The pH value of 0.1 M solutions of CH3COONa (I), CH3COOH (II), CH3 COONH4 (III),

step 1 Hello students. For this question we are given 0 .1m solution of the following compounds that is

The pH value of 0.1 M solutions of CH3COONa (I), ...

The pH value of $0.1 \mathrm{M}$ solutions of $\begin{array}{llll}\mathrm{CH}_{3} \mathrm{COONa} & \text { (I), } & \mathrm{CH}_{3} \mathrm{COOH} & \text { (II), }\end{array}$ $\mathrm{CH}_{3} \mathrm{COONH}_{4}$ (III), $\mathrm{NaOH}$ (IV) and $\mathrm{HCl}(\mathrm{V})$ is in the order (a) $\mathrm{I}<\mathrm{II}<\mathrm{III}<\mathrm{IV}<\mathrm{V}$ (b) $\mathrm{V}<\mathrm{IV}<\mathrm{III}<\mathrm{II}<\mathrm{I}$ (c) $\mathrm{V}<\mathrm{II}<\mathrm{III}<\mathrm{I}<\mathrm{IV}$ (d) $\mathrm{V}<\mathrm{II}<\mathrm{I}<\mathrm{III}<\mathrm{IV}$

The pH value of $0.1 \mathrm{M}$ solutions of $\begin{array}{llll}\mathrm{CH}_{3} \mathrm{COONa} & \text { (I), } & \mathrm{CH}_{3} \mathrm{COOH} & \text { (II), }\end{array}$
$\mathrm{CH}_{3} \mathrm{COONH}_{4}$ (III), $\mathrm{NaOH}$ (IV) and
$\mathrm{HCl}(\mathrm{V})$ is in the order
(a) $\mathrm{I}<\mathrm{II}<\mathrm{III}<\mathrm{IV}<\mathrm{V}$
(b) $\mathrm{V}<\mathrm{IV}<\mathrm{III}<\mathrm{II}<\mathrm{I}$
(c) $\mathrm{V}<\mathrm{II}<\mathrm{III}<\mathrm{I}<\mathrm{IV}$
(d) $\mathrm{V}<\mathrm{II}<\mathrm{I}<\mathrm{III}<\mathrm{IV}$

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

pH is the measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. It provides a scale, typically from 0 to 14, where values below 7 indicate acidic solutions, 7 is neutral, and values above 7 indicate basic solutions.

Strong Acids and Bases

Strong acids and bases are substances that completely dissociate into their ions in aqueous solution. Strong acids, such as HCl, release a high concentration of hydrogen ions leading to very low pH values, while strong bases, like NaOH, generate a high concentration of hydroxide ions resulting in high pH values.

Weak Acids

Weak acids only partially ionize in solution, meaning that not all acid molecules donate their hydrogen ions. This partial ionization is quantified by the acid dissociation constant (Ka), resulting in a pH that is less extreme than that of a strong acid at the same concentration.

Salt Hydrolysis

Salt hydrolysis occurs when an ion from a dissolved salt reacts with water to produce an acidic or basic solution. This reaction depends on the relative strengths of the acid and base from which the salt is formed, often leading to deviations in pH from neutral even when the original salt is derived from weak acids or bases.

Please give Ace some feedback