Solve How much ammonium chloride $\left({\mathrm{NH}}_4\mathrm{Cl}\right),$ in grams, is needed to produce2.5 $\mathrm{L}$ of a 0.5 $\mathrm{M}$ aqueous solution?

Step by Step Solution: Step 1. Using the formula: Molarity $(M)=\frac{moles}{volume(L)}$, calculate the number of moles of ammonium chloride required. Step 2. Rearrange the formula to get the number of moles required: Moles $=Molarity\times volume(L)$ Step 3. Substitute the values to get the moles of ammonium chloride required Step 4. Calculate the mass of ammonium chloride using the formula: $mass=moles\times molarmass$ Step 5. Look up the molar mass of ammonium chloride and substitute the previously calculated moles to find the mass of ammonium chloride required. Final Answer: 68.5 g