Assertion (A): The solubility of HCl in water does not follow Henry's law.
Reason (R): Henry's law is not applicable to polar substances.

Options

A. Both A and Rare true and R is the correct ex planation of A
B. Both A and Rare true but R is not the correct explanation of A
C. A is true but R is false
D. A is false but R is true

Explanation

To analyze the given assertion and reason, we will break down the concepts involved step by step.

### Step 1: Understand Henry's Law
Henry's Law states that the concentration of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. Mathematically, it can be expressed as:
\[ C = k_H \cdot P \]
where:
- \( C \) is the concentration of the gas in the solution,
- \( k_H \) is Henry's constant,
- \( P \) is the partial pressure of the gas.

**Hint:** Remember that Henry's Law applies to gases dissolving in liquids and is based on the idea of equilibrium between the gas phase and the dissolved phase.

### Step 2: Analyze the Assertion
The assertion states that "The solubility of HCl in water does not follow Henry's law."

When HCl is dissolved in water, it dissociates completely into H⁺ and Cl⁻ ions. This dissociation means that HCl behaves as a strong acid in solution, and its solubility cannot be accurately described by Henry's Law, which assumes that the gas remains undissociated.

**Hint:** Consider how the dissociation of HCl affects its behavior in solution compared to non-dissociating gases.

### Step 3: Analyze the Reason
The reason states that "Henry's law is not applicable to polar substances."

This statement is incorrect. Henry's Law is applicable to both polar and non-polar substances, as long as the gas does not dissociate in the solvent. The key point is that Henry's Law is not applicable when the solute (gas) undergoes a chemical reaction or dissociation in the solvent.

**Hint:** Think about the conditions under which Henry's Law holds true and whether it depends on the polarity of the substances involved.

### Step 4: Conclusion
- The assertion is correct: HCl does not follow Henry's Law due to its dissociation in water.
- The reason is incorrect: Henry's Law is applicable to both polar and non-polar gases, provided they do not dissociate.

Thus, the correct answer is that the assertion is true, and the reason is false.

**Final Answer:** The assertion is true, and the reason is false.