$H_2S$ is less acidic than $H_2Te$. Why?

(N/A) The acidic character of hydrides of group $16$ elements depends on the bond dissociation enthalpy of the $E-H$ bond.
As we move down the group from $S$ to $Te$,the size of the central atom increases,which leads to an increase in the bond length.
Consequently,the $E-H$ bond dissociation enthalpy decreases down the group.
Since it becomes easier to break the $H-Te$ bond compared to the $H-S$ bond,$H_2Te$ is more acidic than $H_2S$.