Determine whether each pair is a conjugate acid-base pair. check all that apply. check all that apply. hcl, hbr nh3, nh+4 c2h3o−2, hc2h3o2 hco−3, no−3

            Following are the conjugate acid-base pairs;

            1)  NH₃  ,  NH₄⁺

            2)  CH₃CO₂⁻  ,  CH₃COOH

Explanation:
                   According to Brønsted–Lowry acid–base theory an acid is any specie which can donate H⁺. When an acid donates proton it is converted into conjugate base.

Example:
                     CH₃COOH  +  BASE    →    CH₃COO⁻  + Base-H

In above reaction Acetic Acid (CH₃COOH) is acid, and after loosing proton it is converted into conjugate base i.e. Acetate (CH₃COO⁻).

And according to Brønsted–Lowry acid–base theory base is any specie which can accept H⁺. When base accepts proton it is converted into conjugate acid.

Example:
                                 NH₃  +  A-H    →    NH₄⁺  + A⁻

In above reaction Ammonia (NH₃) is a base, and after accepting proton it is converted into conjugate acid i.e. Ammonium (NH₄⁺)

There is one s orbital, and there are three p orbitals, five d orbitals, and seven f orbitals. thus, the answer is b. do not confuse the number of orbitals in a subshell with the number of electrons the subshell can hold. each orbital can hold two electrons, so the capacity of an nf subshell is 14 electrons.

Hno3(aq) → h+(aq) + no3−(aq). picture ii best represents the strong acid hno3. strong acids are strong electrolytes