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Question: The increasing order of base strength of \[C{l^ - }C{H_3}CO{O^ - }\], \[^ - OH\] and \[{F^ - }\] is ...

The increasing order of base strength of Cl−CH3COO−C{l^ - }C{H_3}CO{O^ - }, −OH^ - OH and F−{F^ - } is
A.  Cl− < F− < CH3COO− <OH−A.\,\,C{l^ - }\, < \,{F^ - }\, < \,C{H_3}CO{O^ - }\, < O{H^ - }
B.  Cl− > F− > CH3COO− >OH−B.\,\,C{l^ - }\, > \,{F^ - }\, > \,C{H_3}CO{O^ - }\, > O{H^ - }
C.  CH3COO− < Cl− <  F− <OH−C.\,\,C{H_3}CO{O^ - }\, < \,C{l^ - }\, < \,\,{F^ - }\, < O{H^ - }
D.  None  of theseD.\,\,None\,\,of\,these

Explanation

Solution

Acids does the proton donation and base accepts the proton. The primary strength of any type is its ability to accept H+{H^ + } of another type. The greater the type's ability to accept H+{H^ + } of another species, the greater its fundamental strength. Organic chemists usually compare the strength of bases using the forces of their conjugate acids, measured in pKa. Example: Base strengths of F−{F^ - } and HS−H{S^ - }.

Complete step-by-step answer:
Conjugate acid of F− =  F− +  H+ =  HF{F^ - }\, = \,\,{F^ - }\, + \,\,{H^ + }\, = \,\,HF
pKa of HF = 3.17pKa{\text{ }}of{\text{ }}HF{\text{ }} = {\text{ }}3.17
Conjugate acid of HS− =  HS− +  H+ =  H2SH{S^ - }\, = \,\,H{S^ - }\, + \,\,{H^ + }\, = \,\,{H_2}S
pKa of H2S = 7.00pKa{\text{ }}of{\text{ }}{H_2}S{\text{ }} = {\text{ }}7.00
In this, the HFHF is a stronger acid than H2S{H_2}S. As there is the stronger acid, the weaker the conjugate base, and vice versa. Therefore, HS−H{S^ - } is a stronger base than F−{F^ - } .
The strong acid is a weak conjugate base and the strong base is a weak conjugate acid.

In the given options let's add the H+{H^ + } so that we can get the conjugate acid and let’s arrange in the increasing order of acidic strength.
H2O < CH3COOH < HF < HCl{H_2}O{\text{ }} < {\text{ }}C{H_3}COOH{\text{ }} < {\text{ }}HF{\text{ }} < {\text{ }}HCl
If we write the acidic strength in the opposite, it becomes the basic strength.
OH−> CH3COO−> F−> Cl−O{H^ - } > {\text{ }}C{H_3}CO{O^ - } > {\text{ }}{F^ - } > {\text{ }}C{l^ - }
So, the basic strength in the given option is;
A.  Cl− < F− < CH3COO− <OH−A.\,\,C{l^ - }\, < \,{F^ - }\, < \,C{H_3}CO{O^ - }\, < O{H^ - }

So, the correct answer is option A.

Note: Not all acids and bases ionize or dissociate to the same extent. This leads to the assertion that acids and bases are not all of the equal strength to produce H+{H^ + } and OH−O{H^ - } ions in solution. The terms "strong" and "weak" indicate the strength of an acid or a base. The terms strong and weak describe the ability of acidic and basic solutions to conduct electricity. If the acid or base strongly conducts electricity, it is a strong acid or base. When there is weak acid or base it conducts electricity weakly.