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Do not be intimidated by this sort of question. All we are doing is taking the starting formula, #HX#, #H_2SO_4#, #HNO_3#, or even #HCO_3^-#, and removing a proton, #H^+#, to form the conjugate bases, #X^-#, #HSO_4^-#, #NO_3^-#, and #CO_3^(2-)# . As with all such chemical reactions, both MASS and CHARGE are conserved.
If I switch the solvent to ammonia, #NH_3#, rather than water, what is the conjugate base of ammonia in solvent of ammonia (i.e., here #NH_3# takes on the role of #H_2O#)? What is the conjugate acid? I could even switch the solvent to an acidic solvent such as #HF#, or #H_2SO_4#. What are the conjugate acids in these solvents?
