Statement 1: Acid strength increases in the order given as `HFltltHClltltHBrltltHI`.
Statement 2: As the size of the elements `F,Cl,Br,I` increases down the group, the bond strength of `HF,HCl,HBr` and `HI` decreases and so the acid strength increases.
In the light of the above statements, choose the correct answer from the options given below:

Options

A. Statement 1 is Correct, Statement 2 is False.
B. Statement 1 is incorrect, Statement 2 is true.
C. Both Statement 1 and Statement 2 are true
D. Both Statement 1 and Statement 2 are false

Answer

To solve the question, we need to evaluate the two statements regarding the acid strength of the hydrogen halides (HF, HCl, HBr, and HI) and the relationship between bond strength and acid strength.

### Step-by-Step Solution:

1. **Understanding Acid Strength**:
- Acid strength is determined by the ability of the acid to dissociate and release H⁺ ions. A stronger acid will dissociate more readily.

2. **Analyzing Statement 1**:
- Statement 1 claims that the acid strength increases in the order: HF < HCl < HBr < HI.
- To evaluate this, we need to consider the bond strengths of the hydrogen halides.

3. **Bond Strength Consideration**:
- The bond strength of H-X (where X is a halogen) decreases as we move down the group in the periodic table. This is because the size of the halogen atoms increases, leading to longer and weaker bonds.
- Specifically, the bond strengths are approximately:
- HF has a strong bond due to the small size of F.
- HCl has a weaker bond than HF.
- HBr is weaker than HCl.
- HI has the weakest bond of all.

4. **Conclusion from Statement 1**:
- Since HF has the strongest bond, it is the weakest acid. Conversely, HI, with the weakest bond, is the strongest acid. Therefore, the order of acid strength is indeed HF < HCl < HBr < HI, confirming Statement 1 is true.

5. **Analyzing Statement 2**:
- Statement 2 explains that as the size of the halogen atoms (F, Cl, Br, I) increases down the group, the bond strength of HF, HCl, HBr, and HI decreases, leading to an increase in acid strength.
- This statement is also true because weaker bonds break more easily, allowing for easier dissociation of H⁺ ions.

6. **Final Evaluation**:
- Both statements are true, and Statement 1 is correctly supported by Statement 2. Therefore, the correct answer is that both statements are true.

### Final Answer:
- The correct option is **Option 3**: Both Statement 1 and Statement 2 are true.