0.01 moles of a weak acid HA () is dissolved in 1.0 L of 0.1 M HCl solution. The degree of dissociation of HA is (Round off to Nearest Integer).

[Neglect volume change on adding HA; assume degree of

Question

0.01 moles of a weak acid HA () is dissolved in 1.0 L of 0.1 M HCl solution. The degree of dissociation of HA is  (Round off to Nearest Integer).

[Neglect volume change on adding HA; assume degree of dissociation ]

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Step 1 — Set up equilibrium:

In 0.1 M HCl solution,  M (from HCl, strong acid)

Step 2 — ICE table (initial [HA] = 0.01 M):

| | HA | H⁺ | A⁻ |
|--|--|--|--|
| Initial | 0.01 | 0.1 | 0 |
| Change |  |  |  |
| Equil. |  |  |  |

Step 3 — Apply approximation ( and ):

Step 4 — Degree of dissociation:

Expressed as :

Answer: 2

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