Answer: 1) [tex]RCOO^-[/tex]
2) [tex]H_2PO_4^-[/tex]
3) [tex]RNH_2[/tex]
4) [tex]HCO_3^-[/tex]
Explanation:
According to the Bronsted-Lowry conjugate acid-base theory, an acid is defined as a substance which looses donates protons and thus forming conjugate base and a base is defined as a substance which accepts protons and thus forming conjugate acid.
1) [tex]RCOOH\rightarrow RCOO^-+H^+[/tex]
Here, [tex]RCOOH[/tex] is loosing a proton, thus it is considered as an acid and after losing a proton, it forms [tex]RCOO^-[/tex] which is a conjugate base.
2) [tex]H_3PO_4\rightarrow H_2PO_4^-+H^+[/tex]
Here, [tex]H_3PO_4[/tex] is loosing a proton, thus it is considered as an acid and after losing a proton, it forms [tex]H_2PO_4^-[/tex] which is a conjugate base.
3) [tex]RNH_3^+\rightarrow RNH_2+H^+[/tex]
Here, [tex]RNH_3^+[/tex] is loosing a proton, thus it is considered as an acid and after losing a proton, it forms [tex]RNH_2[/tex] which is a conjugate base.
4) [tex]H_2CO_3\rightarrow HCO_3^-+H^+[/tex]
Here, [tex]H_2CO_3[/tex] is loosing a proton, thus it is considered as an acid and after losing a proton, it forms [tex]HCO_3^-[/tex] which is a conjugate base.
