Question

An aqueous solution of $C{{H}_{3}}COONa$ is:
A. Acidic
B. Basic
C. Neutral
D. None of the above

Answer 1

Hint: Sodium acetate ($C{{H}_{3}}COONa$) is a salt formed as result of the neutralisation reaction between acetic acid ($C{{H}_{3}}COOH$) and sodium hydroxide (NaOH). Now that you know the reaction which results in the production of $C{{H}_{3}}COONa$ and the reactants involved in the procedure, you should be able to find out the nature of its acidic solution fairly easily.

Step-by-Step Solution:
Let us analyse Sodium Acetate as a compound first before we get on to the particulars of this question.
Sodium acetate ($C{{H}_{3}}COONa$) is a solid-state salt that cannot be used in anhydrous or liquid form as an acid or base. Now, with NaOH being a strong base and $C{{H}_{3}}COOH$ being a weak acid, the resulting solution is basic in nature. Sodium acetate is therefore basic in an aqueous medium.
Let us now observe the hydrolysis of $C{{H}_{3}}COONa$ which will help us understand the given solution better:

& C{{H}_{3}}COONa\text{ }\xrightarrow{\text{Ionisation}\text{ in aqueous solution}}CH3CO{{O}^{-}}_{strong\text{ }base}+N{{a}^{+}} \\\ & C{{H}_{3}}CO{{O}^{-}}+{{H}_{2}}O\to C{{H}_{3}}COOH+O{{H}^{-}} \\\ \end{aligned}$$ Acetate ion undergoes hydrolysis and the resulting solution is slightly basic due to excess of $O{{H}^{-}}$ ions. Therefore, through our detailed analysis and the accompanying thorough explanation, we can hereby conclude that the answer to this question is b) basic. Note: Just knowing the reactants required for the production of $C{{H}_{3}}COONa$ might be enough for you to guess the answer to this question. However, it is highly recommended that you be well-informed of the ionisation of $C{{H}_{3}}COONa$ in water that results in the alkaline nature of resultant solution.