Q. \( \mathrm{CH_3COOH} \) strong or weak

Q: . Is \mathrm{CH_3COOH} a strong or weak acid?

\mathrm{CH_3COOH} is a weak acid. It partially ionizes in water to form \mathrm{H_3O^+} and \mathrm{CH_3COO^-} , but not completely.

Q: What is the dissociation equation for \mathrm{CH_3COOH} in water?

\mathrm{CH_3COOH + H_2O \rightarrow H_3O^+ + CH_3COO^-} . The key point is it does not go fully to completion, so it is weak.

Q: What \mathrm{p}K_a value suggests \mathrm{CH_3COOH} is weak?

Acetic acid has \mathrm{p}K_a \approx 4.76 . A higher \mathrm{p}K_a means weaker acidity, so \mathrm{CH_3COOH} is weak.

Q: How does \mathrm{CH_3COOH} compare to strong acids like \mathrm{HCl} ?

\mathrm{HCl} is strong and fully dissociates, while \mathrm{CH_3COOH} only partially dissociates. So \mathrm{CH_3COOH} produces fewer \mathrm{H_3O^+} ions at the same concentration.

Q: What does “weak acid” mean in terms of equilibrium?

Weak acids establish an equilibrium where some \mathrm{CH_3COOH} remains undissociated while some forms \mathrm{H_3O^+} and \mathrm{CH_3COO^-} .

Q: What common shortcut can identify \mathrm{CH_3COOH} as weak?

Most carboxylic acids like \mathrm{CH_3COOH} are weak. Strong acids are typically minerals such as \mathrm{HCl} , \mathrm{HBr} , \mathrm{HI} , \mathrm{H_2SO_4} , and \mathrm{HNO_3} .

Answer

Acetic acid, \( \mathrm{CH_3COOH} \), is a weak acid because it only partially ionizes in water. It does not fully dissociate like a strong acid.

Detailed Explanation

Problem: Is CH₃COOH (acetic acid) a strong or weak acid?

Step 1: Identify the compound

Acetic acid is

\( \mathrm{CH_3COOH} \)

. In aqueous solution, it can donate a proton (hydrogen ion) as follows:

\[ \mathrm{CH_3COOH \rightleftharpoons H^+ + CH_3COO^-} \]

This is a reversible (equilibrium) process, which is the key sign of a weak acid.

Step 2: Decide what “strong” versus “weak” means

A strong acid fully (or almost fully) dissociates in water, producing a large amount of ions. That means the equilibrium lies far to the right.

A weak acid only partially dissociates in water. That means the equilibrium does not go to completion; some acid remains undissociated.

Step 3: Use general chemistry classification knowledge

Acids like hydrochloric acid, nitric acid, and sulfuric acid are strong, but acetic acid is not one of the strong acids.

Acetic acid is a well-known weak acid and only partially ionizes in water.

Step 4: Final answer

\( \mathrm{CH_3COOH} \) is a weak acid.

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General Chemistry FAQs

. Is \( \mathrm{CH_3COOH} \) a strong or weak acid?

\( \mathrm{CH_3COOH} \) is a weak acid. It partially ionizes in water to form \( \mathrm{H_3O^+} \) and \( \mathrm{CH_3COO^-} \), but not completely.

What is the dissociation equation for \( \mathrm{CH_3COOH} \) in water?

\( \mathrm{CH_3COOH + H_2O \rightarrow H_3O^+ + CH_3COO^-} \). The key point is it does not go fully to completion, so it is weak.

What \( \mathrm{p}K_a \) value suggests \( \mathrm{CH_3COOH} \) is weak?

Acetic acid has \( \mathrm{p}K_a \approx 4.76 \). A higher \( \mathrm{p}K_a \) means weaker acidity, so \( \mathrm{CH_3COOH} \) is weak.

How does \( \mathrm{CH_3COOH} \) compare to strong acids like \( \mathrm{HCl} \)?

\( \mathrm{HCl} \) is strong and fully dissociates, while \( \mathrm{CH_3COOH} \) only partially dissociates. So \( \mathrm{CH_3COOH} \) produces fewer \( \mathrm{H_3O^+} \) ions at the same concentration.

Does the concentration of \( \mathrm{CH_3COOH} \) change whether it is weak or strong?

No. “Strong” or “weak” is about the extent of ionization as an acid type. Higher concentration changes \( \mathrm{[H_3O^+]} \), but \( \mathrm{CH_3COOH} \) remains weak.

What does “weak acid” mean in terms of equilibrium?

Weak acids establish an equilibrium where some \( \mathrm{CH_3COOH} \) remains undissociated while some forms \( \mathrm{H_3O^+} \) and \( \mathrm{CH_3COO^-} \).

What common shortcut can identify \( \mathrm{CH_3COOH} \) as weak?

Most carboxylic acids like \( \mathrm{CH_3COOH} \) are weak. Strong acids are typically minerals such as \( \mathrm{HCl} \), \( \mathrm{HBr} \), \( \mathrm{HI} \), \( \mathrm{H_2SO_4} \), and \( \mathrm{HNO_3} \).

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