The solution you identified in question (1) acts as a buffer due to reactions that occur within the solution when an acid or a b

Question

3 years ago

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The solution you identified in question (1) acts as a buffer due to reactions that occur within the solution when an acid or a b

ase is added. Write the net ionic chemical equation for the reaction that occurs within this buffer solution when HCl(aq) is added. (Phase labels should be included in all net ionic chemical equations.)

Chemistry

1 answer:

weeeeeb [17] · Answer 1 · 2022-10-08T08:31:42+03:00

Answer:

The answer is " $\bold{CH_3COO^{-} \ (aq) + H^{+}\ (aq) \longrightarrow CH_3COOH \ (aq)}$ "

Explanation:

When $HCI$ is added in the chemical equation it reacts with sodium acetate so, it will give the following chemical equation:

$CH_3COONa\ (aq) + HCl\ (aq)\longrightarrow CH_3COOH\ (aq) + NaCl\ (aq)\\\\$

In this, the $CH_3COOH$ is a weak acid so, it not completely dissociated.

$CH_3COONa \ (aq) \ \ and \ NaCl$ were strong electrolytes they are completely dissociated.

The $HCl$ is a strong acid so, it is completely dissociated So, the net ionic equation is:

$CH_3COO^{-} \ (aq) + H^{+}\ (aq) \longrightarrow CH_3COOH \ (aq)$