In a solution containing `0.1M HCl & 0.1M H_(3)PO_(4)` (having dissociation constants `K_(a_(1)),K_(a_(2)),K_(a_(3)))` assuming `alphaltlt1` for `H_(3)PO_(4)`,

Options

A. `pH=1`
B. `alpha_(H_(3)PO_(4))=10K_(a_(1))`
C. `[HPO_(4)^(2-)]=10K_(a_(1))K_(a_(2))`
D. All of these

Explanation

To solve the problem, we need to analyze the dissociation of the acids in the solution containing 0.1 M HCl and 0.1 M H₃PO₄.

### Step-by-Step Solution:

1. **Understanding the Solution**:
- We have a solution containing 0.1 M HCl (a strong acid) and 0.1 M H₃PO₄ (a weak acid).
- HCl will completely dissociate in solution, contributing to the concentration of H⁺ ions.

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