$1)$ $\mathrm{HF}<\mathrm{HCl}<\mathrm{HBr}<\mathrm{HI}$ bond strength decreases therefore, acidic strength increases.
$2)$ ${\mathrm{H}}_2\mathrm{O}<{\mathrm{H}}_2 \mathrm{S}<{\mathrm{H}}_2\mathrm{Se}<{\mathrm{H}}_2\mathrm{Te}$ from going down the group bond length increase so bond strength decreases therefore, acidic nature of these will increase but ${\mathrm{pK}}_{\mathrm{a}}$ will decrease.
So, this given order is wrong.
$3)$ ${\mathrm{NH}}_3<{\mathrm{PH}}_3<{\mathrm{AsH}}_3<{\mathrm{SbH}}_3$ from going down the group bond length increases, so bond strength decreases therefore, acidic nature of these will increase
$4)$ ${\mathrm{CO}}_2<{\mathrm{SiO}}_2<{\mathrm{SnO}}_2<{\mathrm{PbO}}_2$ From going down the group stability of higher oxidation state decreases due to inert pair effect therefore, their tendency to reduce will increase, so their oxidizing power will increase.