To find the new concentration in molarity of the ammonium chloride (NH₄Cl) solution after dilution, we follow these steps:
1. Determine the initial volume in liters:
- The initial volume given is 295 mL.
- We convert this to liters:
[tex]\[
\text{Initial volume} = \frac{295 \text{ mL}}{1000} = 0.295 \text{ L}
\][/tex]
2. Calculate the total volume after dilution:
- An additional 2.25 L of water is added to the initial solution.
- So, the total volume is:
[tex]\[
\text{Total volume} = 0.295 \text{ L} + 2.25 \text{ L} = 2.545 \text{ L}
\][/tex]
3. Find the initial number of moles of NH₄Cl:
- The initial concentration of the solution is 1.00 M (molarity), which means there is 1 mole of NH₄Cl per liter of solution.
- Using the initial volume in liters (0.295 L):
[tex]\[
\text{Moles of NH₄Cl} = \text{Concentration} \times \text{Volume} = 1.00 \text{ M} \times 0.295 \text{ L} = 0.295 \text{ moles}
\][/tex]
4. Calculate the new concentration:
- After dilution, the number of moles of solute (NH₄Cl) remains the same, but the volume increases.
- The new concentration (Molarity) is given by the number of moles divided by the total volume in liters:
[tex]\[
\text{New concentration} = \frac{\text{Moles of NH₄Cl}}{\text{Total volume}} = \frac{0.295 \text{ moles}}{2.545 \text{ L}} \approx 0.116 \text{ M}
\][/tex]
Therefore, the new concentration of the diluted NH₄Cl solution is approximately [tex]\(0.116\)[/tex] M (molarity).
