To solve the problem of determining the new concentration of a 1.00 M ammonium chloride solution after dilution, follow these steps:
1. Identify the initial conditions:
- Initial volume (V_initial) of the ammonium chloride solution: 295 mL
- Initial molarity (M_initial) of the ammonium chloride solution: 1.00 M
2. Determine the volume of water added:
- Volume of water added (V_added): 2250 mL
3. Calculate the total final volume after dilution:
- The total final volume (V_final) is the sum of the initial volume of the solution and the volume of water added:
[tex]\[
V_{\text{final}} = V_{\text{initial}} + V_{\text{added}}
\][/tex]
[tex]\[
V_{\text{final}} = 295\ \text{mL} + 2250\ \text{mL}
\][/tex]
[tex]\[
V_{\text{final}} = 2545\ \text{mL}
\][/tex]
4. Use the dilution formula to find the new molarity:
- The dilution formula is expressed as:
[tex]\[
M_{\text{initial}} \times V_{\text{initial}} = M_{\text{final}} \times V_{\text{final}}
\][/tex]
- Rearranging to solve for the final molarity (M_final):
[tex]\[
M_{\text{final}} = \frac{M_{\text{initial}} \times V_{\text{initial}}}{V_{\text{final}}}
\][/tex]
5. Substitute the known values into the equation:
[tex]\[
M_{\text{final}} = \frac{1.00\ \text{M} \times 295\ \text{mL}}{2545\ \text{mL}}
\][/tex]
6. Calculate the final molarity:
[tex]\[
M_{\text{final}} \approx 0.11591355599214145\ \text{M}
\][/tex]
Therefore, the new concentration of the ammonium chloride solution after dilution is approximately [tex]\( 0.116 \)[/tex] M.
