The compound(s) with P-H bond(s) is(are)

The oxo-acids of phosphorus can be recognised from the general formula $$H_nP_mO_x$$ and by remembering that:

• Every hydrogen attached to oxygen appears as an $$-OH$$ group and is ionisable (acidic).
• Any hydrogen that is written directly next to phosphorus in the condensed formula is attached to phosphorus itself; that bond is a $$P-H$$ bond. Such hydrogens are non-ionisable and take part in reduction reactions.

Let us inspect each option.

Option A : $$H_3PO_4$$ (Orthophosphoric acid)
Expanded structure: $$\;HO-P(=O)(OH)_2$$.
All three hydrogens are bonded to oxygen as $$-OH$$ groups, so there is no $$P-H$$ bond in this molecule.

Option B : $$H_3PO_3$$ (Phosphorous acid)
The correct expanded formula is $$\;HP(=O)(OH)_2$$.
Here two hydrogens are bonded to oxygen ($$-OH$$ groups) and one hydrogen is directly attached to phosphorus. Therefore the molecule contains one $$P-H$$ bond.

Option C : $$H_4P_2O_7$$ (Pyrophosphoric acid)
This acid is obtained by condensation of two $$H_3PO_4$$ units: $$HO-P(=O)(OH)-O-P(=O)(OH)_2$$.
All four hydrogens appear in $$-OH$$ groups; again, no $$P-H$$ bond is present.

Option D : $$H_3PO_2$$ (Hypophosphorous acid)
Expanded structure: $$\;H_2P(=O)(OH)$$.
One hydrogen forms an $$-OH$$ group, while two hydrogens are directly attached to phosphorus. Thus the molecule contains two $$P-H$$ bonds.

Hence, the acids that contain at least one $$P-H$$ bond are:

Option B which is: $$H_3PO_3$$,
Option D which is: $$H_3PO_2$$.

All other options lack a $$P-H$$ bond.

Final answer: Option B (H$$_3$$PO$$_3$$), Option D (H$$_3$$PO$$_2$$)