1. Write the balanced chemical equation:

ZnS(s) + 2HCl(aq) → ZnCl₂(aq) + H₂S(g)

2. Calculate the moles of zinc sulfide:

* Molar mass of ZnS = 65.38 g/mol (Zn) + 32.06 g/mol (S) = 97.44 g/mol

* Moles of ZnS = mass / molar mass = 45.5 g / 97.44 g/mol = 0.467 mol

3. Determine the moles of HCl needed:

* From the balanced equation, 1 mole of ZnS reacts with 2 moles of HCl.

* Moles of HCl = 0.467 mol ZnS * (2 mol HCl / 1 mol ZnS) = 0.934 mol HCl

4. Calculate the volume of HCl solution:

* Molarity (M) = moles of solute / volume of solution (in liters)

* Volume of HCl solution = moles of HCl / Molarity = 0.934 mol / 6.00 M = 0.156 L

5. Convert liters to milliliters:

* Volume of HCl solution = 0.156 L * 1000 mL/L = 156 mL

Therefore, you need 156 mL of a 6.00 M hydrochloric acid solution to completely react with 45.5 g of zinc sulfide.