Step 1: Think in terms of the conjugate base:
When $\text{H}_2\text{E}$ loses a proton it forms $\text{HE}^-$. The larger the atom E, the more the negative charge spreads over a big volume, so the ion is more stable.
Step 2: Rank the conjugate bases:
Stability of $\text{HE}^-$ rises as $\text{OH}^- < \text{SH}^- < \text{SeH}^- < \text{TeH}^-$. A more stable conjugate base means a stronger parent acid.
Step 3: Conclude:
$\text{H}_2\text{Te}$ has the most stable conjugate base and the weakest H-Te bond, so it is the most acidic. Its dissociation constant is the largest of the four.
Final Answer:
Because the H-Te bond is the weakest, $\text{H}_2\text{Te}$ is the strongest acid.
\[ \boxed{\text{(D) }\text{H}_2\text{Te}} \]