Rank the following species in order of increasing acidity.

Step 1 of 3

According to Bronsted-Lowry acid base theory the compounds which have ability to donate proton or accepts electrons are known as Bronsted acid, and the compound that can donate electron or accepts protons are called as base.
All negative charged carrying species or p-electrons carrying species can behave as a base.
All positive charged carrying species or electron deficient species can heave as an acid.
The order of acidity can be explained by using the following points or the factor affecting acidity of compounds are as follows:

(i) Electronegativity: More the electronegativity of atom, attached from a compound more will be the acidity.

(ii) Electron withdrawing groups: If these types of groups are attached within conjugation in compound then they will increase the acidity, due to + I effect.

(iii) Electron donating groups: If these types of groups are attached within conjugation in compound then they will decrease the acidity, due to - I effect.

(iv) \(pk_a\) value: More the \(pk_a\) value of compound less will be the acidity.The pKa value table for the given compounds is shown below:

\(\begin{array}{|l|l|}
\hline \text { Compound } & \text { pKa } \\
\hline \mathrm{HF} & 3.17 \\
\mathrm{NH}_{3} & 33 \\
\mathrm{H}_{2} \mathrm{SO}_{4} & -5 \\
\mathrm{CH}_{3} \mathrm{OH} & 15.5 \\
\mathrm{CH}_{3} \mathrm{COOH} & 4.74 \\
\mathrm{H}_{3} \mathrm{O}^{+} & -1.7 \\
\mathrm{H}_{2} \mathrm{O} & 15.7 \\
\hline
\end{array}\)