It is a standard practice in textbook thermodynamics analyses to tacitly equip the surroundings with equipment that does not generate entropy during a process. One such piece of equipment is the so-called ideal constant temperature reservoir. The fluid in such a reservoir is assumed to have an infinite mass times heat capacity so that the temperature of the fluid remains virtually constant when it exchanges heat with the system. For such an ideal reservoir, the key operating characteristic is that its entropy change is equal to the heat it receives from the system $Q_{res}$ divided by its absolute temperature (irrespective of any irreversible entropy generation within the system):$$\Delta S_{res}=\frac{Q_{res}}{T_{res}}$$
The "ideal constant temperature reservoir" describes the limiting behavior of any finite thermal capacity reservoir, for which $$\Delta S=\int_{T_i}^{T_f}{mC\frac{dT}{T}}=mC\ln{(T_f/T_i)}$$ with $$Q=mC(T_f-T_i)$$where $T_i$ and $T_f$ are the temperatures in the initial and final thermodynamic equilibrium states of the reservoir and Q is the actual amount of heat received by the reservoir in the irreversible process.
If we combine these two equations, we obtain:
$$\Delta S=mC\ln{\left(1+\frac{Q}{mCT_i}\right)}$$In the limit of mC becoming infinite, this reduces to:$$\Delta S=\frac{Q}{T_i}$$
I should also mention that the fluid within the ideal constant temperature reservoir is assumed to have either an infinite thermal conductivity or is extremely well-mixed, such that the temperature throughout the reservoir is uniform spatially at $T_{res}$, including (and specifically) at the interface with the "system."
