The standard electrode potential of Zn, Ag and Cu are -0.76 , 0.80...

Given standard reduction potentials:

$E^{{}^{\circ}}_{\text{Zn}^{2+}/\text{Zn}} = -0.76 \text{ V}$
$E^{{}^{\circ}}_{\text{Cu}^{2+}/\text{Cu}} = 0.34 \text{ V}$
$E^{{}^{\circ}}_{\text{Ag}^{+}/\text{Ag}} = 0.80 \text{ V}$

A species with a lower standard reduction potential acts as a stronger reducing agent. Since Zn has the lowest standard reduction potential among the given metals, it has the highest tendency to get oxidized.

Therefore, Zn acts as a strong reducing agent and can reduce both $\text{Ag}^{+}$ and $\text{Cu}^{2+}$ ions.

Answer: Zn can reduce $\text{Ag}^+$ and $\text{Cu}^{2+}$