A) HF < HCl < HBr < HI: increasing acidic strength
B) \[{{H}_{2}}O<{{H}_{2}}S<{{H}_{2}}Se<{{H}_{2}}Te:\] increasing \[p{{K}_{a}}\] values
C) \[N{{H}_{3}}<\text{ }P{{H}_{3}}<\text{ }As{{H}_{3}}<\text{ }Sb{{H}_{3}}:\]increasing acidic character
D) \[C{{O}_{2}}<Si{{O}_{2}}<Sn{{O}_{2}}<Pb{{O}_{2}}:\]increasing oxidizing power.
Correct Answer: B
Solution :
The acidic character of hydride increases down the group, so, \[p{{K}_{a}}\]decreases.
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