Answer
No precipitation will occur.
Work Step by Step
1. Find $[Ag^+]$
$[Ag^+] = [AgNO_3] = C_f$
$C_i * V_i = C_f * V_f$
$* V_f = 10ml + 100ml = 110ml$
$0.05 * 0.10 = C_f * 0.11$
$C_f = 0.0455 = [Ag^+]$
2. Find $[SO_4^{2-}]$:
$[SO_4^{2-}] = [Na_2SO_4] = C_f$
$0.05 * 0.01 = C_f * 0.11$
$C_f = 0.00455 M = [SO_4^2-]$
3. Calculate the product of the concentrations for $Ag_2SO_4$:
$P = [SO_4^{2-}][Ag^+]^2$
$P = 4.55 \times 10^{-3} * (4.55 \times 10^{-2})^2$
$P = 4.55 \times 10 ^{-3} * 2.070 \times 10^{-3}$
$P = 9.419 \times 10^{-6}$
4. Compare this product with the Ksp:
$Ksp (Ag_2SO_4)= 1.3 \times 10^{-5} $
$P = 9.419 \times 10^{-6}$
Since the Ksp value is higher, there will be no precipitations.