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Question

Consider the three solutions of 1M concentration
I) Sodium acetate (CH3COONa)
II) Acetic acid + sodium acetate (CH3COOH+CH3COONa)
III) Acetic acid (CH3COOH)
The pH of these solutions will lie in the following sequence

A
III<I<II
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B
III<II<I
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C
I<II<III
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D
II<I<III
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Solution

The correct option is B III<II<I
1) CH3COONa is formed by reaction of sodium hydroxide (NaOH) and acetic acid (CH3COOH). Acetic acid is a weak acid and sodium hydroxide is a strong base.
Thus, sodium acetate (CH3COONa) is basic in nature and thus pH will be greater than 7

2) When sodium acetate added to aq. solution of acetic acid which is acidic in nature, the concentration of H+ decreases, CH3COOH + CH3COONa will form an acidic buffer so it's pH<7 but greater than pH of CH3COOH

3) CH3COOH is a weak acid so its pH<7.

Hence, the correct option is III<II<I

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