, Br, being lower in the group than Cl, is a stronger base.
The conjugate acid for this anion is HBrO, or hypobromous acid. Finding the formula of a conjugate acid is simple actually. All you have to do is remove a negative charge and ad an "H" at the beginning.
HBr is not a weak base; it is a strong acid. In water, HBr completely dissociates into H+ and Br- ions, leading to a high concentration of H+ ions in solution. This strong acidity makes HBr a poor proton acceptor and hence not a base.
Acid + base conjugate base + conjugate acid
The conjugate base of NH3 is NH2-, formed by removing a proton (H+) from NH3.
The conjugate base and conjugate acid for HS04 is: Conjugate acid is H2SO4 Conjugate base is SO42
In the reaction, HBr donates a proton (H+) to H2O, making HBr the acid and H2O the base. The resulting products are Br- (conjugate base of HBr) and H3O+ (conjugate acid of H2O).
The conjugate base of H2O is OH-. When H2O loses a proton, it forms the hydroxide ion OH-, which is the conjugate base of water.
The conjugate acid in the reaction is H3O+. It is formed when HBr donates a proton (H+) to water, resulting in the formation of the hydronium ion (H3O+).
The conjugate base of H3PO4 is H2PO4-. The formula for the conjugate base can be found by removing one proton (H+) from the acid molecule.
PO43-
The conjugate base of H2SeO3 is HSeO3-. This is formed when H2SeO3 donates a proton (H+) in a reaction.